chem final

What is the number of moles of solute in 250 mL of a 0.4M solution? a. 0.1 mol b. 0.62 mol c. 0.16 mol d. 1.6 mol

a. 0.1 mol

What mass of Na2SO4 is needed to make 2.5 L of 2.0M solution? (Na = 23 g; S = 32 g; O = 16 g) a. 284 g b. 710 g c. 356 g d. 178 g

b. 710 g

What is the volume, in liters, of 0.500 mol of C3H8 gas at STP? a. 16.8 L b. 22.4 L c. 11.2 L d. 0.0335 L

c. 11.2 L

What is the molar mass of (NH4)2CO3? a. 138 g b. 78 g c. 144 g d. 96 g

d. 96 g

If 2.0 mL of 6.0M HCl is used to make a 500.0-mL aqueous solution, what is the molarity of the dilute solution? a. 0.024M b. 0.30M c. 0.83M d. 0.24M

a. 0.024M

To 225 mL of a 0.80M solution of KI, a student adds enough water to make 1.0 L of a more dilute KI solution. What is the molarity of the new solution? a. 0.18M b. 180M c. 2.8M d. 0.35M

a. 0.18M

Calculate the number of moles of Al2O3 that are produced when 0.60 mol of Fe is produced in the following reaction. 2Al(s) + 3FeO(s) --> 3Fe(s) + Al2O3(s) a. 0.20 mol b. 0.40 mol c. 0.60 mol d. 0.90 mol

a. 0.20 mol

What are the coefficients that will balance the skeleton equation below? N2 + H2→ NH3 a. 1, 3, 2 b. 1, 1, 2 c. 1, 3, 3 d. 3, 1, 2

a. 1, 3, 2

What are the missing coefficients for the skeleton equation below?Al2(SO4)3(aq) KOH(aq) → Al(OH)3(aq) K2SO4(aq) a. 1, 6, 2, 3 b. 1, 3, 2, 3 c. 4, 6, 2, 3 d. 2, 12, 4, 6

a. 1, 6, 2, 3

How many grams of chromium are needed to react with an excess of CuSO4 to produce 27.0 g Cu? 2Cr(s) + 3CuSO4(aq) → Cr2(SO4)3(aq) + 3Cu(s) a. 14.7 g b. 33.2 g c. 81.5 g d. 18.0 g

a. 14.7 g

What is the mass of oxygen in 250 g of sulfuric acid, H2SO4? a. 160 g b. 16 g c. 0.65 g d. 3.9 g

a. 160 g

When the following equation is balanced, what is the coefficient for HCl? Mg(s) + HCl(aq) → MgCl2(aq) + H2(g) a. 2 b. 1 c. 6 d. 3

a. 2

How many moles of CaBr2 are in 5.0 grams of CaBr2? a. 2.5 10^-2 mol b. 4.2 x 10^-2 mol c. 1.0 x 10^3 mol d. 4.0 x 10^1 mol

a. 2.5 10^-2 mol

The volume of alcohol present in 620 mL of a 40.0% (v/v) solution of alcohol is ____. a. 248 mL b. 372 mL c. 40.0 mL d. 580 mL

a. 248 mL

If the percent by volume is 2.0% and the volume of solution is 250 mL, what is the volume of solute in solution? a. 5.0 mL b. 0.5 mL c. 1.25 mL d. 12.5 mL

a. 5.0 mL

The solubility of potassium chloride 34g KCl/100 g H2O is at 20 degrees C. What is the maximum amount of KCl that can dissolve in 200 g of water at 20C? a. 68 g b. 17 g c. 34 g d. 6800 g

a. 68 g

If 60.2 grams of Hg combines completely with 24.0 grams of Br to form a compound, what is the percent composition of Hg in the compound? a. 71.5% b. 60.1% c. 39.9% d. 28.5%

a. 71.5%

A double-replacement reaction takes place when aqueous cobalt(III) chloride reacts with aqueous lithium hydroxide. One of the products of this reaction is a. Co(OH)3 b. LiCo3 c. LiCl3 d. Co(OH)2

a. Co(OH)3

What is the empirical formula of a compound that is 40% sulfur and 60% oxygen by weight? a. SO3 b. SO2 c. S6O4 d. SO

a. SO3

What do you know about a chemical reaction if the value of ^H is positive? a. The reaction is endothermic. b. The reaction is exothermic. c. The reaction cannot occur at room temperature. d. The reaction occurs without the addition of energy.

a. The reaction is endothermic.

What happens to the solubility of a gas in a liquid if the partial pressure of the gas above the liquid decreases? a. The solubility decreases. b. The solubility cannot be determined. c. The solubility increases. d. The solubility remains the same.

a. The solubility decreases.

The atomic masses of any two elements contain the same number of ____. a. atoms b. grams c. ions d. milliliters

a. atoms

A process that absorbs heat is a(n) ____. a. endothermic process b. ectothermic process c. polythermic process d. exothermic process

a. endothermic process

How can energy change during a chemical reaction? a. transfer of heat and/or work b. increase in heat and/or destruction of matter c. change in the mass of the reactants or thermal energy d. increase or decrease in total energy of a system

a. transfer of heat and/or work

What is the specific heat of a substance if 1560 cal are required to raise the temperature of a 312-g sample by 15 degrees C? a. 1.33 cal/g degrees C b. 0.33 cal/g degrees C c. 0.033 cal/g degrees C d. 0.99 cal/g degrees C

b. 0.33 cal/g degrees C

How many moles of glucose, C6H12O6 can be "burned" biologically when 10.0 mol of oxygen is available? C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l) a. 60.0 mol b. 1.67 mol c. 0.938 mol d. 53.3 mol

b. 1.67 mol

How many grams of beryllium are needed to produce 36.0 g of hydrogen? (Assume an excess of water.) Be(s) + 2H2O(l) → Be(OH)2 (aq) + H2(g) a. 4.00 g b. 162 g c. 324 g d. 36.0 g

b. 162 g

What is the mass of silver in 3.4 g AgNO3? a. 3.0 g b. 2.2 g c. 0.025 g d. 0.64 g

b. 2.2 g

The molar volume of a gas at STP occupies ____. a. 1 kilopascal b. 22.4 L c. 12 grams

b. 22.4 L

If 1 egg and 1/3 cup of oil are needed for each bag of brownie mix, how many bags of brownie mix do you need if you want to use up all 3 eggs and 1 cup of oil? a. 1 b. 3 c. 4 d. 2

b. 3

When the equation Fe + Cl2 → FeCl3 is balanced, what is the coefficient for Cl2? a. 1 b. 3 c. 2 d. 4

b. 3

How many kilocalories of heat are required to raise the temperature of 225 g of aluminum from 20 degrees C to 100 degrees C? (specific heat of aluminum = 0.21 cal/ g degrees C) a. 0.59 kcal b. 3.8 kcal c. 38 kcal d. 85 kcal

b. 3.8 kcal

What is the molar mass of AuCl3? a. 130 g b. 303.6 g c. 96 g d. 232.5 g

b. 303.6 g

What mass of sucrose, C12H22O11, is needed to make 500.0 mL of a 0.200M solution? a. 100 g b. 34.2 g c. 17.1 g d. 68.4 g

b. 34.2 g

How many hydrogen atoms are in 5 molecules of isopropyl alcohol, C3H7O? a. 5 b. 35 c. 5 x (6.02 10^23) d. 35 x (6.02 10^23)

b. 35

Rewrite the following word equation as a balanced chemical equation. What is the coefficient and symbol for fluorine?nitrogen trifluoride → nitrogen + fluorine a. F3 b. 3F2 c. 6F d. 6F2

b. 3F2

In a particular reaction between copper metal and silver nitrate, 12.7 g Cu produced 38.1 g Ag. What is the percent yield of silver in this reaction? Cu + 2AgNO3 → Cu(NO3)2 + 2Ag a. 77.3% b. 88.2% c. 176% d. 56.7%

b. 88.2%

What is the balanced chemical equation for the reaction that takes place between bromine and sodium iodide? a. Br + NaI2 --> NaBrI2 b. Br2 + 2NaI --> 2NaBr I2 c. Br + NaI2 --> NaBr I2 d. Br2 + NaI --> NaBr2 + I

b. Br2 + 2NaI --> 2NaBr I2

Which of the following is the correctly balanced equation for the incomplete combustion of heptene, C7H14? a. 2C7H14 + 21O2 --> 14CO2 + 14H2O b. C7H14 + 7O2 --> 7CO + 7H2O c. C7H14 + 14O --> 7CO + 7H2O d. C7H14 + O2--> C7O2 + 7H2

b. C7H14 + 7O2 --> 7CO + 7H2O

How is thermal energy transferred between two objects that are at different temperatures? a. Heat flows back and forth between the two objects until they reach the same temperature. b. Heat flows from the warmer object to the cooler object until they reach the same temperature. c. Heat flows from the object that has more thermal energy to the object that has less thermal energy. d. The object at a lower temperature pulls heat energy from the warmer object.

b. Heat flows from the warmer object to the cooler object until they reach the same temperature.

One of the products when aqueous Na2CO3 reacts with aqueous Sn(NO3)2 is... a. Sn(CO3)2- b. NaNO3- c. NaSn d. CNO3

b. NaNO3-

Use the activity series of metals to complete a balanced chemical equation for the following single replacement reaction. Ag(s) + KNO3(aq) → a. AgNO3 + K b. No reaction takes place because silver is less reactive than potassium. c. AgKNO3 d. AgK + NO3

b. No reaction takes place because silver is less reactive than potassium.

What are the correct formulas and coefficients for the products of the following double-replacement reaction? RbOH + H3PO4→ a. H3Rb + PO4OH b. Rb3PO4 + 3H2O c. Rb(PO4)3 + H2O d. RbPO4 + 2H2O

b. Rb3PO4 + 3H2O

The equation 2C3H7OH + 9O2→ 6CO2 + 8H2O is an example of which type of reaction? a. double-replacement reaction b. combustion reaction c. decomposition reaction d. single-replacement reaction

b. combustion reaction

The equation H3PO4 + 3KOH → K3PO3 + 3H2O is an example of which type of reaction? a. single-replacement reaction b. double-replacement reaction c. combination reaction d. decomposition reaction

b. double-replacement reaction

What does the symbol ^H stand for? a. the specific heat of a substance b. the heat of reaction for a chemical reaction c. the heat capacity of a substance d. one Calorie given off by a reaction

b. the heat of reaction for a chemical reaction

What is the number of moles in 9.63 L of H2S gas at STP? a. 3.54 mol b. 0.104 mol c. 0.430 mol d. 14.7 mol

c. 0.430 mol

What are the coefficients that will balance the skeleton equation below? AlCl3 + NaOH → Al(OH)3 NaCl a. 3, 1, 3, 1 b. 1, 3, 3, 1 c. 1, 3, 1, 3 d. 1, 1, 1, 3

c. 1, 3, 1, 3

Mercury can be obtained by reacting mercury(II) sulfide with calcium oxide. How many grams of calcium oxide are needed to produce 36.0 g of Hg? 4HgS(s) + 4CaO(s) → 4Hg(l) + 3CaS(s) + CaSO4 a. 7.56 g b. 13.4 g c. 10.1 g d. 1.80 g

c. 10.1 g

What is the molarity of 200 mL of solution in which 2.0 moles of sodium bromide is dissolved? a. 4.0M b. 0.40M c. 10M d. 2.0M

c. 10M

What is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution? a. 4.0M b. 0.081M c. 12M d. 81M

c. 12M

What are the missing coefficients for the skeleton equation below?Cr(s) + Fe(NO3)2(aq) → Fe(s) + Cr(NO3)3(aq) a. 4, 6, 6, 2 b. 2, 3, 2, 3 c. 2, 3, 3, 2 d. 1, 3, 3, 1

c. 2, 3, 3, 2

The equation below shows the decomposition of lead nitrate. How many grams of oxygen are produced when 11.5 g NO2 is formed? 2Pb(NO3)2 (s) --> 2PbO (s) + 4NO2 (g) + O2(g) a. 1.00 g b. 2.88 g c. 2.00 g d. 32.0 g

c. 2.00 g

The specific heat of silver is 0.24 J/ g degrees C . How many joules of energy are needed to warm 4.37 g of silver from 25.0 degrees C to 27.5 degrees C? a. 0.022 J b. 45.5 J c. 2.62 J d. 0.14 J

c. 2.62 J

What is the percent composition of chromium in BaCrO4? a. 25.2% b. 9.47% c. 20.5% d. 4.87%

c. 20.5%

Iron(III) oxide is formed when iron combines with oxygen in the air. How many grams of Fe2O3 are formed when 16.7 g of Fe reacts completely with oxygen? 4Fe + 3O2 --> 2Fe2O3 a. 12.0 g b. 95.6 g c. 23.9 g d. 47.8 g

c. 23.9 g

One mole of hydrogen is burned in oxygen to produce water in the gas phase, ^H = -285.8 kJ. What is the energy change when 1 mole of water, in the gas phase, decomposes to form hydrogen and oxygen? a. 285.8 kJ of heat is released. b. 142.9 kJ of heat is absorbed. c. 285.8 kJ of heat is absorbed. d. 142.9 kJ of heat is released.

c. 285.8 kJ of heat is absorbed.

Aluminum reacts with sulfuric acid to produce aluminum sulfate and hydrogen gas. How many grams of aluminum sulfate would be formed if 250 g H2SO4 completely reacted with aluminum? 2Al + 3H2SO4 --> Al2(SO4)3 + 3H2 a. 450 g b. 870 g c. 290 g d. 0.85 g

c. 290 g

The volume of 6.00M HCl needed to make 319 mL of 6.80M HCl is ____. a. 7.8 mL b. 281 mL c. 362 mL d. 0.128 mL

c. 362 mL

How many atoms are in 0.075 mol of titanium? a. 6.4 x 10^2 b. 1.2 x 10^-25 c. 4.5 x 10^22 d. 2.2 x 10^24

c. 4.5 x 10^22

What is the amount of heat required to raise the temperature of 200.0 g of aluminum by 10 degrees C? (specific heat of aluminum = 0.21 cal/g degrees C) a. 4200 cal b. 42,000 cal c. 420 cal d. 420,000 cal

c. 420 cal

Calculate the energy required to produce 7.00 mol ClO on the basis of the following balanced equation. 2Cl2(g) + 7O2(g) + 130 kcal --> 2Cl2O7(g) a. 65 kcal b. 130 kcal c. 455 kcal d. 7.00 kcal

c. 455 kcal

How many mL of a 2.0M NaBr solution are needed to make 200.0 mL of 0.50M NaBr? a. 100 mL b. 150 mL c. 50 mL d. 25 mL

c. 50 mL

What is the percent by mass of carbon in acetone, C3H6O? a. 20.7% b. 1.61% c. 62.1% d. 30.0%

c. 62.1%

How many grams of H3PO4 are produced when 10.0 moles of water react with an excess of P4O10? P4O10 + 6H2O --> 4H3PO4 a. 6.7 g b. 1.22 g c. 653 g d. 147 g

c. 653 g

When glucose is consumed, it reacts with oxygen in the body to produce carbon dioxide, water, and energy. How many grams of carbon dioxide would be produced if 45 g of C6H12O6 completely reacted with oxygen? a. 11 g b. 1.5 g c. 66 g d. 1.8 g

c. 66 g

If the percent (mass/mass) for a solute is 4% and the mass of the solution is 200 g, what is the mass of solute in solution? a. 80 g b. 800 g c. 8.0 g d. 50 g

c. 8.0 g

How many moles of tungsten atoms are in 4.8 x 10^25 atoms of tungsten? a. 1.3 x 10^-1 moles b. 1.3 x 10^-2 moles c. 8.0 x 10^1 moles d. 8.0 x 10^2 moles

c. 8.0 x 10^1 moles

Lead nitrate can be decomposed by heating. What is the percent yield of the decomposition reaction if 9.9 g Pb(NO3)2 are heated to give 5.5 g of PbO? 2Pb(NO3)2(s) → 2PbO(s) + 4NO2(g) + O2(g) a. 56% b. 67% c. 82% d. 44%

c. 82%

What is the percent composition of carbon, in heptane, C7H16? a. 68% b. 12% c. 84% d. 19%

c. 84%

If a combination reaction takes place between rubidium and bromine, the chemical formula for the product is ____. a. RbBr2 b. Rb2Br c. RbBr d. RuBr

c. RbBr

When two substances react to form products, the reactant which is used up is called the ____. a. determining reagent b. excess reagent c. limiting reagent d. catalytic reagent

c. limiting reagent

Avogadro's number of representative particles is equal to one ____. a. kelvin b. kilogram c. mole d. gram

c. mole

In a combustion reaction, one of the reactants is a. a metal. b. hydrogen. c. oxygen d. nitrogen.

c. oxygen.

In the chemical equation H2O2(aq) → H2O(l) O2(g), the is O2 a ____. a. catalyst b. solid c. product d. reactant

c. product

The equation Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) is an example of which type of reaction? a. double-replacement reaction b. combination reaction c. single-replacement reaction d. decomposition reaction

c. single-replacement reaction

The type of reaction that takes place when one element reacts with a compound to form a new compound and a different element is a ____. a. combination reaction b. double-replacement reaction c. single-replacement reaction d. decomposition reaction

c. single-replacement reaction

The quantity of heat required to change the temperature of 1 g of a substance by 1 degrees C is defined as ____. a. a joule b. a calorie c. specific heat d. density

c. specific heat

How many moles of H3PO4 are produced when 71.0 g P4O10 reacts completely to form H3PO4? P4O10 + 6H2O --> 4H3PO4 a. 0.063 5 mol b. 4.00 mol c. 16.0 mol d. 1.00 mol

d. 1.00 mol

How many molecules are in 2.10 mol CO2? a. 3.49 x 10^-24 molecules b. 3.79 x 10^24 molecules c. 2.53 x 10^24 molecules d. 1.26 x 10^24 molecules

d. 1.26 x 10^24 molecules

What is the number of moles in 432 g Ba(NO3)2? a. 0.605 mol b. 0.237 mol c. 3.66 mol d. 1.65 mol

d. 1.65 mol

Metallic copper is formed when aluminum reacts with copper(II) sulfate. How many grams of metallic copper can be obtained when 54.0 g of Al react with 319 g of CuSO4? Al + 3CuSO4 --> Al2(SO4)3 + 3Cu a. 162 g b. 21.2 g c. 381 g d. 127 g

d. 127 g

How many milliliters of alcohol are in 167 mL of an 85.0% (v/v) alcohol solution? a. 145 mL b. 228 mL c. 252 mL d. 142 mL

d. 142 mL

In the reaction 2CO(g) + O2(g) → 2CO2(g), what is the ratio of moles of oxygen used to moles of CO2 produced? a. 1:1 b. 2:2 c. 2:1 d. 1:2

d. 1:2

When the equation KClO3(s) → KCl(s) + O2(g) is balanced, the coefficient of KClO3 is a. 3. b. 4. c. 1. d. 2.

d. 2.

How many atoms are in 3.5 moles of arsenic atoms? a. 7.5 x 10^1 atoms b. 5.8 x 10^-24 atoms c. 1.7 x 10^23 atoms d. 2.1 x 10^24 atoms

d. 2.1 x 10^24 atoms

When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed. The balanced equation for this reaction is ____. a. KH + BaCl --> KCl + BaH b. KOH + BaCl --> KCl + BaOH c. KOH + BaCl2 --> KCl2 + BaOH d. 2KOH + BaCl2 --> 2KCl + Ba(OH)2

d. 2KOH + BaCl2 --> 2KCl + Ba(OH)2

What is the concentration of a solution that contains 6 moles of solute in 2 liters of solution? a. 12M b. 6M c. 7M d. 3M

d. 3M

Whats the maximum number of PH3 that can be formed when 6.2 g of phosphorus reacts with 4.0 g of hydrogen to form PH3? P4(g) + 6H2(g) → 4PH3(g) a. 270 g b. 0.43 g c. 45 g d. 6.8 g

d. 6.8 g

What is the mass in grams of 5.90 mol C8H18? a. 0.0512 g b. 19.4 g c. 389 g d. 673 g

d. 673 g

What is the empirical formula of a substance that is 53.5% C, 15.5% H, and 31.1% N by weight? a. C4H14N2 b. CH4N7 c. C3HN2 d. C2H8N

d. C2H8N

When your body breaks down sugar completely, how much heat is released compared to burning the same amount of sugar in a flame? a. More heat is released. b. No heat is released inside the body. c. Less heat is released. d. The same amount of heat is released.

d. The same amount of heat is released.

What is the concentration of a solution? a. a measure of the volume of solvent used to make the solution b. a measure of the number of moles of solute dissolved c. a measure of the amount of solute that can be dissolved d. a measure of the amount of solute in a specified quantity of solvent

d. a measure of the amount of solute in a specified quantity of solvent

In every balanced chemical equation, each side of the equation has the same number of ____. a. moles b. molecules c. coefficients d. atoms of each element

d. atoms of each element

The reaction 2Fe + 3Cl→ 2FeCl3 is an example of which type of reaction? a. combustion reaction b. decomposition reaction c. single-replacement reaction d. combination reaction

d. combination reaction

The volume of one mole of a substance is 22.4 L at STP for all ____. a. liquids b. solids c. compounds d. gases

d. gases

During an endothermic chemical reaction, what is the source of energy that causes the reaction to continue? a. materials that are part of the system b. reactants involved in the reaction c. chemical bonds of the reaction products d. materials in the surroundings of the system

d. materials in the surroundings of the system

If adding of a crystal of the solute to an aqueous solution causes many particles to come out of the solution, the original solution was ____. a. saturated b. an emulsion c. unsaturated d. supersaturated

d. supersaturated

What information is needed to calculate the percent composition of a compound? a. the weight of the sample to be analyzed and its molar volume b. the formula of the compound and its density c. the weight of the sample to be analyzed and its density d. the formula of the compound and the atomic mass of its elements

d. the formula of the compound and the atomic mass of its elements

When an equation is used to calculate the amount of product that will form during a reaction, then the value obtained is called the ____. a. actual yield b. percent yield c. minimum yield d. theoretical yield

d. theoretical yield