Pretty Much Everything...

How many liters of a 0.75 M solution of Ca(NO3)2 will be required to react with 148 g of Na2CO3? Ca(NO3)2 + Na2CO3 --> CaCO3 + 2 NaNO3

(148 g Na2CO3) / (105.9884 g Na2CO3/mol) x (1 mol Ca(NO3)2 / 1 mol Na2CO3) / (0.75 mol/L Ca(NO3)2) = 1.86 L Ca(NO3)2

What is the freezing point of a solution of sugar dissolved in water if the concentration of the solution is 0.24 m?

-.446

What is the freezing point of a solution that contains 68.4 g of sucrose, C12H22O11, dissolved in 100 ml of water?

-3.72

If 7 L of a gas at 45.0°C is cooled until its volume decreases to 5.17 L, what is the temperature of the gas in degrees Celsius

-38 C

How many moles are in 1.31 x 1023 molecules of C6H14?

.218

How many moles are in 1.31 x 1023 molecules of C6H14?

.218 moles

A 5.00 L sample of helium at STP expands to 20.0 L. What is the new pressure on the gas?

.25 atm

A 5.00 L sample of helium at STP expands to 15.0 L. What is the new pressure on the gas?

.33 atm

45.0 g of Ca(NO3)2 was used to create a 0.80 M solution. What is the volume of the solution?

.34 L

How many moles are in 2.62 x 1023 molecules of C6H14?

.435 moles

A 10.00 L sample of helium at STP expands to 20.0 L. What is the new pressure on the gas?

.50 atm

A 10.00 L sample of helium at STP expands to 15.0 L. What is the new pressure on the gas?

.66 atm

12 L sample of gas is determined to contain 0.5 moles of nitrogen. At the same temperature and pressure, how many moles of gas would there be in a 20 L sample?

.83 moles

What is the freezing point depression when sugar is dissolved in water to make a 0.50 molal solution?

.93 degrees

R in the ideal gas law changes values. The value used depends on the pressure unit used in the problem. What is the value for R when the unit for pressure is atm?

0.0821

A sugar water solution has a freezing point of - 0.23oC. What is the molal concentration of the solution?

0.124 molal

How many moles of Ca(NO3)2 are there in 500 mL of 0.25 M solution?.

0.125 mol

Technetium-99 has a half-life of 6 hours. Starting with 200 grams, how much remains in 60 hours? (Round to 3 places)

0.195 grams

How many moles of Fe2O3 are necessary to produce 0.824 mol of CO2? Fe2 O3(s) + 3CO (g) --> 2Fe(s) + 3CO2 (g)

0.275 mol

0.550 moles of NaCl are dissolved in 1.95 L of water. Calculate the molarity of the NaCl solution.

0.282 M

How many kilograms are in 3.492 moles of baking soda (NaCHO3)?

0.2933

What is the molality of a solution prepared by dissolving 0.40 mol into 2.0 kg of solvent?

0.2m

The half-life of Radium-226 is 1,600 years. Starting with 5 grams, how much is left in 6,400 years?

0.3125 grams

4.78 psi = ______ atm.

0.325 atm

How many kilograms are in 6.983 moles of baking soda (NaCHO3)?

0.4749

2NO(g) + O2 (g) --> 2NO2 How many moles of O2 are required to produce 46.0 g NO2?

0.500 mol

2.0 L of a 1.5 M solution is diluted with water until the final volume is 6.0 L. The molarity of the solution is now _____.

0.50m

Find the density of the gas sulfur dioxide at 420K and 29.9 kPa.

0.549 g/L

Fluorine gas reacts with a solution of sodium bromide in a single-replacement producing aqueous sodium fluoride and bromine gas. If a reaction starts with 0.480 mol fluorine gas, how many moles of sodium fluoride are produced?

0.960 mol

How many ionizable hydrogen atoms are present in the CH3COOH molecule?

1

What are the pressure and the temperature of the normal melting point of ice?

1 atm and 0.00°C

Which of these conditions of temperature and pressure exist when ice melts at its normal melting point?

1 atm and 0°C

Calculate the density of SO3 gas at STP.

1 mole= 22.4 L molar mass= 80.1 g/mol P= M/V = 80.1g/22.42= 3.58 g/L

In quantum numbers, orientation is represented by

1,3,5,7

Balance the following redox reaction. 1. S + Cl2 → SCl6 2. Cu + AgNO3 --> Cu(NO3)2 + Ag 3. Al + F2 → AlF3 4. H2 + F2 → HF 5. CO + Fe2O3 → Fe + CO2

1. 3Cl2 + S → SCl6 2. 2AgNO3 + Cu → 2Ag + Cu(NO3)2 3. 3F2 + 2Al → 2AlF3 4. H2 + F2 → 2HF 5. 3CO + Fe2O3 → 3CO2 + 2Fe

Balance the following redox reaction. 1. NH3 + O2 → NO + H2O 2. Cr3+ + ClO3- → CrO42- + Cl- 3. Al + Fe2O3 --> Al2O3 + Fe 4. Al + Fe(NO3)2 --> Al(NO3)3 + Fe 5. Fe + ZnCl2 --> FeCl3 + Zn

1. 4NH3 + 5O2 → 4NO + 6H2O 2. 2Cr3+ + ClO3- + 10OH- → 2CrO42- + Cl- + 5H2O 3. 2Al + Fe2O3 → Al2O3 + 2Fe 4. 3Fe(NO3)2 + 2Al → 3Fe + 2Al(NO3)3 5. 3ZnCl2 + 2Fe → 3Zn + 2FeCl3

In the reaction below and state what is being oxidized and what is being reduced. 1. K + Cl2 → KCl 2. N2 + H2 → NH3 3. SO2 + O2 → SO3

1. Cl- reduced K- oxidized Cl2 + 2K <---->2KCl 2. N- reduced H- oxidized 3H2 + N2 <---> 2NH3 3. O- reduced S- Oxidized 2SO2 + O2 <--->2SO3

In the reaction below state what is being oxidized and what is being reduced. 1. 4 Fe + 3 O 2 → 2 Fe 2 O 3 2. Mg + N2 → Mg3 N2

1. O- reduced Fe- oxidized 4Fe + 3O2 <---> 2Fe2O3 2. N- reduced Mg- oxidized N2 + 3Mg <---->Mg3N2

Name the following compound: 1. CH3CH2CH2CH3 2. CH3CH2CH3 3. CH3CH2CH2CH2CH3 4. CH4 5. CH3CH2CH2CH2CH2CH3

1. butane 2. propane 3. pentane 4. methane 5. hexane

Match the wavelength with its application. 1. radio 2. microwave 3. infrared 4.visible 5. ultraviolet 6. x-ray 7. gamma ray

1. the longest of the waves 2. used for radar 3. gives off heat 4. the color we see 5. used for sterilzation 6. used for medical imaging 7. extremely dangerous for life

State the oxidation number for each element. 1. O2 2. Ag2S 3. HNO2 4. SnCl4 5. N2H4 6. S8 7. SnO 8. Al2O3

1. zero 2. Ag= +1 S= -2 3. H= +2 N= +5 O= -2 (3/10 points) 4. Sn= +4 Cl= -1 5. NOT N= -2 H= +1 6. zero 7. Sn= +2 O= -2 8. Al= +3 O= -2

The value of Kw at 25°C is _____.

1.0 × 10^-14

The concentration of hydrogen ions in a certain aqueous solution is 1.0 × 10−4 M. Calculate the concentration of the hydroxide ion

1.0 × 10−10 M

What is the [H+] in a solution with a pH 8.96?

1.1 x × 10^−9 M

How many carbon atoms are present in 0.92 moles of C2H6O?

1.11 x 1024 atoms

What is the molality of a solution prepared by dissolving 317 g of CaCl2 into 2.50 kg of water?

1.14 m

How many molecules are in 1.95 moles of water?

1.15 x 1023 molecules

Calculate the hydroxide ion concentration in an 8.6 × 10−5 M solution of HCl.

1.2 x 10^-10

How many moles are in 20.50 grams of NH3?

1.204 moles

The half-life of Radium-226 is 1,600 years. Starting with 5 grams, how much is left in 3200 years?

1.25 grams

The isotope Sodium-24 has a half-life of 15 hours. Starting with 22 grams, how much remains in 60 hours?

1.375 grams

15 g of NaCl occupy a volume of 175 mL. What is the molarity of the solution?

1.5 M

An oxygen gas tank holds 1 mole of gas at 10. atm pressure. In order to reduce the pressure of the tank to 2.5 atm particles must be released. How many particles will be left?

1.5 x 1023

A 7.00 L sample of helium expands to 15.0 L at which point the pressure is measured to be 0.720 atm. What was the original pressure of the gas?

1.54 atm

B2O3(s) + 3C(s) + 3Cl2 (g) ---> 2 BCl3(g) + 3CO(g) Calculate how many moles of BCl3 are produced from the reaction of 61.0g of B203?

1.75 mol

2Na(s) + 2 H2O(l) --> 2 NaOH (aq) + H2(g) A reaction produces 0.674 L of hydrogen gas at 601 mm Hg and 14°C. What mass of sodium hydroxide is produced in the reaction?

1.81 g NaOH

N2 (g) + 3 H2 (g)--> 2 NH3 (g) Calculate the volume of ammonia produced at 67°C and 3.49 atm from the complete reaction of 3.48 g of nitrogen with excess hydrogen.

1.99 L NH3

An isotope, Cesium-137, has a half-life of 30 years. Starting with 40 grams. How much is left in 60 years?

10 grams

A 75.0 liter container is filled with 59.3 grams of argon. How many grams of argon are released if the volume of the gas is reduced to 61.8 L.

10.4 gNe

What is the boiling point of a solution of ethanol, C2H5OH and sugar that contains 20.0 g of the sugar in 250 g of water?

100.89 C

Find the total pressure of a mixture of hydrogen and nitrogen gases that is present in a container. The partial pressure of the hydrogen is 34.0 kPa, while the partial pressure of the nitrogen is 67.0 kPa.

101 kPa

___ kPa = 14.7 psi

101.3 kPa

What are the pressure and the temperature of the normal boiling point of water?

101.3 kPa and 100.00°C

1.33 atm = ______ mm Hg.

1010 mm Hg

A rigid tank holds a 2.91 moles of gas at a pressure of 772 kPa. What will the pressure be if another 1.09 moles of gas is added?

1060 kPa

B2O3(s) + 3C(s) + 3Cl2 (g) ---> 2 BCl3(g) + 3CO(g) What is the mass of carbon required in order to produce 6.00 mol BCl3

108 g

The solubility of sodium carbonate is 21.5 g per 100 mL of water at 20°C. How much sodium carbonate is capable of dissolving in 500 mL of water at 20°C?

108g

What is the volume of gas at 2.00 atm and 200.0 K if its original volume was 300. L at STP?

109 .9 L

What is the percent composition of hydrogen found in H2O?

11.2%

2 NO(g) + O2 (g) --> 2 NO2 (g) What mass of NO2 is produced by the reaction of 2.40 mol NO with excess oxygen?

110 g

Find the total pressure of a mixture of hydrogen and nitrogen gases that is present in a container. The partial pressure of the hydrogen is 54.0 kPa, while the partial pressure of the nitrogen is 63.0 kPa.

117 kPa

Calculate the mass of oxygen in 250 g of Al(C2H3O2)3

117.5 grams

Calculate the mass of oxygen in 50 g of Ba(C2H3O2)2

12.55 grams

A gas sample in a rigid container at 455 K is brought to STP (273K and 1 atm). What was the original pressure of the gas in mmHg?

1270 mm Hg

Find the percent composition of water in barium chloride dihydrate

14.7%

What is the empirical formula mass (EFM) of P2O5?

141.94 g/mol

To what temperature does 436 mL of hydrogen originally at 25.0°C need to be heated in order to bring the volume to 2.5 L?

1436 C

If I add 15 grams of sodium chloride to 250 grams of water, what will the melting and boiling points be of the resulting solution? Use the data table in the reading to find the k values.

15/265 x 100= 5.66

How many grams are in 10.19 moles of Al2S3?

1530 grams

An 11.0 liter container is filled with 0.178 mol of gas. If 0.094 moles of gas are added, what is the new volume?

16.8 L

The molar mass of H20 is _______ grams per mole.

18.01

How many moles are in 1.16 x 1025 atoms of H2CO3?

19.27 moles of H2CO3

How many moles are in 1.16 x 1025 atoms of H2CO3?

19.3 moles of H2CO3

Calculate the mass of carbon in 250 g C2H6

199.72 grams

When the equation below is balanced using the smallest whole number coefficients, what is the coefficient in front of C3H8? C3H8 + O2→ H2O + CO2

2

Identify the balanced decomposition reaction for silver oxide?

2 Ag2O (s) --->4 Ag (s) + O2 (g)

Which of the following is the balanced single replacement reaction that occurs when aluminum metal replaces copper in a solution of copper(II) nitrate?

2 Al (s) + 3Cu (NO3)2 (aq) --> 2 Al(NO3)3(aq) + 3Cu(s)

For the following equations, which is NOT a valid mole ratio? 2SO3(g) --> 2SO2(g) + O2(g)

2 mol O2/ 2 mol SO3

How many moles are in 34 grams of NH3?

2 moles

A 5.00 L sample of helium expands to 15.0 L at which point the pressure is measured to be 0.720 atm. What was the original pressure of the gas?

2.16 atm

How many moles are there in 1.3 x 1024 atoms of Calcium?

2.16 moles

B2O3(s) + 3C(s) + 3Cl2 (g) ---> 2 BCl3(g) + 3CO(g) How many moles of chlorine are used up in a reaction that produced 175 g of BCl3?

2.24 mol

How many molecules are in 3.9 moles of water?

2.3 x 1024 molecules of water

Mercury-197 has a half life of 3 days. Starting with 300 grams, how much remains in 3 weeks? (Round to two places)

2.34 grams

The pressure in a car tire is 35 psi. Convert this to atmospheres (atm)

2.4 atm

Fe2O3(s)+3CO(g)⟶2Fe(s)+3CO2(g) A certain reaction produced 7.40 mol carbon dioxide. How many moles of both Fe2O3 and CO reacted?

2.47 mol Fe2O3 7.40 mol CO

N2 (g) + 3H2 (g) -->2 NH3 (g) The equation above is the equation for the Haber process. In a certain reaction, you start with 6.0 moles of nitrogen and 10.0 moles of hydrogen. How much of the excess reactant will be left over after the reaction?

2.6 mol

The isotope Sodium-24 has a half-life of 15 hours. Starting with 22 grams, how much remains in 45 hours?

2.75 grams

How many molecules are in 15 grams of Oxygen gas?

2.8 x 10 23 molecules of O2

Calculate the hydrogen ion concentration in a 3.4 × 10−3 M solution of KOH.

2.9 x 10^-12

An isotope, Cesium-137, has a half-life of 30 years. Starting with 40 grams, How much is left in 30 years?

20 grams

A noble gas is placed in a 10.0 liter container. The noble gas has a mass of 25.25 g, the pressure is 3.05 atm, and the temperature is 24°C. Find the molar mass and symbol for the gas.

20.2 g/mol; Ne

Calculate the mass of hydrogen in 500 g of Al(C2H3O2)3

22.2 grams

What volume does 1 mole of neon gas occupy at STP?

22.4 L

4 N H 3 ( g ) + 5 O 2 ( g ) ⟶ 4 N O ( g ) + 6 H 2 O ( g ) In a reaction that produced 34.8 L of water vapor, what volumes of ammonia and oxygen were consumed?

23.2 L NH3; 29 L O2

What is the melting point of a solution in which 2.5 grams of sodium chloride is added to 230 mL of water?

230+2.5g 2.5/232.5 X 100%= 23.2

Find the mass of carbon dioxide gas in a volume of 81.3 L at 204 kPa and a temperature of 368 K.

239 g CO2

Use the reaction below for the decomposition of sodium azide to sodium metal and nitrogen gas. to answer the question 2NaN3(s) --> 2 Na(s) + 3N2 (g) In a certain reaction, 675 g of NaN3 decomposes. Calculate the mass of sodium produced and the volume of nitrogen produced at STP.

239 g Na; 349 L N2

Find the percent composition of water in calcium chloride dihydrate

24.5%

What is the percent composition of magnesium in MgCl2?

25.53%

The most highly concentrated hydrochloric acid is 12 M. What volume of a 12 M stock solution of HCl should be diluted in order to produce 6.0 L of 0.50 M HCl?

250 ml

A rigid container of hydrogen gas at −104°C and 71.8 kPa is heated until the pressure reaches 2.23 atm. What is the temperature of the hydrogen in degrees Celsius?

259°C

How many grams are in 1.5 moles of water?

27 grams

To what temperature does 1.36 L of hydrogen originally at 25.0°C need to be heated in order to bring the volume to 2.5 L?

274.8C

Identify the spectator ion(s) in the ionic equation below. 2K+ (aq) +CO32- (aq)+Ba2+ (aq)+2NO3- (aq)→2K+ (aq) +2NO3- (aq)+BaCO3 (s)

2K+; 2NO3-

. Which of the equations is the reverse reaction of N2(g) + 3 H2(g) --> 2NH3 (g)

2NH3(g) → N2(g) + 3H2(g)

Which of the following is the balanced double replacement reaction that occurs when aqueous sodium hydroxide reacts with aqueous strontium chloride, producing a precipitate of strontium hydroxide?

2NaOH (aq) + SrCl2 (aq) --> 2NaCl (aq) + Sr(OH)2 (s)

Which of the following is the balanced single replacement reaction that occurs when rubidium reacts with water?

2Rb(s) + 2 H2O(l) ---> 2RbOH(aq) + H2 (g)

In a certain reaction, 5.0 moles of hydrogen is reacted with excess nitrogen. To determine how many moles of ammonia are produced, what conversion factor should be used. N2(g) + 3H2 (g) ---> 2NH3 (g)

2mol NH3/ 3mol H2 and 3mol H2/ 2mol NH3

What volume of a .20 M H3PO4 is needed to react with 100 mL of .1 M NaOH? H3PO4 + 3 NaOH --> Na3PO4 + 3 H2O

3 X 0.20M= .6M 0.010 moles NaOH 0.00333 moles H3PO4 0.00333/0.20= 16.65

How many moles are in 132.3 grams of carbon dioxide?

3.006 moles

What is the mass of 34.8 L of H2 gas at STP?

3.11 g

How many moles of ammonia are produced when 5 moles of hydrogen reacts with excess nitrogen? N2 (g) + 3H2(g) --> 2NH3 (g)

3.3 mol

N2 (g) + 3H2 (g) -->2 NH3 (g) The equation above is the equation for the Haber process. In a certain reaction, you start with 3.0 moles of nitrogen and 5.0 moles of hydrogen,. How many moles of ammonia will be produced in the reaction?

3.3 mol

Calculate the [OH−] in a solution with a pH of 12.52.

3.31 × 10−2 M

2Na(s) + 2 H2O(l) --> 2 NaOH (aq) + H2(g) At a pressure of 88.9 kPa and a temperature of 34 degrees C, how many liters of hydrogen are produced when 5.94 g of sodium reacts with excess water?

3.71 L H2

What is the percent composition of nitrogen in N2S2?

30.4%

2NO(g) + O2 (g) --> 2NO2 How many grams of NO are required to react fully with 5.00 mol of O2?

300. g

42.8 kPa = _____ mm Hg

321 mm Hg

Calculate the mass of aluminum in 250 g of Al(C2H3O2)3

33.05 grams

4 Fe(s) + 3O2(g) -->2Fe2O3(g) In a certain reaction, 27.3 g of iron is reacted with 45.8 g of Oxygen How many grams of the excess reactant remain after the reaction is complete

34.1g

How many grams of aluminum are required to react with 35 mL of 2.0 M hydrochloric acid, HCl? 6 HCl + 2 Al --> 2 AlCl3 + 3 H2

35 mL x (1 L / 1000 mL ) = .035 L 57.14286 moles HCl x (2 moles Al / 6 moles HCl) = 19.04762 moles of Al 19.04762 moles of Alx 26.982 grams per mole of Al = 513.94288, or 5.1394288 x 10^2 2.0 M = X/.035 L X = .070 moles of HCl 0.70 moles HCI x (2mol Al/6 mol HCI) (26.98Al/ 1 mol Al) = .63g Al

How many moles are in 2.32 x 1025 atoms of H2CO3?

38.6 moles of H2CO3

4 Fe(s) + 3O2(g) -->2Fe2O3(g) In Certain reaction, 27.3 g of iron is reacted with 45.8 g of Oxygen How many grams of Iron (III) oxide are produced in the reaction?

39.0g

Which of the following is the balanced double replacement reaction that occurs when an aqueous solution of copper(II) nitrate combines with an aqueous potassium phosphate?

3Cu(NO3)2(aq) + 2K3PO4(aq) --> Cu3(PO4)2(s) +6KNO3 (aq)

Which of the following is the balanced double replacement reaction that occurs when an aqueous solution of nickel (II) nitrate combines with an aqueous lithium phosphate?

3Ni(NO3)2(aq) + 2Li3PO4(aq) --> Ni3(PO4)2(s) +6LiNO3 (aq)

A certain colored light has a frequency of about 7.5 x 10^14Hz. What is the wavelength? Please upload your work, showing all three steps with your answer.Please show your work along with the final answer.

4.0 x 10^2nm C = 3.00 x 10^8 m/s y = ? v = 7.5 x 1014Hz 7.5 x 1014Hz x (1m/10^9) = 7.6 x 10^-6 y = (3.00 x 10^8 m/s) / (7.6 x 10^-6) y = 3.94 x 10^13

2HgO(s) --> 2Hg(l) + O2 (g) In a certain reaction 4.37 of HgO is decomposed, producing 3.21 of Hg What is the theoretical yield of Hg?

4.05g

B2O3(s) + 3C(s) + 3Cl2 (g) ---> 2 BCl3(g) + 3CO(g) How many moles of chlorine are used up in a reaction that produced 0.35 kg of BCl3?

4.48 mol

How many moles of carbon are used up in a reaction that produced 0.35 kg of BCl3? B2O3(s) + 3C(s) + 3Cl2 (g) ---> 2 BCl3(g) + 3CO(g)

4.48 moles

The pH of a certain solution is 11.49. The pOH of this solution is _____.

4.49

What is the pH of a solution that has a [H+] of 1.5 × 10−5 M?

4.8

A certain reaction produced 14.80 mol carbon dioxide. How many moles of both Fe2O3 and CO reacted? FeO3(s) + 3CO(g) --> 2Fe(s) + 3CO2(g)

4.933 mol Fe2O3 ; 14.80 mol Co

How many moles are in 4.24kg of Na2CO3?

40.0 moles

To make 1.00 L of 1.00 M NaOH solution, what mass of NaOH needs to be weighed out?

40.0g

What is the percent composition of nitrogen in (NH4)2S?

41.1%

The molar mass of LiCl is ______ grams per mole

42.39

What is the molar mass of .204 L of gas at STP, if the gas has a mass of 0.400 g?

43.9 g/mol

Use the reaction below for the decomposition of sodium azide to sodium metal and nitrogen gas. to answer the question 2NaN3(s) --> 2 Na(s) + 3N2 (g) What volume of nitrogen at STP is generated by the decomposition of 86.7 g NaN3?

44.8 L N2

Which of the following is the balanced synthesis equation if silver has a charge of +1?

4Ag + O2 → 2Ag2O

Which of the following is the balanced synthesis equation if copper has a charge of +1?

4Cu + O2 → 2Cu2O

Which of the following is the balanced synthesis equation if mercury has a charge of +1?

4Hg + O2 → 2Hg2O

An isotope, Cesium-137, has a half-life of 30 years. Starting with 40 grams. How much is left in 90 years?

5 grams

2 L sample of gas is determined to contain 0.5 moles of nitrogen. At the same temperature and pressure, how many moles of gas would there be in a 20 L sample?

5 moles

What is the percent by volume of a solution prepared by adding water to 30.0 mL of isopropyl alcohol until the volume if the solution is 600. mL?

5.00 %

The isotope Sodium-24 has a half-life of 15 hours. Starting with 22 grams, how much remains in 30 hours?

5.5 grams

How many carbon atoms are present in 0.46 moles of C2H6O?

5.5 x10 23 carbon atoms

The wavelength of green light is 522 nm, what is the frequency of the this radiation?

5.75 x10^14 1/s(Hz)

How many molecules are in .975 moles of water?

5.85 x 1022 molecules

What volume of a 40.0 % by volume acetone solution can be made with 20.0 mL of acetone?

50.0 ml

How many grams are in 3.396 moles of Al2S3?

509.9 grams

Find the pressure in mm Hg of 2.76 g of oxygen gas in a 250. mL container when the temperature is −26°C.

5310 mm Hg

B2O3(s) + 3C(s) + 3Cl2 (g) ---> 2 BCl3(g) + 3CO(g) What is the mass of carbon required in order to produce 3.00 mol BCl3

54 g

If 5.24 L of a gas at 5.0°C is warmed until its volume increases to 6.17 L, what is the temperature of the gas in degrees Celsius?

54.3 C

Ga2O3(s) + 3SOCl2(l) --> 2GaCl3(s) +3SO2 In a certain reaction, 35.9 g of Ga2O3 is reacted with 55.4 g SOCl2.The GaCl3 produced is collected and its mass founded to be 48.83 g. What is the theoretical yield of GaCl3

54.7 g

Find the volume needed to hold 2.33 moles of gas at 0.953 atm and 2.50°C?

55.2 L

The molar mass of NaCl is ______ grams per mole

58.44

How many grams of sodium can be reacted with 750 mL of a 6.0 M solution of sulfuric acid, H2SO4 ? Na + H2SO4 --> NaSO4 + H2

6 mol x 0.75= 4.5 moles 2 x 4.5= 9 moles Na is 22.99g/mol 9 x 22.99g = 210g

Which is the largest number of moles?

6.00 g He

N2 (g) + 3H2 (g) -->2 NH3 (g) The equation above is the equation for the Haber process. If 2.0 moles of nitrogen are available for a reaction, what amount of hydrogen represents the correct stoichiometric ratio?

6.0mol

A 25.5 liter container is filled with .950 moles of neon. How many grams of neon are released if the volume of the gas is reduced to 17.3 L?

6.16 g Ne

What is the percent by mass of a solution made by dissolving 10.0 g of NaCl into 150.0 g of water?

6.25 %

N2 (g) + 3H2 (g) -->2 NH3 (g) The equation above is the equation for the Haber process. In a certain reaction, you start with 6.0 moles of nitrogen and 10.0 moles of hydrogen. How many moles of ammonia will be produced in the reaction?

6.6 mol

A 44.7 mL sample of oxygen is heated from 320 K to 480 K at constant pressure. What is the new volume?

67ml

What is the percent composition of sulfur in N2S2?

69.6%

What is the percent composition of iron in Fe2O3?

69.94%

What is the pH of a neutral solution?

7

How many moles of CO are required to completely react with 2.45 moles of Fe2O3? Fe2 O3(s) + 3CO(g) --> 2Fe(s) + 3CO2 (g)

7.35 mol

Find the total pressure of a mixture of hydrogen and nitrogen gases that is present in a container. The partial pressure of the hydrogen is 24.0 kPa, while the partial pressure of the nitrogen is 47.0 kPa

71kPa

4.65 L of nitrogen at standard pressure is compressed into a 0.480 L container. What is the new pressure in mm Hg?

7378 mm Hg

What percent composition of chlorine in MgCl2?

74.53%

A 50 mL sample of oxygen is heated from 320 K to 480 K at constant pressure. What is the new volume?

75 mL

Identify which pressure is atmospheric pressure at sea level?

760 mmHg

_______torr = One atm

760 torr

If 5.24 L of a gas at 25.0°C is warmed until its volume increases to 6.17 L, what is the temperature of the gas in degrees Celsius?

77.9C

4 Fe(s) + 3O2(g) -->2Fe2O3(g) In a certain reaction, 54.6 g of iron is reacted with 91.6 g of Oxygen How many grams of Iron (III) oxide are produced in the reaction?

78.0 g

2HgO(s) --> 2Hg(l) + O2 (g) In a certain reaction 4.37 of HgO is decomposed, producing 3.21 of Hg What is the percent yield for the reaction?

79.3%

2HgO(s) --> 2Hg(l) + O2 (g) In a certain reaction 8.74 g of HgO is decomposed, producing 6.42 g of Hg. What is the theoretical yield of Hg?

8.10 g

1.2 L sample of gas is determined to contain 0.5 moles of nitrogen. At the same temperature and pressure, how many moles of gas would there be in a 20 L sample?

8.3 moles

Calculate the pH of a solution that has a [OH−] of 2.6 × 10−6 M.

8.4

A 1.00 L sample of a gas at 640. mm Hg is allowed to expand into an 8.00 L container at a constant temperature. The new pressure is _____.

80.0 mm Hg

A sample of gas has a volume of 800. mL at -23.0°C and 300. Torr. What would the volume of the gas be at 227.0°C and 600. Torr?

800. mL

An ideal gas in a rigid container at 0.0°C and 760 kPa is heated to 25°C. The pressure is _____.

830 kPa

Oxygen gas is 21 % of Earth's atmosphere. If the atmospheric pressure is 405 mmHg, what is the partial pressure of oxygen at that location?

85.1 mmHg

A rigid canister holds 50.0 L of helium gas at 32.0°C and 49.9 kPa. The gas is cooled until the pressure reaches 14.2 kPa. What is the Kelvin temperature of the helium?

86.8 K

To what temperature does 736 mL of hydrogen originally at 5.0°C need to be heated in order to bring the volume to 2.28 L?

861K

The actual yield of a certain reaction is 44.0 g, while the theoretical yield is 50.0 g. Calculate the percent yield.

88.0%

To what temperature does 736 mL of hydrogen originally at 15.0°C need to be heated in order to bring the volume to 2.28 L?

892K

500.0 L of gas are prepared at 0.921 atm pressure and 200.0°C. The gas is placed into a tank under high pressure. When the tank cools to 20.0°C, the pressure is 30.0 atm. What is the volume of the gas under these conditions?

9.51 L

A 1.00 L sample of a gas at 720. mm Hg is allowed to expand into an 8.00 L container at a constant temperature. The new pressure is _____.

90.0 mmHg

If you need to make 800. g of a 12.0 % by mass glucose solution, what mass of glucose needs to dissolved into what mass of water?

96.0 g of glucose in 704 g of water

Oxygen gas is 21 % of Earth's atmosphere. If the atmospheric pressure is 457mmHg, what is the partial pressure of oxygen at that location?

96mmHg

The molar mass of Cu(OH)2 is _________ grams per mole

97.55

4.65 L of nitrogen at standard pressure is compressed into a 0.480 L container. What is the new pressure in kPa?

981 kPa

Which of the following systems at constant room temperature and pressure is in a dynamic equilibrium state?

A closed bottle of soda pop

Metal hydroxides decompose and produce _____ and ____.

A metal oxide and water

Which is NOT a product that drives the occurrence of a double-replacement reaction?

A polyatomic ion

Avogadro's Law can be applied to one of the following situations. Which one?

A small balloon deflating as air is let out.

What is a solution equilibrium?

A solution in which the rate of dissolving equals the rate of recrystallizing

What does dynamic equilibrium mean?

A state where no net change is taking place, despite the fact that both reactions are still occurring

Use the heating curve below to answer the question below A. Choose the melting point of the substance. B. Which letter interval represents a solid-liquid equilibrium? C. During which letter interval is the substance vaporizing? D. choose the boiling point of the substance

A. 20C B. BC C. DE D. 90C

Select the phase change with the letter of correct name of the change A. Solid to a liquid B. Liquid to solid C. Liquid to gas D. Gas to liquid E. gas to solid F. solid to gas

A. Melting B. Freezing C. Vaporizaiton D. Condensation E. Deposition F. Sublimaiton

Identify the reaction that is NOT a decomposition reaction?

Al (s) + HCL (aq) -->AlCl3 (ag) + H2 (g)

A compound has a chemical composition of 36% aluminum and 64% sulfur. What is the empirical formula?

Al2S3

Which of the following is a synthesis reaction?

All of the answers are correct.

Which of the following substances react with oxygen?

All of the answers are correct.

Describe where the colored bands come from in the Atomic Emission Spectra? Please give lots of detail, use proper grammar and mechanics.

An Atomic Emission Spectra is the light that is released which comes from the result of atoms absorbing energy. The nucleus is where the atoms and electrons are located. Atoms like to be in the ground state with all of its electrons. These are found in the lowest level of energy. An atom is taken out of the ground state when an electron in the ground state absorbs energy. So it can't stay in a current energy level it has to move to a higher energy level that is corresponding to the new amount of energy that it holds. When electrons are excited, the atoms aren't stable. To make sure it gets back into the stable ground state the electrons have to release their energy so they can go back into the lower energy levels. That energy gives off in the form of light that has energy that correlates to the amount of energy that is given of by the electron. The proton or light that gives off has energy that is exactly the difference of the energy between the principle and the energy level of the electron. The amount of energy released from the electron has control of the wavelength and color of the light excluded. The electron that needs to move from the second to the first principle of the energy level gives off a red light. The center electron that goes to the third to the first gives off a green light. Because the energy that is given off of each of these isn't the same, the color and wavelength of the light aren't the same either. Now it's easier to identify that each line on the emission spectra has a relation to a specific transition made by an electron. Top spectrum is hydrogen, the middle is mercury, and the bottom is helium. Every element has it's own emission spectrum. Because no two elements of principle energy level is in relation to the exact same energy.

The least reactive metals are found _____ of the activity series, while the most reactive metals are found _____.

At the bottom; at the top

How many grams of solid BaSO4 will form when Na2SO4 reacts with 25 mL of 0.50 M Ba(NO3)2? Ba(NO3)2 + Na2SO4 --> BaSO4 + 2NaNO3

Ba2+(aq)+SO2−4(aq)→BaSO4(s) C=n/V C⋅V=0.500M⋅25.0⋅10−3L=0.012 Barium sulfate's molar mass (233.3gmol) mBaSO4=nBaSO4⋅molarmass=0.012moles⋅233.3gmole=2.79g

Identify the molecular compound or compounds. Choose all that are correct.

Both Cl2 and SF4

Compare and contrast nuclear fusion and fission. Please use proper grammar and mechanics.

Both fission and fusion are nuclear reactions that produce energy, but the applications are not the same. Fission is the splitting of a heavy, unstable nucleus into two lighter nuclei, and fusion is the process where two light nuclei combine together releasing vast amounts of energy.

Increasing the temperature:

Both of the increases are true

If a wavelength is 635 nm, what is the frequency? Please upload your work, showing all three steps with your answer.Please show your work along with the final answer.

C = 3.00 x 10^8 m/s y = 635nm v = ? 635 nm x 1m / 10^9 nm = 6.35 x 10^-7 v = 3.00 x 10^8 ms / 6.35 x 10^-7 v = 4.7 x 10^14

If a wavelength is 3.2 x 10^2 meters, what is the frequency? Please show your work along with the final answer.

C = 3.00 x 10^8 m/s y = 3.2 x 102 v = ? v = 3.00 x 10^8ms / 3.2 x 10^2 v = 937500

A light has the frequency of 4.74 x10^14 sec-1. What is the wavelength? Please upload your work, showing all three steps with your answer. Please show your work along with the final answer.

C = 3.00 x 10^8 m/s y = ? v = 4.74 x 10^14 sec^-1 4.74 x 10^14sec^-1 x (1m/10^9nm) 6.32 x 10^2 nm

An unknown substance has the composition of 77.87% C, 11.76% H and 10.37% O. The compound has a molar mass of 154.25 g/mole. What is the molecular formula?

C10H18O

The empirical formula of compound of CH2.. Which could NOT be the molecular formula

C12H22

A compound has a chemical composition of 34.76% oxygen, 2.63% hydrogen, and 62.62% carbon. What is the empirical formula?

C12H6O5

An unknown substance has the composition of 77.87% C, 2.63% H and 55.62% O. The compound has a molar mass of 345.2 g/mole. What is the molecular formula?

C12H9O12

What is the empirical formula for C4H6O8?

C2H3O4

A compound has a chemical composition of 26.1 g carbon, 4.3 g hydrogen, 69.5 g oxygen. What is the empirical formula?

C2H4O4

A compound is 39.3 % C, 8.23 % H and 52.4 % 0 and has a molar mass of 61.1 g/mol. What is the molecular formula of the compound?

C2H5O2

If the empirical formula of a compound is CH4 and the molar mass is 48.1 g/mol, what is the molecular formula?

C3H12

A compound has a chemical composition of .62 g carbon, .10 g hydrogen, .28 g oxygen. What is the empirical formula?

C3H6O

Methyl acetate has a chemical composition of 48.64% carbon, 8.16% hydrogen, and 43.20 % oxygen. What is the empirical formula?

C3H6O2

Select the reaction that is NOT a synthesis reaction?

C3H8 + O2 -->CO2 + H2O

A compound has a chemical composition of 47% carbon, 6% hydrogen, and 47% oxygen. What is the empirical formula?

C4H6O3

If the empirical formula of a compound is C2OH4 and has a molar mass of 88 g/mo, what is its molecular formula?

C4O2H8

A compound has a chemical composition of 97.6 g carbon, 4.9 g hydrogen, 52 g oxygen, 45.5 g nitrogen. What is the empirical formula?

C5H3O2N2

Which of the following is NOT an empirical formula?

C6H12O6

An analysis reveals that a substance consists of 26.7% of carbon, 2.24% of hydrogen and 71.1% of oxygen, If the molar mass of the compound is 270.1 g/mol, what is the MOLECULAR Formula?

C6H6O12

An analysis reveals that a substance consists of 65.5% of carbon, 5.5% of hydrogen and 29.0% of oxygen, If the molar mass of the compound is 110 g/mol, what is the MOLECULAR Formula?

C6H6O2

Select the balanced equation that represents the combustion of octane, C8H18.

C8H18 + O2 → CO2 + H2O

What is the empirical formula for C3H6O9?

CH2O3

Which is NOT an Arrhenius base?

CH3OH

Identify the compound has the lowest boiling point?

CH4

What is NOT an Arrhenius acid?

CH4

Select the reaction that is NOT a synthesis reaction?

CH4 + O2 --> CO2 +H2O

Which reaction can be classified as both a combustion and a synthesis reaction?

CO (g) + O 2 (g) --> CO2 (g)

Which substance sublimes at room temperature?

CO2

Write a skeleton equation for this reaction. When calcium carbonate is heated, it decomposes into calcium oxide and carbon dioxide gas.

CaCo3 (s) --> CaO (s) + CO2 (g)

Which of the equations represents a reversible reaction?

CaO(s) + CO2 <--> CaCO3(g)

A mineral consisted of 29.4% calcium, 23.5% sulfur and 47.1% oxygen. What is the empirical formula?

CaSO4

Write a skeleton equation for this reaction. A piece of calcium metal is placed into a solution of copper (II) nitrate. A reaction occurs, forming calcium nitrate and copper metal.

Calcium + copper (II) nitrate --> calcium nitrate and copper

When a hydrocarbon undergoes combustion, what are the products?

Carbon dioxide and water

Chlorine gas reacts with a solution of sodium bromide in a single-replacement producing aqueous sodium chloride and bromine gas. Which of the following is the correct balanced equation for this reaction?

Cl2(g) + 2 NaBr (aq) -->2NaCl (aq) + Br2(g)

Which of the following is an ionic compound that can create an electrolyte?

CoCl2

State whether each reaction listed below is a synthesis, decomposition, combustion, single or double replacement reaction. C4H10(g) + O2(g) --> CO2 + H2O (l)

Combustion

Which of the following phase changes does NOT require energy

Condensation

What type of compound can have both an empirical formula and molecular formula?

Covalent

A compound has a chemical composition of 32.8% chromium and 67.2% chlorine. What is the empirical formula?

CrCl3

Which compound is soluble in water?

Cs3PO4

Which is the correct dissociation equation for cesium bromide?

CsBr(s)-->Cs+(aq) + Br-(aq)

Identify the balanced equation?

CuCO3 (s) --> CuO(s) + CO2 (g)

Write the formula for copper sulfate hexahydrate.

CuSO4 * 6H2O

Write the formula for copper sulfate nonahydrate.

CuSO4 9H2O

When the surface area of a solid reactant decreases, the rate of reaction _____.

Decreases because of a decrease in collision frequency

State whether each reaction listed below is a synthesis, decomposition, combustion, single or double replacement reaction. Ba(OH)2(aq) + NaSO4 (aq) --> NaOH (aq) + BaSO4 (s)

Double replacement

What is the energy of a photon with the frequency of 1.02 x 10^15 Hz? Please upload your work, showing all the steps with your answer.Please show your work along with the final answer.

E = hv E = ? h = 6.63 x 10^-34 Js v = 1.02 x 10^15 Hz E = (6.63 x 10^-34 Js) x (1.02 x 10^15 Hz) E = 6.8 x 10^-19

Explain how ionic compounds are able to create electrolytes.

Electrolytes may be covalent compounds that chemically react with water to produce ions. Electricity is conducted when charges move from one place to another; it works better with metals. If ionic compounds are melted they roam free and as a result, the solution can be made to conduct electricity.

What type of equation is seen below: Energy + nitrogen + oxygen --> nitrogen monoxide

Endothermic reaction

Which of the following is the best description of the energy in a chemical reaction?

Energy may be either absorbed or released during a reaction.

Who is credited with the invention of the barometer?

Evangelista Torricelli

What type of reaction is identified by the pattern below? CH4 + O2 --> CO2 +H2O + Energy

Exothermic reaction

Identify the substance with the lowest melting point?

F2

Fluorine gas reacts with a solution of sodium bromide in a single-replacement producing aqueous sodium fluoride and bromine gas. Which of the following is the correct balanced equation for this reaction?

F2(g) + 2 NaBr (aq) -->2NaF (aq) + Br2(g)

4 Fe(s) + 3O2(g) --> 2Fe2O3(g) In Certain reaction, 27.3 g of iron is reacted with 45.8 g of Oxygen. What is the limiting reactant?

Fe

State whether each reaction listed below is a synthesis, decomposition, combustion, single or double replacement reaction.

Fe(s) + Br2 (g) --> FeBr3 (s) Synthesis

Who invented the mass spectrograph?

Francis Aston

What is the tool that tests for radiation?

Geiger counter

Which reaction can not be classified as a combustion reaction?

H2(g) + Cl2 (g) ---> 2HCl (g)

Which of the following is polyprotic?

H2CO3 and H3PO3

Write the neutralization reaction that occurs between HBr and NaOH.

HBr(aq) + NaOH(aq) = NaBr(aq) + H2O(l)

A compound has a chemical composition of 23.3 g carbon, 1 g hydrogen, 62 g oxygen, 13.6 g nitrogen. What is the empirical formula?

HC2NO4

Write the neutralization reaction that occurs between HCl and LiOH.

HCI(aq) + LiOH)aq) --> H2O(I) + LiCl(aq)

Write the neutralization reaction that occurs between HCl and NaOH.

HCl + NaOH -> H2O + NaCl

Identify the compound with the higher boiling point?

HF

A solution of the strong acid nitric acid (HNO3) is neutralized by a solution of the strong base potassium hydroxide (KOH). Which is the balanced molecular equation for the reaction?

HNO3 (aq) +KOH (aq) -->KNO3 (aq) + H2O(l)

The following gases are at STP. Which one will diffuse the fastest? F2, CO2, He, SO2, NO, NH3

He

Who discovered radioactivity?

Henri Becquerel

List and describe 5 properties of metals

High electrical conductivity- the ability of certain materials to conduct a large amount of electrical current High thermal conductivity- thermal means heat. It refers to the amount/speed of heat transmitted through a material. Malleability- the degree to which something can be shaped, altered or controlled. Ductility - to be able to undergo change of form without breaking. Luster - a substance, as a coating or polish, used to impart sheen or gloss.

What contributes to a percent yield that is greater that 100%?

Impurities in the product

What are two ways that a liquid can be turned into a gas?

Increase the temperature or decrease the pressure.

Which of these statements best describes what occurs when sugar dissolves in water?

Intermolecular forces between sugar molecules are disrupted

The lattice structure of metals are similar to

Ionic bonds

How does adding a nonvolatile solute to a solvent impact vapor pressure?

It decreases the vapor pressure

As a liquid is heated what happens to the rate of evaporation?

It increases

If a reaction has a high activation energy. What is true about the rate of reaction?

It is likely to be a slow reaction.

Identify the single-replacement reactions that will occur. (More than one answer may be possible.)

K(s) + H2O (l) --> Al (s) + HBr (aq) -->

Which combination below will NOT result in a chemical reaction?

K2SO4 (aq) + NH4Cl (aq) →

Identify the reaction that is a decomposition reaction?

KCl (s) --> K (s) + Cl2 (g)

What scale is used to measure absolute temperature?

Kelvin

Which is the expression for the ion-product of water?

Kw= [H+][OH-]

Lavoisier developed which of the following.

Law of Conservation of Mass

What law explains why equations must be balanced?

Law of Conversation of Mass

Which of the three acid-base definitions involves the classification of some substances as acids or bases that the other two definitions misses?

Lewis

Which ions are present in a solution of lithium hydroxide, LiOH

Li+, OH−

Which combination below will NOT result in a chemical reaction?

Li2SO44 (aq) + Na4Br (aq) →

Write the neutralization reaction that occurs between HF and LiOH.

LiOH(aq) + HF(aq) = LiF(aq) + H2O(l)

Choose the correct unit for reaction rate?

M/s

To convert from mass of A to mass of B in a stoichiometry problem, the following steps are followed:

Mass A ---> Moles A----> Moles B---> Mass B

Which equation is balanced?

Mg + 2HCl → MgCl2 + H2

Write a skeleton equation for this reaction. When magnesium carbonate is heated, it decomposes into magnesium oxide and carbon dioxide gas.

MgCO3 (s) --> MgO (s) + CO2 (g)

Write the formula for magnesium sulfate hexahydrate.

MgSO4 6H2O

Which solution will have a higher boiling point: A solution containing 15 grams of sucrose (C12H22O11) in 25 grams of water or a solution containing 35 grams of sodium chloride in 500 grams of water?

Molar mass of sucrose is 12*12+22*1+11*16=144+22+176=342 15g/342 Molar mass of NaCl is 23+35.5=58.5 35 grams of NaCl is 35/58.5=0.598 ----->0.598*2=1.1974 moles of particles (ions, Na+ and Cl-) So, 35 grams of sodium chloride in 500 grams of water will have a higher boiling point

To convert from moles of A to mass of B in a stoichiometry problem, the following steps are followed:

Moles A----> Moles B---> Mass B

Nitrogen gas reacts with hydrogen gas to form ammonia, a common cleaning liquid when diluted with water. Which equation is correct for this reaction?

N2 + 3H2 → 2NH3

Identify the reaction that is NOT a combustion reaction?

NO(g) +O3(g) --> NO2 (g) + O2 (g)

What is the molarity of HCl found in a titration where 30 ml of HCl is titrated with 50 ml of .1 M NaOH?

NOT 0.18M or 0.14M

What is the molarity of HCl found in a titration where 50 ml of HCl is titrated with 50 ml of .1 M NaOH?

NOT 0.59

What is the molarity of HCl found in a titration where 100 ml of HCl is titrated with 10 ml of 6 M NaOH?

NOT 12.5

Identify the balanced decomposition reaction for silver oxide?

NOT 2 AgO(s) --> 2 Ag(s) + O2 (g)

Given the expression: 2 Mg(NO3)2 How many magnesium, nitrogen, and oxygen atoms are represented?

NOT 2 Mg, 2N, 6 O

What is the molarity of HCl found in a titration where 30 ml of HCl is titrated with 15 ml of .1M NaOH?

NOT 204

When the equation below is balanced using the smallest whole number coefficients, what is the coefficient in front of C12H22O11? C12H22O11 + O2 → H2O + CO2

NOT 3

Which is NOT a single-replacement reaction?

NOT Ba + H20 -->Ba(OH)2 +H2

Identify the product of a synthesis reaction between magnesium metal and nitrogen gas?

NOT MgN

Assuming no other changes in temperature or volume, what will be the effect on the pressure inside a container of gas if the identity of gas is changed from nitrogen to helium?

NOT The effect is impossible to determine.

What happens when we apply great force to a crystalline solid?

NOT The unit cell compacts.

When barium fluoride reacts with sulfuric acid, barium sulfate and hydrofluoric acid are produced. What is the balanced equation for this reaction?

NOT c. BaF + HSO4 → BaSO4 + HF

Choose the correct formula for reaction rate.

NOT distance/time

Which of the following is always a reactant in a combustion reaction?

NOT hydrogen

The rate of diffusion of gases is ________ the rate of diffusion of liquids

NOT less than

What is molality?

NOT moles of solute per kg of solution

When we heat a substance, the

NOT potential energy increases

What are the compounds or elements on the left side of a reaction called?

NOT products

What are the compounds or elements on the right side of a chemical reaction?

NOT reactants

Why might nuclear fusion be a better source of energy on earth than nuclear fission? Please think about your answer, use proper grammar and mechanics.

Nuclear fission is nuclear and may not be so safe for the environment or body. It takes energy to make fusion happen. Atoms with really huge nuclei, such as uranium do the opposite of fusion: they release energy when they break apart. Fission reactions are much more complex than fusion. Fusion reactions also take place at very high temperatures and enormous gravitational pressures.

In several paragraphs, throughly discuss nuclear medicine include what it is and how it works. Please use proper grammar and mechanics.

Nuclear medicine is the diagnosis and treatment of disease. There is usually a giant machine that someone goes through that can detect what the problem is so the doctor can treat it. In some cases, it destroys the infection or virus but progressively.

Which of the following expresses the relationship between pressure, temperature, and volume for an ideal gas?

P X V/ T

The temperature of a gas is T1 and the original pressure is P1. The temperature of the gas is changed to T2. Which of the equations below would you use to find the new pressure (P2)?

P1 X T2 /T1

What is the empirical formula for P4O10?

P2O5

Which compound is NOT soluble in water?

PbS

If reaction A occurs quickly at room temperature and reaction B will not occur unless heated to 500°C. Which statement is true?

Reaction B has a higher activation energy than reaction A.

Which of these is NOT required for equilibrium?

Reaction occurs in an open system

Ga2O3(s) + 3SOCl2(l) --> 2GaCl3(s) +3SO2(g) In a certain reaction, 35.9 g of Ga2O3 is reacted with 55.4 g SOCl2.The GaCl3 produced is collected and its mass founded to be 48.83 g. What is the limiting reactant?

SOCl2

State whether each reaction listed below is a synthesis, decomposition, combustion, single or double replacement reaction. Cu(s) + AgNO3 (aq) --> Cu (NO3)2 (aq) + Aq (s)

Single Replacement

Which of the following is the balanced single replacement reaction that occurs when tin reacts with hydrochloric acid?

Sn(s) + 2HCl (aq) --> SnCl2 (aq) + H2(g)

Which substances can serve as a solute in an solution that has water as the solvent?

Solid, liquid or gas

Select the balanced equation for the decomposition of strontium hydroxide.

Sr(OH)2 → SrO + H2O

Which of the following is true?

Temperature is constant during a change of state.

Compare AND contrast the electromagnetic spectra and the atomic emission spectra. Please use proper grammar and mechanics.

The Atomic Emission Spectra is the light that is released which results in atoms absorbing energy. In Atomic Emission Spectra, the only thing that is given out is a certain wavelength and radiation. The emission spectra is created of discrete emission lines. In the electromagnetic spectra, the radiation of all the wavelengths is there and there aren't any discrete lines or color bands there at all.

Summarize the various atomic models; starting with the Plum Pudding and ending with Quantum Mechanical Model. Please use proper grammar and mechanics.

The Plum Pudding model was a model of the atom that was created by JJ Thompson from his work with cathode ray tubes. In his model, the neutral atom has negatively charged particles that are spread out a cluster of positive charges in plum pudding. The next model is the nuclear model. This model of the atoms was created by Ernest Rutherford. It has resulted from the gold foil experiment. From this experiment, he found out that most of the atom is empty space and the positive charge was in a core that was very dense or a center, which falsified the Plum Pudding Model. Next is Bohr's model which has a nickname called the planetary model. This model was proposed by Niels Bohr. The electrons are orbiting the nucleus that is positively charged along the certain circular orbits that have a particular discrete energy level. The next one is the Quantum Mechanical Model. This is the current model of the atom that was created by Erwin Schrodinger and he merged deBroglie's equation with more classical physics equations to come up with an equation that could foreshadow the location of electrons around the nucleus. The electrons aren't orbiting the nucleus, matter waves are.

Match the type of yield to its description Actual Yield Percent Yield Theoretical Yield

The amount of product that is produced in a reaction. The amount of product that is produced in a reaction divided by the maximum amount of product that can be found in a reaction. The maximum amount of product that can be formed in a reaction.

Which statement correctly describes the concentration of hydrogen ion and hydroxide ion in pure water at 25°C?

The concentration of hydrogen ion and hydroxide ion is 10−7 M.

Compare AND contrast the excited and the ground state of electrons. Please use proper grammar and mechanics.

The ground state is the lowest energy state of a system while excited state is any energy state higher than the ground state. There is only one ground state energy for a system, but there can be many possible excited states per system.

Why do particles of liquids and solids remain much closer together than those of gases?

The lower kinetic energy of the particles allows attractive forces to keep them together

If the empirical formula of a compound is known, what is needed in order to determine the molecular formula?

The molar mass

What will be the effect on the pressure inside a rigid container of gas if the temperature of the gas is increased?

The pressure will increase.

Which statement accurately describes the rate of evaporation and the rate of condensation in a sealed container

The rates are equal and the water level remains the same.

Select the best description of the kinetic energy of two gas particles before and after a collision?

The total kinetic energy of the two particles stays the same.

How does the volume of a gas compare to the space between the particles of a gas is at normal pressure?

The volume of the gas particles is much smaller than the space between the particles.

Particles at the surface of a liquid are pulled which direction?

There is no pull on the surface particles

How are the temperature of a gas sample and the kinetic energy of the particles of the gas related?

They are directly related

Explain why covalent compounds are unable to create electrolytes.

They are unable to create electrolytes because of the substance undergoing it. The type of electron helps determine the outcome if mixed together. Some substances just don't mix well together and can't conduct electricity.

Which of these statements best describes what occurs when oil and water are mixed?

They do not dissolve in each other but form separate layers.

Which is true of most solids?

They have an ordered three-dimensional structure

Which is not true of most solids?

They move randomly to fill their container

When pressure is added to most liquids near their freezing point, ___________.

They will solidify

In several sentences, explain how a nuclear power plant works. Please use proper grammar and mechanics.

Uranium fuel is loaded up into the reactor. In the heart of the reactor, atoms split apart and release heat energy, producing neutrons and splitting other atoms in a carefully controlled nuclear reactions. Control rods made of materials (such as boron) can be raised or lowered into the reactor to soak up neutrons and slow down or speed up the chain reaction. Water is pumped through the reactor to collect the heat energy that the chain reaction produces. It constantly flows around a closed loop linking the reactor with a heat exchanger. Inside the heat exchanger, the water from the reactor gives up its energy to cooler water flowing in another closed loop, turning it into steam. Using two unconnected loops of water and the heat exchanger helps to keep water contaminated with radioactivity safely contained in one place and well away from most of the equipment in the plant. The steam from the heat exchanger is piped to a turbine. As the steam blows past the turbine's vanes, they spin around at high speed. The spinning turbine is connected to an electricity generator and makes that spin too. The generator produces electricity that flows out to the power grid—and to homes, shops, offices, etc.

phase diagram

Use the diagram

What happens to a fluids viscosity when temperature increases?

Viscosity decreases

What happens to a liquid's viscosity when temperature increases?

Viscosity decreases

How is a weak acid different from a strong acid?

Weak acids ionize to a very small extent, while strong acids ionize completely.

In several sentences, describe the Metallic Bond Sea of Electrons model

When metals bond to each other, they form a very different bond than if they were interacting with other elements. Metals have very few, if any, valence electrons in their outer s and p orbitals. As a result, the valance electrons are not bound tightly to the positive proton center. Instead of orbiting their respective metal atoms, the valence electrons delocalize. That is to say they, the valence electrons are free to wander around the entire metal complex. Rather than being shared across a bond, or transferred, the valence electrons float in a sea of electrons, much like a water molecule floats free in the sea. Hence the term electron sea model is used to explain this movement of electrons in a metal bond. In electron sea model also known as free electron gas model, electrons are free to move inside the solid, and moving under a constant potential of the lattice. This model explained nearly all the properties of metals. Due to a constant potential, electrons don't get scattered with the lattice, so there would be minimum resistivity or maximum conductivity in case of metals. As electrons are free to move inside the metals, so they are also known as conducting electrons, hence metals are known as conductors.

Which of the following describes what occurs when a system is in balance between the forward and reverse reactions?

When the rate of the forward reaction is equal to the rate of the reverse reaction

Who x-rayed his wife's hand?

Wilhelm Rontgen

What is the biggest disadvantage to using word equations?

Words take too long to write out.

Choose the reaction that is NOT a double-replacement reaction.

Zn + (CH3COO)2 --> Zn(CH3COO)2

Choose the reactions that are NOT double-replacement reactions

Zn + Cu (CH3COO)2 --> Zn(CH3COO)2 + Cu NH4Cl+ KOH --> KCl + NH3 + H2O

When the equation below is balanced using the smallest whole number coefficients, the coefficient of the O2 is ____.

____H2 + _____O2 --> _____ H2O Answer: 1

When the equation below is balanced using the smallest whole number coefficients, what is the coefficient in front of Cr?

_____Cr + _____ O2 --> ______Cr2O3 Answer: 4

What is the emission on an alpha particle?

a helium atom

What are the products when two water molecules undergo a self-ionization reaction?

a hydronium ion and a hydroxide ion

Ionic bonding is generally.....

a metal and a nonmetal

Metal carbonates decompose and produce _____ and _____

a metal oxide and carbon dioxide

Two reactants are separated by a _____.

a plus sign

What substances are produced when an acid reacts with a base?

a salt and water

What is the best description of the symbol NaCl (aq)

a solution of sodium chloride dissolved in water.

Where is the formula for a catalyst shown in a chemical equation?

above the yield arrow

A solution with a pOH of 12.0 is _____.

acidic

Solutions that are basic are also called _____ solutions.

alkaline

What contributes to a percent yield that is less than 100%?

all of these

One type of solid-solid solution is called a(n) ___.

alloy

A [blank] particle is so weak it cannot penetrate a piece of paper.

alpha

Choose the metal that can replace iron in a single-replacement reaction.

aluminum

Which of the following variables is assumed to be held constant when using Boyle's Law?

amount of gas and temperature

A substance which can act as both an acid and a base in different reactions is said to be _____.

amphoteric

Which symbol separates the reactants from the products?

an arrow

How does water behave in a reaction with ammonia?

as an acid

Which unit of pressure expresses standard atmospheric pressure as 1?

atmosphere

Lattice points of a crystal may be occupied by _____

atoms, ions, or molecules

If a liquid in a container boils at a pressure of 780 mm Hg. Where is the container located:

below sea level

The [blank] particle cannot penetrate a piece of aluminum foil.

beta

The __________ particle cannot penetrate a piece of aluminum foil.

beta

Bases tend to taste _____.

bitter

In the presence of a base, the color of litmus is _____, while the color of phenolphthalein is _____.

blue; pink

Which does NOT indicate a chemical change may be happening?

boiling

What is the symbol for the speed of light?

c

Which specific property of water causes it to rise in a narrow tube?

capillary action

Identify the element that is NOT a diatomic molecule.

carbon

When converting from a word equation to a chemical equation what is added?

chemical formulas

The 3 in this portion of a chemical reaction is call a(n) 3H2O

coefficient

In the expression 5H2O, the 5 is a _____, while the 2 is a _____.

coefficient;subscript

What is changed to balance equations?

coefficients

The amount of solute that is dissolved in a solution is a measure of the _____ of the solution.

concentration

Solutions made of electrolytes

conduct electricity

In the list below, which action is least likely to increase the dissolving of salt in water?

cooling the solute

Name the following hydrate CuSO4 · 5 H2O.

copper (II) sulfate pentahydrate

Name the following hydrate CuSO4 · 3 H2O.

copper (II) sulfate trihydrate

Identify the correct ranking of bonds or forces in order from strongest to weakest is:

covalent bond, hydrogen bond, dispersion force

Which of the following is not an intermolecular force?

covalent bonding

What type of crystal solid is diamond?

covalent network

The highest temperature where a substance can exist in the liquid phase is called its _____.

critical temp

A three-dimensional arrangement of particles in a crystal is called the _____.

crystal lattice

: As the concentration of a reactant decreases, the rate of reaction ________.

decreases

A puddle of liquid is evaporating. What happens to the temperature of the water in the puddle?

decreases

As the pH of a solution increases, the acidity _____.

decreases

As the temperature of a sample of gas decreases at constant volume, the pressure _____.

decreases

When altitude increases, atmospheric pressure _____

decreases

The loose electrons are said to be.....

delocalized

Which of the following is not a colligative property

density

Oxygen is a(n) [ans] molecule.

diatomic

A solution with a relatively small amount of solute is _____, while one with a larger amount of solute is _____.

dilute; concentrated

The pressure of a gas is _____ related to temperature measured on the _____ scale.

directly; Kelvin

State whether each reaction listed below is a synthesis, decomposition, combustion, single or double replacement reaction. ZnCl2(s) + Cu(I) NO3 (aq) --> Zn(NO3)2 (aq) + CuCl2 (s)

double replacement

Particles at the surface of a liquid are pulled which direction?

downwards

What common household item contains a base?

drain cleaner

When gas escapes through a small hole in its container is called _____.

effusion

What type of reaction is identified by the pattern below? Energy + Reactants --> Products

endothermic reaction

A catalyst used in your body is called a(n) ______.

enzyme

The point in a neutralization reaction where the number of moles of hydrogen ions is equal to the number of moles of hydroxide ions is called the _____.

equivalence point

When a electron is at a higher level it is said to be

excited

Containers can be either rigid or flexible. If a large amount of gas is added to a rigid container, it may _____, while the same gas added to a flexible container will cause it to _____.

explode: expand

Nuclear _____ is used in power plants.

fission

Pressure is:

force divided by area

Nuclear _____ occurs on the sun.

fusion

Select the best explanation for what keeps a balloon inflated?

gas particles colliding with the inside of the balloon

Which of these is defined as a fluid?

gases and liquids only

Which situation would cause sugar to dissolve the quickest

granulated sugar in hot water

Use the de Broglie's Wave Equation to find the wavelength of an electron moving at 3 × 106 m/s. Please show your work. Note: h = Plank's constant (6.62607 x 10-34 J s)

h/mv h = 6.62607*10^-34 j-sec v = 17.3*10^6 m/sec m = 9.1*10^-31Kg = h/mv =6.62607*10^-34/9.1*10^-31*17.3*10^6 = 4.2*10^-11m

A solution is made by dissolving a NaCl in water. Compared to the pure water, the solution

has a higher normal boiling point.

What is the heavier nucleus that is created in fusion?

helium

Hydrogen bonds are formed between molecules in which hydrogen is covalently bonded to an element with:

high electronegativity and small atomic radius

solution- solute- solvent-

homogenous mixture substance that is being dissolved dissolving medium

When a solute is surrounded by water molecules it is called _____.

hydration

N2 (g) + 3H2 (g) -->2 NH3 (g) The equation above is the equation for the Haber process. In a certain reaction, you start with 3.0 moles of nitrogen and 5.0 moles of hydrogen, which molecule is the limiting reagent?

hydrogen

The H3O+ ion is called _____.

hydronium

Solid ice floats on top of liquid water because_____

ice is less dense

R is known as the ______.

ideal gas constant

As the temperature of a sample of gas increases at constant pressure, the volume _____.

increases

How does pressure affect the solubility of gases?

increases

The solubility of solid substances generally _____ as temperature increases. The solubility of gaseous substances generally _____ as temperature increases.

increases; decreases

Substances which change color in the presence of acids or bases are called _____.

indicators

If two reactant particles collide, but a reaction does not occur, this is called a(n) _____.

ineffective collision

A precipitate is defined as a (n) __________

insoluble ionic compound

A temporarily uneven electron distribution in an atom or molecule creates a(n) ______.

instantaneous dipole

What causes the individual particles of a liquid to stay together?

intermolecular attractive forces

Dipole-dipole forces are _________?

intermolecular force between polar molecules

Choose the halogen or halogens that can be replaced by bromine

iodine only

Which of these substances can water dissolve?

ionic compounds and polar molecular compounds

Which of the following would you expect to see in a double-replacement reactions?

ionic compounds in aqueous solution

Name the following hydrate FeSO4 · 7 H2O.

iron (II) sulfate heptahydrate

Name the following hydrate FeSO4 · 9 H2O.

iron (II) sulfate nonahydrate

What happens to the freezing temperature of water when salt is spread on the roads?

it decreases

What happens to the pressure inside a rigid container if the amount of gas inside is doubled?

it doubles

What happens to the boiling temperature of water when salt is added to boil noodles?

it increases

How does doubling the volume of a solution by adding solvent affect the molarity?

it is cut in half

When a binary compound decomposes what are the products?

its component elements

Which unit of pressure expresses standard atmospheric pressure as 101.325?

kPa

What two factors determine whether a collision between reacting particles will occur?

kinetic energy and orientation

An acidic solution has a pH of:

less than 7

To become stable, an excited electron gives off

light

In a chemical reaction, one reactant, called the ______ reactant, will control the extent of the reaction. A portion of the other reactants, called the ________ reactants, will remain.

limiting; excess

What do we call a fluid that has a partially organized structure?

liquid crystal

To find R, the volume of a gas must be in _____, and the gas temperature is in _____.

liters; Kelvin

In a chemical reaction lithium metal is placed in water, and lithium hydroxide is produced along with hydrogen gas. What are the reactants?

lithium and H2O

In a chemical reaction lithium metal is placed in water, and lithium hydroxide is produced along with hydrogen gas. What are the products?

lithium hydroxide and hydrogen gas

To convert from Mass A to moles of B in stoichiometry problems, the following steps are followed:

mass A ---> moles A --> moles B

To convert from mass of A to liters of B in a stoichiometry problem, the following steps are followed:

mass A --> moles A --> moles B ---> liters B

All net ionic equations must be balanced by both _____ and _____.

mass and charge

An Arrhenius base is a compound consisting of hydroxide ions and _____.

metal cations

The lattice points in a metallic crystal are made of _____.

metal cations

Which of these options lists the three general types of single-replacement reactions?

metal, hydrogen, halogen

Which type of crystal solid has delocalized electrons?

metallic

The bonds that are seen in an iron nail are

metallic bonds

Metallic Bonding is

metals only

In which type of crystal solid are the particles at the lattice points held together by dispersion forces or hydrogen bonds?

molecular

Which of the following is a variable in Avogadro's Law, but not in Boyle's, Charles's, and Gay-Lussac's Laws?

moles

What is molarity?

moles of solute per liter of solution

The coefficient of a particular substance in a balanced equation represents

moles, molecules and formula units

What ion(s) occupies the lattice points in an ionic crystal?

monatomic or polyatomic cations and anions

A reaction with a low activation energy would be likely to react _____ a reaction with a high activation energy.

more rapidly than

When a single-replacement reaction occurs, the element doing the replacing must be _____ than the element being replaced.

more reactive

In water molecules, the oxygen atoms have a slightly _____ charge, while the hydrogen atoms has a slightly _____ charge.

negative; positive

Which type of crystal is made of atoms that are all covalently bonded to their nearest neighbors?

network solid

When equal moles of strong acid and strong base are mixed, the resulting solution is _____.

neutral

The reaction between an acid and a base is called a(n) _____

neutralization reaction

Choose the metal that can displace hydrogen in an acid

nickel

Compounds containing which polyatomic anion are all soluble?

nitrate

N2 (g) + 3H2 (g) -->2 NH3 (g) The equation above is the equation for the Haber process. In a certain reaction, you start with 3.0 moles of nitrogen and 5.0 moles of hydrogen, which is the excess reactant?

nitrogen

Which molecules are diatomic?

nitrogen, bromine, hydrogen

In order for a hydrogen bond to form, a hydrogen atom must be covalently bonded to one of the three elements. What are they?

nitrogen, oxygen, fluorine

Covalent bonding is

nonmetals only

Water cannot dissolve _______________ compounds.

nonpolar

Which of the following are conserved in a chemical reaction?

number of atoms and mass

What is the only thing held constant in a combined gas law problem?

number of moles

The amount of a gas is typically defined by the _____, and represented by the variable ____.

number of moles; n

Colligative properties cause changes based:

on the number of dissolved solute particles

Which temperature scale should be used when solving Charles's Law problems?

only the Kelvin scale

The positive ion in an ionic compound is attracted to the _____ atoms in water. The negative ion in an ionic compound is attracted to the _____ atoms in water.

oxygen; hydrogen

Which expresses the relationship of pH to pOH?

pH + pOH = 14

Which is the correct equation for calculating pH?

pH= - log [H+]

Where do water particles in a beaker of water experience unequal attractive forces?

particles at the surface of the water

Identify the particles in a liquid that are the first to evaporate?

particles with the highest kinetic energy

All of the following are colligative properties except?

polarity

What do the letters pH stand for?

power of hydrogen

A solid that forms when two or more aqueous solutions are mixed is called a _____.

precipitate

What will happen to the pressure inside a rigid container of gas if some of the gas is allowed to escape? (Assuming no change in temperature).

pressure will decrease

Boyle's Law states that _____ is inversely related to _____ if _____ is held constant.

pressure; volume; temperature

Which is NOT a property of a base?

reacts with metal

The process of a dissolved solute returning to the solid state is called _____.

recrystallization

An ionic compound that is neither an acid nor a base is classified as a(n):

salt

Which would NOT be an amorphous solid?

salt

A solution that contains the maximum possible amount of dissolved solute is _____.

saturated

Crystals can be classified into how many different crystal systems?

seven

Choose the metals that can both be replaced by tin in a single-replacement reaction.

silver and lead

An equation that shows the chemical symbols and not coefficients or chemical names is called a _____.

skeleton equation

In a chemical reaction sodium metal is placed in water, and sodium hydroxide is produced along with hydrogen gas. What are the products?

sodium hydroxide and hydrogen gas

What state of matter is a precipitate

solid

What is the best description of the symbol NaCl (s)

solid sodium chloride

In a solution of sugar water, the sugar is the _____ and the water is the _____.

solute; solvent

When solute particles are surrounded by solvent particles, it is called______.

solvation

A species that is dissolved in a solutio, but does not take part in the chemical reaction is a(n)...

spectator ion

A highly concentrated solution from which dilutions are typically made for laboratory used is called a ________.

stock solution

Select the best description of the path of gas particles in a given sample of gas?

straight path which changes upon collisions with other particles

An acid which ionizes completely in water is a _____.

strong electrolyte

Liquids with _____ have the most surface tension

strong intermolecular forces

The 2 in the portion of a chemical reaction below is called a(n) 3H20

subscript

Which common substance does NOT contain an acid?

table salt

If I spill some of the product before I weigh it, how will that affect the actual yield?

the actual yield will be less than the theorectial yield

What is the solvent in a liquid-liquid solution?

the liquid present in the greater amount

What pieces of information do we need in order to calculate percent yield?

the maximim amount possible of product and the amount experimentally recovered

What quantity is needed to convert between the moles of a given gaseous substance and its volume?

the molar volume

The symbol (s) tells us ______.

the physical state of the substance

What is critical pressure?

the pressure required to liquefy a substance at the critical temperature

We can compress gases because of

the very large space between gas particles

The laboratory experiment where a solution of known concentration is reacted with a solution of unknown concentration to determine its molarity is called a _____.

titration

The two isotopes of hydrogen called "heavy" are _____ and _____.

tritium and deuterium

Which is NOT a property of an acid?

turn phenolphthalein pink

Water is called the _____ solvent because it can dissolve many different solutes.

universal

How does an experimenter visually follow the reaction during a titration experiment?

using an indicator

Real gases at room temperature and normal pressure behave:

very nearly like an ideal gas

The O-H covalent bond in a water molecule is described as _____.

very polar

What term measures a fluid's resistance to flow?

viscosity

Dilution of a solution changes the:

volume and molarity

In a can of soda, which of the following is the solvent

water

In an aqueous solution:

water is the solvent

Select the product of the combustion of hydrogen?

water only

Unit 6 starting here........ Identify the change that is NOT a chemical reaction?

water seeping through a pot of soil

A base which does not ionize completely in water is a _____.

weak electrolyte

London dispersion forces are stronger or weaker than dipole-dipole forces?

weaker

Use the de Broglie's Wave Equation to find the wavelength of a 2.00 g ball moving at 2 m/s. Please show your work. Note: h = Plank's constant (6.62607 x 10-34 J s)

y = h/mv Wavelength = planck's constant / mass in kg x velocity in m/s 2.00= 6.62607 x 10^-34/ 2

What does the arrow in a chemical reaction mean?

yields

In a chemical reaction zinc metal is placed into a solution of hydrochloric acid, and zinc chloride is produced along with hydrogen gas. What are the reactants?

zinc and hydrochloric acid

In a chemical reaction zinc metal is placed into a solution of hydrochloric acid, and zinc chloride is produced along with hydrogen gas. What are the products?

zinc chloride and hydrogen gas

If 6.24 L of a gas at 45.0°C is cooled until its volume decreases to 5.17 L, what is the temperature of the gas in degrees Celsius

−9.53°C