Chem Final Complete

The pressure of a neon gas sample at 25 °C decreases from 1.00 atm to 0.500 atm. What is the final Celsius temperature if the volume remains constant? 422 °C 149 °C 596 °C -124 °C 323 °C

-124 °C

What are the ion concentrations in a 0.12 M solution of AlCl 3? 0.12 M Al3+ ions and 0.36 M Cl- ions 0.12 M Al3+ ions and 0.040 M Cl- ions 0.36 M Al3+ ions and 0.12 M Cl- ions 0.040 M Al3+ ions and 0.040 M Cl- ions none of the above

0.12 M Al 3+ ions and 0.36 M Cl - ions

If a 20.0 mL test tube measures 15.0 cm, what is the length in meters? 0.150 m 1.50 m 1500 m 15.0 m none of the above

0.150 m

What is the molarity of a hydrochloric acid solution prepared by diluting 500.0 mL of 1.00 M HCl to a total volume of 2.50 L? 0.500 M 0.200 M 0.100 M 5.00 M 2.00 M

0.200 M

What is the molarity of aqueous lithium bromide if 25.0 mL of LiBr reacts with 10.0 mL of 0.250 M Pb(NO 3) 2? Pb(NO 3) 2( aq) + 2 LiBr( aq) → PbBr 2( s) + 2 LiNO 3( aq) 1.25 M 0.100 M 0.250 M 0.200 M 0.0500 M

0.200 M

What is the mass of 2.10 x 10 21 atoms of copper, Cu? 0.00349 g 63.5 g 0.222 g 0.101 g 831 g

0.222 g

How many moles of water are produced from the reaction of 0.112 mol of oxygen according to this equation? 2H 2( g) + O 2( g) → 2H 2O( g) 2.00 mol 0.0560 mol 0.112 mol 0.224 mol 0.448 mol

0.224 mol

How many moles of nitrogen are formed when 58.6 g of KNO 3 decomposes according to the following reaction? The molar mass of KNO 3 is 101.11 g/mol. 4 KNO 3(s) → 2 K 2O(s) + 2 N 2(g) + 5 O 2(g) 0.724 mol N2 1.73 mol N2 0.290 mol N2 0.580 mol N2 18.5 mol N2

0.290 mol N2

What is the molarity of a sucrose solution that contains 10.0 g of C 12H 22O 11 (342.34 g/mol) dissolved in 100.0 mL of solution? 0.00292 M 0.292 M 0.0292 M 3.42 M 34.2 M

0.292 M

A sample of ozone gas occupies 225 mL at 1.00 atm and 0 °C. If the volume of the gas is 625 mL at 25 °C, what is the pressure? 0.393 atm 2.54 atm 0.330 atm 3.03 atm 0.360 atm

0.393 atm

Calculate the volume (in L) of a solution that contains 3.12 moles of NaCl if the concentration of this solution is 6.67 M NaCl. 20.8 L 0.208 L 2.14 L 0.468 L

0.468 L

How many moles of oxygen gas react with 1.00 mol NO? (Unbalanced) __NO( g) + __O 2( g) -> __NO 2( g) 0.250 mol 2.00 mol 1.00 mol 0.500 mol none of the above

0.500 mol

If a copper solid has a volume of 8.75 cm 3, what is the volume in cubic inches? (1 inch = 2.54 cm) 143 in.3 3.44 in.3 0.534 in.3 22.2 in.3 1.36 in.3

0.534 in. 3

Calculate the grams of magnesium needed to completely react with 100.0 mL of 0.557 M HClO 4 solution, given the following reaction: Mg (s) + 2 HClO 4 (aq) Mg(ClO 4) 2 (aq) + H 2 (g) 2.70 g 675 g 1350 g 0.677 g

0.677 g

Given:2 Na + O2 Na2O2Calculate the moles of sodium peroxide (Na2O2) produced if 32.5 g of sodium reacts with excess oxygen. 0.707 mol 0.354 mol 27.6 mol 55.1 mol

0.707 mol

How many moles of steam, H 2O, react with 1 mol of charcoal, C, according to the balanced chemical equation? C( s) + H2O( g) -> CO( g) + H2( g) 4 mol 1 mol 2 mol 3 mol none of the above

1 mol

According to the metric system, 1 g = ________ cg. 1 x 101 1 x 102 1 x 106 1 x 103 none of the above

1 x 10 2

If 37.5 mL of 0.100 M calcium chloride reacts completely with aqueous silver nitrate, what is the mass of AgCl (143.32 g/mol) precipitate? CaCl 2( aq) + 2 AgNO 3( aq) → 2 AgCl( s) + Ca(NO 3) 3( aq) 537 g 1.07 g 0.269 g 0.537 g 269 g

1.07 g

If the radius of a silicon atom is 1.18 x 10 -8 cm, what is the radius in nm? 1.18 x 10-1 nm 1.18 x 10-15 nm 1.18 x 103 nm 1.18 x 10-10 nm none of the above

1.18 x 10 -1 nm

How many molecules of methane gas, CH 4, have a mass equal to 3.20 g? 1.20 x 1024 molecules 1.20 x 1023 molecules 3.01 x 1024 molecules 3.01 x 1023 molecules 1.93 x 1024 molecules

1.20 x 10 23 molecules

What is the equivalent pressure of 968 mm Hg in units of atm? 0.785 atm 1.27 atm 968 atm 1.30 atm none of the above

1.27 atm

If the mass of Mars is 6.42 x 10 23 kg, what is the mass in pounds?(Given: 1 lb = 454 g) 1.41 x 1018 lb 2.91 x 1023 lb 2.91 x 1024 lb 6.42 x 1023 lb 1.41 x 1024 lb

1.41 x 10 24 lb

If Earth is 1.50 x 10 8 km from the Sun, what is the distance in Gm? 1.50 x 105 Gm 1.50 x 102 Gm 1.50 x 1020 Gm 1.50 x 10-1 Gm none of the above

1.50 x 10 2 Gm

Each d-subshell can accommodate a maximum of ________ electrons. 2 6 10 3 5

10

What is the maximum number of electrons that the d subshell can hold? 5 6 10 32

10

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO 3? Assume that there is excess NO 2 present. The molar masses are as follows: H 2O = 18.02 g/mol, HNO 3 = 63.02 g/mol. 3 NO 2(g) + H 2O(l) → 2 HNO 3(aq) + NO(g) 38.0 g H2O 21.7 g H2O 10.9 g H2O 26.5 g H2O 43.4 g H2O

10.9 g H 2O

The total number of subatomic particles (protons, electrons, and neutrons) in an atom of 75Ge is ________. 143 107 84 86

107

What are the bond angles in the following molecular model of CCl 4? - less than 109.5° - 109.5° - less than 120° but greater than 109.5° - 120°

109.5°

The bond angles marked a, b, and c in the molecule below are about ________, ________, and ________, respectively. (Picture) 109.5°, 109.5°, 90° 90°, 180°, 90° 109.5°, 109.5°, 109.5° 109.5°, 109.5°, 120° 120°, 109.5°, 120°

109.5°, 109.5°, 120°

Draw the electron dot formula for silicon tetrabromide, SiBr 4. How many nonbonding electron pairs are in a silicon tetrabromide molecule? 12 2 4 1 none of the above

12

Determine the volume of O 2 (at STP) formed when 50.0 g of KClO 3 decomposes according to the following reaction. The molar mass for KClO 3 is 122.55 g/mol. 2 KClO 3( s) → 2 KCl( s) + 3 O 2( g) 12.3 L 9.14 L 8.22 L 13.7 L 14.6 L

13.7 L

At maximum, an f subshell can hold ________ electrons, a d subshell can hold ________ electrons and a p subshell can hold ________ electrons. 18, 8, 2 10, 14, 6 2, 12, 21 14, 10, 6

14, 10, 6

Ammonium sulfate, (NH 4) 2SO 4, is in fertilizer and replenishes nitrogen to the soil. What is the number of atoms in the chemical formula of ammonium sulfate? - 20 - 14 - 15 - 13

15

8.60 mol of water has a mass of ________. 32.0 g 18.0 g 155 g 1000. g 15.5 g

155 g

How many waffles can be made from 1 dozen eggs, assuming you have enough of all other ingredients?Given: 2 cups flour + 3 eggs + 1 tbs oil → 4 waffles 16 48 12 4 not enough information

16

What volume of 16 M acid must be diluted with distilled water to prepare 500.0 mL of 0.50 M acid? 1.6 mL 0.016 mL 16 mL 0.16 mL 160 mL

16 mL

What is the volume of 6.00 M nitric acid that contains 6.302 g of HNO 3 solute (63.02 g/mol)? 167 mL 1670 mL 0.600 mL 16.7 mL 60.0 mL

16.7 mL

What is the mass of a 7.50% urine sample that contains 122 g of dissolved solute? 1630 g 9.89 g 1500 g 9.15 g 915 g

1630 g

What is the mass of zinc acetate (183.49 g/mol) dissolved in 0.200 L of 0.500 M Zn(C 2H 3O 2) 2 solution? 91.7 g 1.83 g 18.3 g 12.4 g 36.7 g

18.3 g

What volume of 0.255 M hydrochloric acid reacts completely with 0.400 g of sodium hydrogen carbonate, NaHCO 3 (84.01 g/mol)? NaHCO 3( s) + HCl( aq) → NaCl( aq) + H 2O( l) + CO 2( g) 121 mL 18.7 mL 53.6 mL 4.76 mL 132 mL

18.7 mL

Determine the answer to the following equation with correct number of significant figures:(17.103 + 2.03) × 1.02521 = ________ 20 19.6 19.6153 19.62 none of the above

19.62

The ground state electron configuration of Ga is ________. 1s22s22p63s23p64s24d104p1 1s22s23s23p64s23d104p1 [Ar]4s23d11 1s22s22p63s23p64s23d104p1 1s2 2s2 2p6 3s2 3p6 4s2 3d104d1

1s 22s 22p 63s 23p 64s 23d 104p 1

What is the electron configuration for an aluminum ion, Al 3+? 1s2 2s2 2p6 1s2 2s2 2p6 3s2 1s2 2s2 2p6 3s2 3p1 1s2 2s2 2p6 3p1 none of the above

1s2 2s2 2p6

Any one d orbital can hold up to ________ electrons. 6 18 10 2 8

2

Calcium has ________ valence electron(s) 8 10 6 4 2

2

How many of the following elements and symbols are entirely correct? magnesium, (Mg) iron, Ir potassium, K gold, Go - 2 - 3 - 1 - 0

2

What is the ionic charge for the lead ion in Pb(C 2H 3O 2) 2? zero 1+ 2+ 3+ none of the above

2+

What are the coefficients for the following reaction when it is properly balanced?___potassium iodide + ___lead (II) acetate → ___lead (II) iodide +___potassium acetate 1, 1, 2, 2 2, 1, 1, 1 3, 2, 2, 1 2, 1, 1, 2 none of the above

2, 1, 1, 2

How many moles of hydrogen iodide are produced from 1.00 mol of iodine? (not balanced) __H 2( g) + __I 2( g) -> __HI( g) 2.00 mol 0.500 mol 4.00 mol 1.00 mol none of the above

2.00 mol

How many grams of solid KCl are needed to prepare 250. mL of a 0.125 M solution? 9.32 g 31.3 g 15.6 g 2.33 g

2.33 g

How many moles of ammonia contain 1.51 x 10 24 NH 3 molecules? 0.251 mol 2.51 mol 3.99 mol 0.399 mol 25.1 mol

2.51 mol

If a nitrogen gas sample occupies a volume of 2.55 L at 22.0 °C and 0.860 atm, what is the mass of the N 2 gas? 1.27 g 34.0 g 2.54 g 0.394 g 5.13 g

2.54 g

The volume occupied by 4.00 g oxygen gas at STP is ________. 11.2 L 22.4 L 5.60 L 2.80 L

2.80 L

How many moles of Al are needed to react exactly with 10.0 moles of Fe 2O 3 according to the following equation? Fe 2O 3 + 2 Al -> Al2O3 + 2Fe 60.0 moles 30.0 moles 20.0 moles 15.0 moles

20.0 moles

How many moles of H 2O will be produced if 6.80 x 10 24 formula units of NH 4NO 3 are decomposed in the reaction given below? NH4 NO3 -> N2O + 2H2O 22.6 moles 3.30 moles 0.876 mole 5.40 moles

22.6 moles

Which of the following correctly illustrates the conservation of mass for the reaction below? 4Fe( s) + 3O 2( g) → 2Fe 2O 3( s) 223 g Fe, 96.0 g O2, 319 g Fe2O3 4.00 g Fe, 3.00 g O2, 2.00 g Fe2O3 40.0 g Fe, 30.00 g O2, 70.0 g Fe2O3 55.9 g Fe, 16.0 g O2, 160. g Fe2O3 100. g Fe, 100. g O2, 200. g Fe2O3

223 g Fe, 96.0 g O 2, 319 g Fe 2O 3

Using atomic notation, indicate the isotope having 11 p +, 12 n 0, and 11 e -. 23/11 Na 23/12 Mg 23/12 Na 12/11 Mg 12/11 Na

23/11 Na

What is the total number of valence electrons in a silicate ion, SiO 3 2-? 22 20 24 40 none of the above

24

An Indy 500 car can travel 111 m/s. What is the speed of the car in miles per hour? (Given: 1 mi = 1.61 km, and 1 h = 3600 s) 643 mi/h 111 mi/h 248 mi/h 178 mi/h 400 mi/h

248 mi/h

The number with the most significant zeros is ________. 0.00002510 0.02500001 2.501 × 10-7 250000001 2.5100000

250000001

A sample of argon gas at 520 mm Hg expands from 0.150 L to 0.300 L. If the temperature remains constant, what is the final pressure in mm Hg? 260 mm Hg 1040 mm Hg 760 mm Hg 520 mm Hg none of the above

260 mm Hg

What is the total number of valence electrons in one molecule of N 2O 3? 18 11 2 28 none of the above

28

How many types of subshells are present in the third electron shell? 2 4 1 3

3

Predict the number of resonance structures for a nitrate ion, NO 3 -. 1 2 3 4 none of the above

3

Predict the number of valence electrons for a Group IIIA/13 element. 3 2 13 8 5

3

What is the coefficient of chlorine gas after balancing the following equation? __Fe( s) + __Cl 2( g) → __FeCl 3( s) 3 2 1 4 none of the above

3

Draw the structural formula for phosphorus triiodide, PI 3, and state the type of bonds in a phosphorus triiodide molecule. 3 single bonds 3 double bonds 2 single bonds and 1 double bond 1 single bond and 2 double bonds none of the above

3 single bonds

What is the ionic charge for the cobalt ion in CoN? 2+ 3+ zero 1+ none of the above

3+

How many molecules of methane are in 0.500 mol of CH 4 gas? 3.01 x 1022 molecules 3.01 x 1024 molecules 3.01 x 1023 molecules 1.20 x 1024 molecules 1.20 x 1023 molecules

3.01 x 10 23 molecules

How many atoms of carbon are contained in 47.6 g of Al 2(CO 3) 3? The molar mass of Al 2(CO 3) 3 is 233.99 g/mol. 2.96 × 1024 C atoms 1.23 × 1023 C atoms 3.68 × 1023 C atoms 1.10 × 1024 C atoms 2.87 × 1025 C atoms

3.68 × 10 23 C atoms

Chlorine, which exists in nature in two isotopic forms, has an atomic mass of 35.5 amu. This means that ________. 35Cl constitutes 75% of full chlorine atoms, 37Cl represents 25% all chlorine atoms have masses of 35.5 amu 35.5 amu is the upper limit for the mass of a chlorine atom 35Cl and 37Cl each constitute approximately 50% of all chlorine atoms

35Cl constitutes 75% of full chlorine atoms, 37Cl represents 25%

If the pressure of 50.0 mL of oxygen gas at 100 °C increases from 735 mm Hg to 925 mm Hg, what is the final volume? Assume temperature remains constant. 48.4 mL 39.7 mL 62.9 mL 51.7 mL 50.0 mL

39.7 mL

Draw the structural formula for ethylene, C 2H 4, and state the type of bonds in an ethylene molecule. 1 single bond and 4 double bonds 4 single bonds and 1 double bond 4 single bonds and 1 triple bond 5 single bonds none of the above

4 single bonds and 1 double bond

How many microliters are in 41.0 mL? 4.1 × 1010 4.10 × 104 4.1 × 103 0.041 none of the above

4.10 × 10 4

Calculate the mass (in kg) of water produced from the combustion of 1.0 gallon (3.8 L) of gasoline (C 8H 18). The density of gasoline is 0.79 g/mL. (C 8H 18 molar mass is 114.2 g/mole) 2C8H18 + 25O2 → 16CO2 + 18 H2O 0.47 18.5 4.3 8.3 0.75

4.3

If a 50.0 mL sample of xenon gas is at 0.921 atm and 27 °C, what is the volume of the gas at STP? 41.9 mL 59.7 mL 54.9 mL 49.4 mL 50.6 mL

41.9 mL

A 40.0 mL volume of ethane gas is heated from 25.0 °C to 50.0 °C. If the pressure remains constant, what is the final volume in milliliters? 20.0 mL 40.0 mL 43.4 mL 80.0 mL 36.9 mL

43.4 mL

A rare metal alloy is a superconductor at -225 °C. What is the temperature on the Kelvin scale? -498 K 498 K -225 K -48 K 48 K

48 K

Which s orbital is the largest? 1s 2s 3s 4s

4s

Predict the number of valence electrons for a phosphorus atom. 15 5 8 31 3

5

What is the coefficient of oxygen gas after balancing the following equation? __P( s) + __O 2( g) → __P 2O 5( s) 1 4 5 2 none of the above

5

The correct scientific notation for the number 500.0 is: 5.000 × 102 5.00 × 102 5 × 102 5 × 10-2 none of the above

5.000 × 10 ^2

How many grams of carbon are present in 26.2 grams of H 2CO 3? 47.3 g 5.07 g 16.8 g 11.60 g

5.07 g

Read the water level with the correct number of significant figures. 5.320 mL 5 mL 5.3 mL 5.32 mL 5.3200 mL

5.3 mL

Magnesium is one of the least dense elements ( d = 1.74 g/cm 3). What is the volume of a 10.0 g sample of the metal?\ 17.4 cm3 174 cm3 10.0 cm3 5.75 cm3 57.5 cm3

5.75 cm 3

Automobile air bags use the decomposition of sodium azide as their source of gas for rapid inflation: (2NaN 3 (s) → 2Na (s) + 3N 2 (g)) What mass (g) of NaN 3 is required to provide 26.5 L of N 2 at 22.0 °C and 1.10 atm?(FW) NaN 3 = 65.01 700. 52.2 0.807 1.21 1.10

52.2

Determine the theoretical yield of HCl if 60.0 g of BCl 3 and 37.5 g of H 2O are reacted according to the following balanced reaction. A possibly useful molar mass is BCl 3 = 117.16 g/mol. BCl 3(g) + 3 H 2O(l) → H 3BO 3(s) + 3 HCl(g) 25.3 g HCl 56.0 g HCl 132 g HCl 187 g HCl 75.9 g HCl

56.0 g HCl

Draw the electron dot formula for the nitrite ion, NO 2 -. How many nonbonding electron pairs are in a nitrite ion? 4 2 6 8 none of the above

6

What is the coefficient of water after balancing the following equation? __H 3PO 4( aq) + __Ba(OH) 2( aq) → __Ba 3(PO 4) 2( s) + __H 2O( l) 1 2 6 3 none of the above

6

How many atoms of nickel equal a mass of 58.69 g? (Refer to the Periodic Table.) 1 58.69 28 6.022 x 1023 59

6.022 x 10 23

One mol of particles of any substance contains how many particles? 6.022 × 1023 3 × 1010 106 3 × 10-10 6.022 × 10-23

6.022 × 10 23

What is the mass of solute dissolved in 50.0 g of 12.5% saline solution? 625 g 7.14 g 4.00 g 43.8 g 6.25 g

6.25 g

How many neutrons are in the nucleus of an atom of silver-107? 60 154 47 107 none of the above

60

The formula for the illegal drug cocaine is C 17H 21NO 4 (303.39 g/mol). What is the percentage of carbon in the compound? 3.959% 21.09% 67.30% 6.991% 4.618%

67.30%

Calculate the volume (in mL) of a 2.75 M solution that must be used to make 1.25 L of a 0.150 M solution. 33.0 mL 0.0330 mL 0.0682 mL 68.2 mL

68.2 mL

What is the equivalent pressure of 0.905 atm in units of mm Hg? 688 13.3 0.905 840 none of the above

688

Ethane, C 2H 6, burns to give carbon dioxide and water. What is the coefficient of oxygen in the balanced equation for the reaction? __C 2H 6( g) + __O 2( g) __CO 2( g) + __H 2O( g) 7 14 10 5 none of the above

7

If 25.0 mL of urine has a mass of 25.725 g and contains 1.929 g of solute, what is the mass/mass percent concentration of solute in the urine sample? 97.2% 3.887% 7.499% 13.34% 7.72%

7.499%

In an experiment, 1.201 g of charcoal reacts with 6.414 g of powdered sulfur. Using the conservation of mass law, predict the mass of product. C( s) + 2 S( s) -> CS 2( g) 4.408 g 14.029 g 7.615 g 8.816 g 5.213 g

7.615 g

The numerical value for (5.6 x 10 4) ÷ (7.89 x 10 2) is, with the proper number of significant figures, equal to: 71.0 70.976 7.098 x 101 71

71

The temperature of liquid nitrogen is -196 °C. What is the corresponding reading on the Kelvin scale? 146 K 48 K -91 K -127 K 77 K

77 K

A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water: Mg 3N 2 + 3H 2O → 2NH 3 + 3MgO The yield of MgO is 3.60 g. What is the percent yield in the reaction? (Hint limiting reaction)Molar masses (g/mole)Mg 3N 2 =100.95H 2O = 18.02MgO= 40.31 20.8 49.4 94.5 46.6 78.7

78.7

Draw the electron dot formula for sulfur trioxide, SO 3. How many nonbonding electron pairs are in a sulfur trioxide molecule? 6 2 8 3 none of the above

8

Propane (C 3H 8) burns in oxygen to form CO 2 and H 2O according to the following equation. How many grams of O 2 are required to burn 3.01 x 10 23 propane molecules? C 3H 8 + 5 O 2 -> 3 CO 2 + 4 H2O 160 g 64.0 g 80.0 g 40.0 g

80.0 g

What are the number of protons, neutrons, and electrons in 19/9 F 9 protons, 9 neutrons, and 10 electrons 9 protons, 9 neutrons, and 19 electrons 19 protons, 19 neutrons, and 19 electrons 9 protons, 10 neutrons, and 9 electrons

9 protons, 10 neutrons, and 9 electrons

How many C 2H 4 molecules are contained in 45.8 mg of C 2H 4? The molar mass of C 2H 4 is 28.05 g/mol 4.69 × 1023 C2H4 molecules 9.83 × 1020 C2H4 molecules 3.69 × 1023 C2H4 molecules 7.74 × 1026 C2H4 molecules 2.71 × 1020 C2H4 molecules

9.83 × 10 20 C 2H 4 molecules

What is the molar mass of caffeine, C 4H 5N 2O? 102.16 g/mol 116.17 g/mol 97.11 g/mol 43.03 g/mol 113.11 g/mol

97.11 g/mol

Which of the following descriptions of a subatomic particle is correct? A neutron has no charge and its mass is negligible. A proton has a positive charge and a negligible mass. An electron has a negative charge and a mass of approximately 1 amu. A neutron has a positive charge and a mass of approximately 1 amu. A proton has a positive charge and a mass of approximately 1 amu.

A proton has a positive charge and a mass of approximately 1 amu.

What are the products from the following double-replacement reaction? AgNO 3( aq) + NaCl( aq) → Ag3N and NaClO3 AgClO3 and NaNO2 AgClO3 and NaNO3 AgCl and NaNO2 AgCl and NaNO3

AgCl and NaNO 3

Which of the following is an exothermic reaction? - burning gasoline when driving a car - creating an explosion by detonating nitroglycerine - burning propane gas in a barbecue - All of the above are exothermic reactions.

All of the above are exothermic reactions.

Which of the following substances is NOT a solution? soda bronze homogenized milk sea water All of the above are solutions.

All of the above are solutions.

Which statement about a hypothesis is TRUE? - It can be tested by experiments. - It is a tentative interpretation or explanation. - It is part of the scientific method. - It has the potential to be proven wrong. - All of the above statements are true.

All of the above statements are true.

The following diagrams represent the reaction of A 2 (shaded spheres) with B 2 (unshaded spheres). Identify the limiting reactant and write a balanced equation for the reaction. https://blackboard.missouristate.edu/courses/1/CHM116-SP21-33226/ppg/chapter8quiz0125211209/f1q18g1.jpg B2 is the limiting reactant; A2 + 3 B2 → 2 AB3. A2 is the limiting reactant; A2 + 3 B2 → 2 AB3. B2 is the limiting reactant; A + 3 B → AB3. A2 is the limiting reactant; A + 3 B → AB3.

B 2 is the limiting reactant; A 2 + 3 B 2 → 2 AB 3.

If a mixture containing an unlimited amount of A, 3.00 moles of B and 5.00 moles of C is allowed to react according to the equation 2A + 2B + 4C 4D + 3E C will be the limiting reactant. A will be the limiting reactant. B will be the limiting reactant. both A and C are the limiting reactants.

C will be the limiting reactant.

Which probably has the lowest boiling point at 1.0 atm pressure? C5H12 C4H10 C2H6 C3H8 C6H14

C2H6

Which of the following is already in its empirical formula? C6H12O3 C22H34O10 C5H12O2 C6H6 none of the above

C5 H12 O2

A common name for galactose is cerebrose, or brain sugar. What is the molecular formula of galactose if the empirical formula is CH 2O, and the approximate molar mass is 180 g/mol? C12H22O11 CH2O6 CHO CH2O C6H12O6

C6 H12 O6

Which molecule has hydrogen bonding as the predominant intermolecular force? CO2 CH4 CH3OH C6H6 C4H10

CH 3OH

The normal boiling point of a substance is determined by its molecular mass and its intermolecular forces. Considering these two factors, predict the order of increasing boiling points for the following substances: CH4, CS2, KBr, NH3. CS2 < CH4 < KBr < NH3 NH3 < KBr < CS2 < CH4 CH4 < KBr < NH3 < CS2 CH4 < CS2 < NH3 < KBr

CH 4 < CS 2 < NH 3 < KBr

Rank the compounds NH 3, CH 4, and PH 3 in order of increasing boiling point. CH4 < PH3 < NH3 NH3 < CH4< PH3 CH4< NH3 < PH3 NH3 < PH3< CH4 PH3< NH3 < CH4

CH 4 < PH 3 < NH 3

Which molecule below has hydrogen bonding? CH3CH2OH CH4 HCl H2 all of the above

CH3CH2OH

What is the symbol of the element in Period 4 and Group 2A(2)? C Be Si Ca Mg

Ca

What is the chemical formula for the ternary compound composed of Ca 2+ and PO 4 3- ions? CaPO4 Ca6(PO4)6 Ca2(PO4)3 Ca3(PO4)2 none of the above

Ca 3(PO 4) 2

Which of the following anions will have the electronic configuration 1s 22s 22p 63s 23p 6? S2- Cl1- K1- Br1-

Cl1-

What is the chemical formula for the hypochlorite ion? ClO2- ClO3- ClO4- ClO- none of the above

ClO -

If 6.00 mol of cobalt combines with 9.00 mol of sulfur, what is the empirical formula of the cobalt sulfide product? Co6S9 Co9S6 Co2S3 Co3S2 none of the above

Co 2S 3

What is the chemical formula for cobalt(III) bromide? Co3Br2 Co3Br CoBr3 Co2Br3 none of the above

CoBr 3

What is the chemical formula for the copper(I) ion? Co2+ Co+ Cu2+ Cu+ none of the above

Cu +

15.0 g of Cu are combined with 46.0 g of HNO 3 (molar mass = 63.02), according to the reaction 3Cu + 8HNO3 -> 3Cu(NO 3)2 + 2NO + 4H2O Which reactant is limiting, and how many grams of H 2O (Molar mass = 18.02 ) are produced? Cu, 3.79 g Cu, 5.67 g HNO3, 6.13 g HNO3, 0.737 g

Cu, 5.67 g

According to the general trends in the periodic table, which of the following is the most electronegative element? S Cl O F N

F

In the molecule below, which atom has the largest partial negative charge? Cl | F-C-Br | I F Cl Br C I

F

Which of the following groups of elements has the lowest ionization energy? Group VIIIA/18 Group IA/1 Group IIB/12 Group IIA/2 Group VIIA/17

Group IA/1

What is the chemical formula for sulfuric acid? HSO4(aq) H2SO4(aq) HSO3(aq) H2SO3(aq) none of the above

H 2SO 4( aq)

What is the chemical formula for the hydrogen carbonate ion? HCO3- C2H3O2- HCO32- C2H3O22- none of the above

HCO 3 -

What substance is reduced in the following redox reaction? Co( s) + 2 HCl( aq) → CoCl 2( aq) + H 2( g) H2 CoCl2 Co HCl none of the above

HCl

Arrange the following compounds in order of increasing boiling point: HCl, HBr, HI. HI, HCl, HBr HBr, HI, HCl HCl, HI, HBr HCl, HBr, HI HI, HBr, HCl

HCl, HBr, HI

What is the chemical formula for nitric acid? H2NO2(aq) H2NO3(aq) HNO2(aq) HNO3(aq) none of the above

HNO 3( aq)

Which of the following compounds is the most viscous? (CH3CH 2OH) (CH3CH2CH2CH3) (HOCH2CH2OH) (CH3OCH2CH3) CH3CH2CH2CH3 HOCH2CH2OH CH3OCH2CH3 CH3CH2OH

HOCH2CH2OH

Which of the following elements has the highest ionization energy? Cl F H He Ne

He

Which response contains all of the following that are physical changes? I.Candle wax melts. II.Skin turns yellow when it comes in contact with nitric acid. III.Milk curdles. IV.Ice freezes to water. V.Windows fog when the temperature drops rapidly. - II and III - I, III, and V - I, IV, and V - II and IV

I, IV, and V

Which one of the following properties describes a liquid? - Its particles move very rapidly. - There is essentially no interaction between the particles. - Its particles are close together and move randomly. - It has its own shape. - It fills the entire volume of the container.

Its particles are close together and move randomly.

Which of the following elements has the most metallic character? Na K Fe Al Ca

K

What is the correct formula for a potassium ion with 18 electrons? K- P+ P- K+ none of the above

K +

Of the following, which gives the correct order for atomic radius for Ca, K, As, Ge and Kr? Kr > As > Ge > Ca > K Ge > As > Kr > K > Ca Ca > K > As > Ge > Kr Kr > Ge > As > K > Ca K > Ca > Ge > As > Kr

K > Ca > Ge > As > Kr

What unit of temperature is used in gas law calculations? Kelvin Celsius Fahrenheit either Celsius or Fahrenheit either Celsius or Kelvin

Kelvin

What is the chemical formula for lithium fluoride? LiF3 LiF2 Li3F2 LiF none of the above

LiF

Predict which of the following has an ionic bond. HI LiH IBr all of the above none of the above

LiH

Which of the following elements has only 12 protons? C O Mg Zn none of the above

Mg

Which element has the following electron configuration: [Ar] 4 s 2 3 d 5? Cl Kr Tc Mn Br

Mn

What is the chemical formula for laughing gas, dinitrogen oxide? N2O N2O2 NO NO2 none of the above

N 2O

Which of the following elements has the largest atomic radius? Li Na Be B Mg

Na

If 0.587 g of nickel metal reacts with 1.065 g of chlorine gas, what is the empirical formula of the nickel chloride product? NiCl3 Ni3Cl2 NiCl NiCl2 Ni2Cl3

NiCl 3

What is the major component of the air we breathe? nitrogen argon smog oxygen carbon dioxide

Nitrogen

Which of the following is true of the intermolecular attractions in liquids? Nonpolar molecules are attracted by dipole forces. Nonpolar molecules are attracted by hydrogen bonds. Nonpolar molecules are attracted by dispersion forces. all of the above none of the above

Nonpolar molecules are attracted by dispersion forces.

What is the chemical formula for the oxide ion? O2- O22- O- O2- none of the above

O 2-

[Ne]3s 23p 3 is the electron configuration of a(n) ________ atom. Sn As V Sb P

P

To solve problems using Boyle's Law, which mathematical equation should be used? P1V1 = P2V2 P2V1 = P1V2 none of the above

P 1V 1 = P 2V 2

A compound is found to be 43.7% phosphorus and 56.3% oxygen. Given the molecular mass as 285, calculate the empirical and molecular formulas. PO2; P4O8 P4O10; P4O10 P2O3; P6O9 P2O5; P4O10

P2 O5; P4 O10

Which element pair is incorrect? - Hg - mercury - Pb - iron - Au - gold - Ag - silver - Mg - magnesium

Pb - Iron

Considering the following precipitation reaction:Pb(NO 3) 2(aq) + 2KI(aq) → PbI 2(s) + 2KNO 3(aq)What is the correct net ionic equation? 2NO3- + 2K+ → 2KNO3 Pb2+ + I2- → PbI2(s) Pb2+ + 2NO3- + 2K+ + 2I- → PbI2(s) + 2K+ + 2NO3- Pb2+ + 2I- → PbI2(s) none of the above

Pb 2+ + 2I - → PbI 2(s)

Considering the following precipitation reaction:Pb(NO 3) 2(aq) + 2KI(aq) → PbI 2(s) + 2KNO 3(aq)Which ion(s) would NOT be spectator ions? K+, I- Pb2+, NO3- NO3-, Pb2+ Pb2+, I - All the above ions are in the net ionic equation.

Pb 2+, I -

All of the following compounds are soluble in water EXCEPT: NH4Cl. FeCl3. NaCl. CaCl2. PbCl2.

PbCl 2.

Energy that is associated with the position or composition of an object is called - chemical energy. - thermal energy. - potential energy. - kinetic energy.

Potential energy

What is the chemical formula for the sulfite ion? SO4- SO42- SO3- SO32- none of the above

SO 3 2-

The compound sodium sulfate is soluble in water. When this compound dissolves in water, which ion listed below would be present in solution? S2- SO42- O2- Na22+ none of the above

SO 4 2-

Which element has the following electron configuration: [Kr] 5 s 2 4 d 10 5 p 2? Sn Xe Pb Sr Zr

Sn

Which of the statements below best describes the following reaction? Na 2CO 3( s) ->Na 2O( s) + CO 2( g) Sodium carbonate decomposes with heat. Sodium carbonate decomposes to sodium oxide and carbon dioxide. Sodium carbonate is heated to give sodium oxide and carbon dioxide. Sodium carbonate decomposes to sodium oxide and carbon dioxide gas. Solid sodium carbonate is heated to give solid sodium oxide andcarbon dioxide gas.

Solid sodium carbonate is heated to give solid sodium oxide andcarbon dioxide gas.

What is the predicted product from the following combination reaction? Sr( s) + Br 2( l) Sr2Br Sr2Br3 Sr3Br2 SrBr SrBr2

SrBr 2

When solid NaCl is stirred into water, which of the following is NOT true? The solution will conduct electricity. Individual sodium and chloride ions are present. The solution will taste salty. The NaCl will fail to dissociate. none of the above

The NaCl will fail to dissociate.

A fictional element has two naturally occurring isotopes with the natural abundances shown here: Isotope Abundance 16 50.0% 18 50.0% The atomic mass would be more than 18. The atomic mass would be 18. The atomic mass would be 17. The atomic mass would be 16. The atomic mass would be less than 16.

The atomic mass would be 17.

According to Gay-Lussac's law, what happens to a gas as temperature increases? The volume decreases. The pressure decreases. The volume increases. The pressure increases. none of the above

The pressure increases.

If a helium balloon is placed in a cold freezer, what happens in the balloon? The temperature decreases and the volume decreases. The temperature decreases and the volume increases. The temperature increases and the volume increases. The temperature increases and the volume decreases. none of the above

The temperature decreases and the volume decreases.

According to Charles's law, what happens to a gas as temperature increases? The pressure increases. The pressure decreases. The volume decreases. The volume increases. none of the above

The volume increases.

Which of the following is NOT true for the atoms 13N, 14N, and 15N? They all have the same atomic number. They all have 7 protons. They are isotopes. They all have the same mass number. They all have 7 electrons.

They all have the same mass number.

Of the following, ________ radiation has the shortest wavelength. radio ultraviolet infrared microwave X-ray

X-ray

What substance is oxidized in the following redox reaction? Zn( s) + Cu 2+( aq) → Zn 2+( aq) + Cu( s) Zn2+ Cu2+ Zn Cu none of the above

Zn

What is the chemical formula for the ternary compound composed of Zn 2+ and OH - ions? ZnOH2 ZnOH Zn2OH Zn(OH)2 none of the above

Zn(OH) 2

When an atom loses an electron, the resulting particle is called: a cation. a proton. an anion. an isotope. none of the above

a cation.

Which of the following is a base unit and symbol in the metric system? meter (m) liter (L) gram (g) all of the above none of the above

all of the above

What is the systematic name for NH 4Cl? nitrogen tetrahydrogen chloride tetraammonium chloride ammonium chloride ammonium tetrachloride none of the above

ammonium chloride

The elements lithium, sodium, and potassium ________. have the same number of neutrons have the same mass number are isotopes of each other are in the same group are in the same period of elements

are in the same group

According to the kinetic molecular theory of gases, particles of a gas are very far apart. decrease in kinetic energy as temperature increases. move slowly. are very large particles. lose their valence electrons.

are very far apart.

Isotopes are: atoms of the same element that have different number of electrons. atoms of the same element that have different number of neutrons. atoms of the same element that have the same number of neutrons. atoms of the same element that have different number of protons. none of the above

atoms of the same element that have different number of neutrons.

What is the molecular shape of a water molecule, H 2 O? bent trigonal pyramidal linear tetrahedral none of the above

bent

Which process absorbs energy? - bond breaking - bond formation - both A and B - none of the above

bond breaking

Boron occurs naturally as 10B and 11B. Which isotope is more abundant?(Hint: Refer to the Periodic Table.) boron-11 boron-5 boron-10 boron-6 none of the above

boron-11

If the products have a higher energy than the reactants ________. - the reaction is exothermic - the reactants have less energy than the products - the reaction is endothermic - both B and C

both b and c

Which types of subshells are allowed in the n=2 energy level? both s and p p d s

both s and p

What is the systematic name for CdI 2? cadmium(II) iodide cadmium iodide cadmium(I) iodide cadmium diiodide none of the above

cadmium(II) iodide

What type of chemical reaction is illustrated in the following example? SO 2( g) + O 2( g) → SO 3( g) double-replacement reaction single-replacement reaction decomposition reaction combination reaction neutralization reaction

combination reaction

Which of the following type of matter/classification of matter pairs is incorrectly matched? type of matterclassification of matter concrete homogeneous mixture pure gold element saline solution homogeneous mixture fruitcake heterogeneous mixture

concrete homogeneous mixture

An isotope represented as S-34: contains exactly 18 neutrons. must have exactly 18 electrons. is an isotope of sodium. has 34 protons. none of the above

contains exactly 18 neutrons.

Which of the following is a compound? - iron - copper - magnesium - copper (II) oxide

copper (II) oxide

Which of the following is a general trend in the periodic table for the metallic character of the elements? - decreases from left to right, increases from bottom to top - increases from left to right, increases from bottom to top - decreases from left to right, decreases from bottom to top - increases from left to right, decreases from bottom to top - none of the above

decreases from left to right, decreases from bottom to top

The solubility of gases in water: is independent of temperature. decreases with increasing temperature. increases with increasing temperature. gases are not soluble in water. none of the above

decreases with increasing temperature.

What is the systematic name for Cl 2O 7? chlorine heptaoxide dichlorine heptaoxide dichlorine hexaoxide chlorine hexaoxide none of the above

dichlorine heptaoxide

In a liquid sample of NCl 3, what is the dominant intermolecular force present? hydrogen bonding London forces dipole-dipole interactions instantaneous bonding

dipole-dipole interactions

What type(s) of intermolecular forces exist between Cl 2 and CCl 4? dispersion forces and dipole-dipole dispersion forces dispersion forces and ion-dipole dispersion forces, ion-dipole, and dipole-dipole None. Since both are gases at room temperature, they do not interact with each other.

dispersion forces

Which intermolecular force is present in all molecules and atoms? dipole-dipole forces X-forces dispersion forces hydrogen bonding none of the above

dispersion forces

What types of intermolecular forces exist between NH 3 and H 2O? dispersion forces, dipole-dipole forces, and hydrogen bonds dispersion forces, hydrogen bonds, and ion-dipole forces dispersion forces dispersion forces and ion-dipole forces dispersion forces and hydrogen bonds

dispersion forces, dipole-dipole forces, and hydrogen bonds

What type of chemical reaction is illustrated in the following example? AlCl 3( aq) + AgNO 3( aq) → Al(NO 3) 3( aq) + AgCl( s) decomposition reaction combination reaction double-replacement reaction single-replacement reaction neutralization reaction

double-replacement reaction

Identify the state of matter that is the most compressible. liquid gas solid All are compressible. None is compressible.

gas

Which of the following is an example of a physical change? - digesting a hot dog - grinding pepper - burning a candle - converting hydrogen and oxygen to water - frying an egg

grinding pepper

Which of the following may not be classified as matter? - heat - tooth filling - seawater - sand

heat

Pepsi-Cola is carbonated by injection with carbon dioxide gas. Under what conditions is carbon dioxide gas least soluble? high temperature, low pressure low temperature, low pressure low temperature, high pressure high temperature, high pressure none of the above

high temperature, low pressure

Precision refers to ________. how close a measured number is to zero how close a measured number is to other measured numbers how close a measured number is to the true value how close a measured number is to infinity how close a measured number is to the calculated value

how close a measured number is to other measured numbers

What is the systematic name for aqueous HF? hydrofluoric acid hydrogen fluoride fluoric acid fluorous acid none of the above

hydrofluoric acid

What is the strongest intermolecular force in a liquid containing molecules with H-O bonds? dispersion forces covalent bonds dipole forces hydrogen bonds none of the above

hydrogen bonds

Vaporization occurs more readily with: increased temperature, increased surface area, decreased volume increased temperature, increased surface area, increased intramolecular forces increased temperature, decreased surface area, decreased intermolecular forces increased temperature, decreased surface area, decreased intermolecular forces increased temperature, increased surface area, decreased intermolecular forces

increased temperature, increased surface area, decreased intermolecular forces

Which of the following is a general trend for the electronegativity of elements in the periodic table? - increases from left to right; increases from bottom to top - decreases from left to right; increases from bottom to top - decreases from left to right; decreases from bottom to top - increases from left to right; decreases from bottom to top - none of the above

increases from left to right; increases from bottom to top

The solubility of solids in water: is independent of the temperature. decreases with increasing temperature. increases with increasing temperature. Solids are not soluble in water. none of the above

increases with increasing temperature.

The empirical formula of a compound: indicates the structure of the molecule. indicates the simplest ratio of atoms in the compound. describes the mass relationships in a molecule. is the same as the molecular formula. none of the above

indicates the simplest ratio of atoms in the compound.

There are exactly 2.54 centimeters in 1 inch. When using this conversion factor, how many significant figures are you limited to? 1 3 ambiguous depends on if you are using it in multiplication/division or addition/subtraction infinite number of significant figures

infinite number of significant figures

Which intermolecular force is the strongest? dispersion force ion-dipole force hydrogen bonding dipole-dipole force none of the above

ion-dipole force

Chemical equations are balanced in order to obey the law of mass action. definite proportions. multiple proportions. mass conservation.

mass conservation.

The number of neutrons in an atom is equal to the ________. number of protons mass number mass number + the atomic number mass number - the atomic number atomic number

mass number - the atomic number

What is the Stock system name for Hg 2Cl 2? mercurous chloride mercury(I) chloride mercury(II) chloride mercuric chloride none of the above

mercury(I) chloride

Water and methanol are two liquids which dissolve in each other. When the two are mixed they form one layer. The liquids are ________. immiscible partially miscible miscible unsaturated

miscible

What general term refers to the mass of 1 mol of any substance? molar mass gram-atomic mass gram-molecular mass gram-formula mass none of the above

molar mass

Molarity could be used as a conversion factor between ________. moles of solute and volume of solution grams of solute and volume of solution grams of solute and moles of solvent moles of solute and kilograms of solute

moles of solute and volume of solution

What type of chemical reaction is illustrated in the following example? HClO 4( aq) + KOH( aq) → KClO 4( aq) + H 2O( l) single-replacement reaction combination reaction double-replacement reaction decomposition reaction neutralization reaction

neutralization reaction

Group 8A elements are also called: noble gases. halogens. alkaline earth metals. alkali metals. none of the above

noble gases.

Which of the following chemical elements corresponds to the symbol A? - arsenic - antimony - argon - aluminum - none of the above

none of the above

Which of the following increases the pressure of a gas? increasing the volume decreasing the number of gas molecules decreasing the temperature all of the above none of the above

none of the above

Which of the following is true according to the kinetic theory of gases? Molecules remain in fixed positions. Molecules are attracted to one another. Molecules lose energy after colliding. all of the above none of the above

none of the above

Which ingredient is the limiting reactant if you have 6 cups of flour, 9 eggs and 2 tbs of oil? Given: 2 cups flour + 3 eggs + 1 tbs oil → 4 waffles flour oil waffles eggs not enough information

oil

The NH 4 + ion is classified as which of the following? monoatomic cation monoatomic anion polyatomic anion polyatomic cation none of the above

polyatomic cation

A reaction which forms a solid product is an example of a(n): precipitation reaction. gas evolution reaction. oxidation-reduction reaction. combustion reaction. none of the above

precipitation reaction.

Which subatomic particle has a relative charge of +1 and a mass of about 1 amu ? alpha neutron proton electron none of the above

proton

The nucleus of an atom consists mainly of: protons and neutrons. protons, neutrons, and electrons. neutrons and electrons. protons and electrons. none of the above

protons and neutrons.

Nonmetals are located where on the periodic table? left side right side middle zig-zag diagonal line none of the above

right side

In this list, which substance can be classified as a chemical? - sleep - salt - temperature - cold - heat

salt

Which of the following chemical elements corresponds to the symbol Ag? - argon - gold - silver - mercury - none of the above

silver

In water, a substance that ionizes completely in solution is called a ________. nonconductor strong electrolyte weak electrolyte semiconductor nonelectrolyte

strong electrolyte

Which of the following elements is a metal? fluorine argon phosphorus strontium nitrogen

strontium

Paradichlorobenzene, a material used in "moth balls," is known to go directly from a solid form to a gaseous form. This process is known as: melting boiling condensation sublimation evaporation

sublimation

What is the electron pair geometry for a phosphine molecule, PH 3? trigonal pyramidal tetrahedral bent linear none of the above

tetrahedral

What is the electron pair geometry for a water molecule, H2O? tetrahedral bent trigonal pyramidal linear none of the above

tetrahedral

The molecular geometry of the CHF 3 molecule is ________, and the molecule is ________. seesaw, nonpolar seesaw, polar trigonal pyramidal, polar tetrahedral, polar tetrahedral, nonpolar

tetrahedral, polar

Atoms are neutral because ________. the atomic number equals the number of electrons equal numbers of protons and neutrons are present neutrons neutralize the (+) and (−) charges in the atom all atoms contain neutrons

the atomic number equals the number of electrons

An international group of zookeepers with successful breeding programs made the following animal exchanges last year. Using the same bartering system, how many oryxes can a zoo obtain in exchange for 15 flamingos? five oryxes four oryxes one oryx three oryxes

three oryxes

The molecular geometry of the right-most carbon in the molecule below is ________. (picture) trigonal planar octahedral tetrahedral T-shaped trigonal bipyramidal

trigonal planar

What is the molecular shape of a carbonate ion, CO 3 2-? bent trigonal planar tetrahedral trigonal pyramidal linear

trigonal planar

What is the molecular shape of a phosphine molecule, PH 3? tetrahedral linear bent trigonal pyramidal none of the above

trigonal pyramidal

Draw the structural formula for the cyanide ion, C N -, and state the type of bond in a cyanide ion. single bond double bond ionic bond triple bond none of the above

triple bond

The solubility of Pb(NO 3) 2 is 55 grams per 100 g H 2O at 20°C. Which term would properly describe a solution where 44 grams of Pb(NO 3) 2 is added to 100 grams of water at this temperature? insoluble unsaturated saturated supersaturated none of the above

unsaturated

If the molecules in a liquid have a strong attraction for each other, which of the following properties has a relatively low value? boiling point vapor pressure viscosity surface tension all of the above

vapor pressure

Which of the following is an example of potential energy? - riding an exercise bike - chewing food - burning wood - water stored in a reservoir - a fan blade turning

water stored in a reservoir