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Chemistry: A Molecular Approach, 2e (Tro)
Chapter 4 Chemical Quantities and Aqueous Reactions
1) Global warming is thought to be caused by the increase of one particular gas. Name the gas.
A) oxygen
B) carbon monoxide
C) carbon dioxide
D) nitrogen
E) helium
2) How many grams of Li3N can be formed from 1.75 moles of Li? Assume an excess of nitrogen.
6 Li(s) + N2(g) → 2 Li3N(s)
A) 18.3 g Li3N
B) 20.3 g Li3N
C) 58.3 g Li3N
D) 61.0 g Li3N
E) 15.1 g Li3N
3) How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the
following reaction? The molar mass of KNO3 is 101.11 g/mol.
4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)
A) 0.290 mol O2
B) 0.580 mol O2
C) 18.5 mol O2
D) 0.724 mol O2
E) 1.73 mol O2
4) How many moles of nitrogen are formed when 58.6 g of KNO3 decomposes according to the
following reaction? The molar mass of KNO3 is 101.11 g/mol.
4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)
A) 0.290 mol N2
B) 0.580 mol N2
C) 18.5 mol N2
D) 0.724 mol N2
E) 1.73 mol N2
5) Two samples of calcium fluoride are decomposed into their constituent elements. The first sample
produced 0.154 g of calcium and 0.146 g of fluorine. If the second sample produced 294 mg of fluorine,
how many g of calcium were formed?
A) 0.280 g
B) 3.09 × 102 g
C) 3.13 g
D) 0.309 g
E) 2.80 × 102 g
6) Two samples of potassium iodide are decomposed into their constituent elements. The first sample
produced 13.0 g of potassium and 42.3 g of iodine. If the second sample produced 24.4 kg of potassium,
how many kg of iodine were produced?
A) 13.3 kg
B) 22.5 kg
C) 79.4 kg
D) 44.4 kg
E) 92.4 kg
7) A 14.01 g sample of N2 reacts with 3.02 g of H2 to form ammonia (NH3). If ammonia is the only
product, what mass of ammonia is formed?
A) 17.01 g
B) 1.10 g
C) 14.01 g
D) 3.02 g
E) 23.07 g
8) Consider the following balanced reaction. How many grams of water are required to form 75.9 g of
HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02
g/mol, HNO3 = 63.02 g/mol.
3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
A) 38.0 g H2O
B) 21.7 g H2O
C) 43.4 g H2O
D) 10.9 g H2O
E) 26.5 g H2O
9) Consider the following reaction. How many moles of oxygen are required to produce 2.33 moles of
water? Assume that there is excess C3H7SH present.
C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O(g)
A) 1.55 moles O2
B) 3.50 moles O2
C) 2.33 moles O2
D) 4.14 moles O2
E) 6.21 moles O2
10) Consider the following balanced reaction. What mass (in g) of CO2 can be formed from 288 mg of
O2? Assume that there is excess C3H7SH present.
C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O(g)
A) 0.396 g CO2
B) 0.209 g CO2
C) 0.792 g CO2
D) 0.126 g CO2
E) 0.198 g CO2
11) According to the following reaction, how many grams of sulfur are formed when 37.4 g of water are
formed?
2 H2S(g) + SO2(g) → 3 S(s) + 2H2O(l)
A) 99.8 g S
B) 66.6 g S
C) 56.1 g S
D) 44.4 g S
E) 14.0 g S
12) How many molecules of H2S are required to form 79.0 g of sulfur according to the following
reaction? Assume excess SO2.
2 H2S(g) + SO2(g) → 3 S(s) + 2H2O(l)
A) 1.48 × 1024 molecules H2S
B) 9.89 × 1023 molecules H2S
C) 5.06 × 1025 molecules H2S
D) 3.17 × 1025 molecules H2S
E) 2.44 × 1023 molecules H2S
13) Give the theoretical yield, in moles, of CO2 from the reaction of 4.00 moles of C8H18 with 4.00
moles of O2.
2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
A) 0.640 moles
B) 64.0 moles
C) 2.56 moles
D) 16.0 moles
14) A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride
(PCl3). If it is the only product, what mass of PCl3 is formed?
A) 30.15 g
B) 54.93 g
C) 140.01 g
D) 79.71 g
E) 91.86 g
15) Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g
N2O4 and 45.0 g N2H4. Some possibly useful molar masses are as follows: N2O4 = 92.02 g/mol,
N2H4 = 32.05 g/mol.
N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g)
A) LR = N2H4, 59.0 g N2 formed
B) LR = N2O4, 105 g N2 formed
C) LR = N2O4, 45.7 g N2 formed
D) LR = N2H4, 13.3 g N2 formed
E) No LR, 45.0 g N2 formed
16) Determine the theoretical yield of HCl if 60.0 g of BCl3 and 37.5 g of H2O are reacted according to
the following balanced reaction. A possibly useful molar mass is BCl3 = 117.16 g/mol.
BCl3(g) + 3 H2O(l) → H3BO3(s) + 3 HCl(g)
A) 75.9 g HCl
B) 132 g HCl
C) 187 g HCl
D) 56.0 g HCl
E) 25.3 g HCl
17) According to the following reaction, what amount of Al2S3 remains when 20.00 g of Al2S3 and
2.00 g of H2O are reacted? A few of the molar masses are as follows: Al2S3 = 150.17 g/mol, H2O =
18.02 g/mol.
Al2S3(s) + 6 H2O(l) → 2 Al(OH)3(s) + 3 H2S(g)
A) 28.33 g
B) 14.00 g
C) 8.33 g
D) 19.78 g
E) 17.22 g
18) Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18
with 4.000 moles of O2.
2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
A) 20.00%
B) 25.00%
C) 50.00%
D) 12.50%
19) Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18
with 8.000 moles of O2.
2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
A) 20.00%
B) 25.00%
C) 50.00%
D) 12.50%
20) Give the percent yield when 28.16 g of CO2 are formed from the reaction of 8.000 moles of C8H18
with 4.000 moles of O2.
2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
A) 20.00%
B) 25.00%
C) 50.00%
D) 12.50%
21) Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe2O3 react
with excess Al according to the following reaction.
Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s)
A) 61.03 %
B) 28.65 %
C) 57.30 %
D) 20.02 %
E) 81.93 %
22) Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield
750.0 mL of solution.
A) 1.50 M
B) 1.18 M
C) 0.130 M
D) 0.768 M
E) 2.30 M
23) Determine the molarity of a solution formed by dissolving 468 mg of MgI2 in enough water to yield
50.0 mL of solution.
A) 0.0297 M
B) 0.0337 M
C) 0.0936 M
D) 0.0107 M
E) 0.0651 M
24) How many molecules of sucrose (C12H22O11, molar mass = 342.30 g/mol) are contained in 14.3
mL of 0.140 M sucrose solution?
A) 8.29 × 1022 molecules C12H22O11
B) 1.21 × 1021 molecules C12H22O11
C) 6.15 × 1022 molecules C12H22O11
D) 1.63 × 1023 molecules C12H22O11
E) 5.90 × 1024 molecules C12H22O11
25) According to the following reaction, how many moles of Fe(OH)2 can form from 175.0 mL of 0.227
M LiOH solution? Assume that there is excess FeCl2.
FeCl2(aq) + 2 LiOH(aq) → Fe(OH)2(s) + 2 LiCl(aq)
A) 3.97 × 10-2 moles
B) 2.52 × 10-2 moles
C) 1.99 × 10-2 moles
D) 5.03 × 10-2 moles
E) 6.49 × 10-2 moles
26) According to the following reaction, what volume of 0.244 M KCl solution is required to react
exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution?
2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)
A) 97.4 mL
B) 116 mL
C) 43.0 mL
D) 86.1 mL
E) 58.1 mL
27) According to the following reaction, what mass of PbCl2 can form from 235 mL of 0.110 M KCl
solution? Assume that there is excess Pb(NO3)2.
2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)
A) 7.19 g
B) 3.59 g
C) 1.80 g
D) 5.94 g
E) 1.30 g
28) Determine the number of grams H2 formed when 250.0 mL of 0.743 M HCl solution reacts with
3.41 x 1023 atoms of Fe according to the following reaction.
2 HCl(aq) + Fe(s) → H2(g) + FeCl2(aq)
A) 0.374 g
B) 1.33 g
C) 1.14 g
D) 0.187 g
E) 1.51 g
29) What volume of 0.305 M AgNO3 is required to react exactly with 155.0 mL of 0.274 M Na2SO4
solution? Hint: You will want to write a balanced reaction.
A) 581 mL
B) 173 mL
C) 345 mL
D) 139 mL
E) 278 mL
30) What mass (in g) of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC2H3O2 solution
with 55.0 mL of 0.109 M MgCl2 solution?
2 AgC2H3O2(aq) + MgCl2(aq) → 2 AgCl(s) + Mg(C2H3O2)2(aq)
A) 0.838 g
B) 1.72 g
C) 0.859 g
D) 2.56 g
E) 1.70 g
31) Identify acetic acid.
A) strong electrolyte, weak acid
B) weak electrolyte, weak acid
C) strong electrolyte, strong acid
D) weak electrolyte, strong acid
E) nonelectrolyte
32) Identify HCl.
A) strong electrolyte, weak acid
B) weak electrolyte, weak acid
C) strong electrolyte, strong acid
D) weak electrolyte, strong acid
E) nonelectrolyte
33) Choose the statement below that is TRUE.
A) A weak acid solution consists of mostly nonionized acid molecules.
B) The term "strong electrolyte" means that the substance is extremely reactive.
C) A strong acid solution consists of only partially ionized acid molecules.
D) The term "weak electrolyte" means that the substance is inert.
E) A molecular compound that does not ionize in solution is considered a strong electrolyte.
34) Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of
lithium sulfide and copper (II) nitrate are mixed.
A) Li+(aq) + SO42-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + Li+(aq) + NO3-(aq)
B) Li+(aq) + S-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + LiNO3(aq)
C) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → Cu2+(aq) + S2-(aq) + 2 LiNO3(s)
D) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq)
E) No reaction occurs.
35) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of K2S and
Fe(NO3)2 are mixed.
A) K+(aq) + NO3-(aq) → KNO3(s)
B) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → FeS(s) + 2 K+(aq) + 2 NO3-(aq)
C) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → Fe2+(aq) + S2-(aq) + 2 KNO3(s)
D) Fe2+(aq) + S2-(aq) → FeS(s)
E) No reaction occurs.
36) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of H2SO4
and KOH are mixed.
A) H+(aq) + OH-(aq) → H2O(l)
B) 2 K+(aq) + SO42-(aq) → K2SO4(s)
C) H+(aq) + OH-(aq) + 2 K+(aq) + SO42-(aq) → H2O(l) + K2SO4(s)
D) H22+(aq) + OH-(aq) → H2(OH)2(l)
E) No reaction occurs.
37) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of
Al(C2H3O2)3 and LiNO3 are mixed.
A) Al3+(aq) + 3 NO3-(aq) → Al(NO3)3(s)
B) Li+(aq) + C2H3O2-(aq) → LiC2H3O2(s)
C) Al3+(aq) + 3 NO3-(aq) + Li+(aq) + C2H3O2-(aq) → Al(NO3)3(aq) + LiC2H3O2(s)
D) 3 Li+(aq) + (C2H3O2)33-(aq) → Li3(C2H3O2)3(s)
E) No reaction occurs.
38) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3
and HCl are mixed.
A) 2 H+(aq) + CO32-(aq) → H2CO3(s)
B) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 NaCl(aq)
C) 2 H+(aq) + CO32-(aq) → H2O(l) + CO2(g)
D) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 Na+(aq) + 2 Cl-(aq)
E) No reaction occurs.
39) Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of
MgSO3 and HI are mixed.
A) 2 H+(aq) + SO32-(aq) → H2SO3(s)
B) Mg2+(aq) + 2 I-(aq) → MgI2(s)
C) 2 H+(aq) + SO32-(aq) + Mg2+(aq) + 2 I-(aq)→ H2SO3(s) + MgI2(aq)
D) 2 H+(aq) + SO32-(aq) → H2O(l) + SO2(g)
E) No reaction occurs.
40) Which of the following is an acid-base reaction?
A) C(s) + O2(g) → CO2(g)
B) 2 HClO4(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(ClO4)2(aq)
C) Fe(s) + 2 AgNO3(aq) → 2 Ag(s) + Fe(NO3)2(aq)
D) MgSO4(aq) + Ba(NO3)2(aq) → Mg(NO3)2(aq) + BaSO4(s)
E) None of the above are acid base reactions.
41) Which of the following is a gas-evolution reaction?
A) 2 C2H6(l) + 7 O2(g) → 4 CO2(g) + 6 H2O(g)
B) 2 H2(g) + O2(g) → 2 H2O(g)
C) LiCl(aq) + NaNO3(aq) → LiNO3(aq) + NaCl(g)
D) NH4Cl(aq) + KOH(aq) → KCl(aq) + NH3(g) + H2O(l)
E) None of the above are gas-evolution reactions.
42) The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of 0.12 M
LiOH solution. What is the concentration of the H2SO4 solution (in M)?
A) 0.20 M
B) 0.40 M
C) 0.10 M
D) 0.36 M
E) 0.25 M
43) The titration of 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL of 0.218 M
KOH solution. What is the concentration of the H3PO4 solution (in M)?
A) 1.03 M
B) 0.343 M
C) 0.114 M
D) 0.138 M
E) 0.0461 M
44) Choose the reaction that represents the combustion of C6H12O2.
A) C6H12O2(l) + 8 O2(g) → 6 CO2(g) + 6 H2O(g)
B) Mg(s) + C6H12O2(l) → MgC6H12O2(aq)
C) 6 C(s) + 6 H2(g) + O2(g) → C6H12O2(l)
D) C6H12O2(l) → 6 C(s) + 6 H2(g) + O2(g)
E) None of the above represent the combustion of C6H12O2.
45) Determine the oxidation state of P in PO33-.
A) +3
B) +6
C) +2
D) 0
E) -3
46) Determine the oxidation state of C in CO3-2.
A) +4
B) +2
C) -2
D) -4
E) +6
47) Determine the oxidation state of nitrogen in NO.
A) +5
B) +3
C) 0
D) +2
E) +4
48) Determine the oxidation state of nitrogen in NO2.
A) +5
B) +3
C) 0
D) +2
E) +4
49) What element is undergoing oxidation (if any) in the following reaction?
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)
A) O
B) H
C) C
D) both C and H
E) None of the elements is undergoing oxidation.
50) What element is undergoing reduction (if any) in the following reaction?
Zn(s) + 2 AgNO3(aq) → Zn(NO3)2(aq) + 2 Ag(s)
A) Zn
B) N
C) O
D) Ag
E) This is not an oxidation-reduction reaction.
51) What element is undergoing oxidation (if any) in the following reaction?
Zn(s) + 2 AgNO3(aq) → Zn(NO3)2(aq) + 2 Ag(s)
A) Zn
B) N
C) O
D) Ag
E) This is not an oxidation-reduction reaction.
52) Determine the reducing agent in the following reaction.
2 Li(s) + Fe(C2H3O2)2(aq) → 2 LiC2H3O2(aq) + Fe(s)
A) O
B) H
C) C
D) Fe
E) Li
53) Determine the oxidizing agent in the following reaction.
Ni(s) + 2 AgClO4(aq) → Ni(ClO4)2(aq) + 2 Ag(s)
A) Ag
B) Ni
C) Cl
D) O
E) This is not an oxidation-reduction reaction.
Algorithmic Questions
1) According to the following balanced reaction, how many moles of NO are formed from 8.44 moles of
NO2 if there is plenty of water present?
3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
A) 25.32 moles NO
B) 12.66 moles NO
C) 8.44 moles NO
D) 5.63 moles NO
E) 2.82 moles NO
2) According to the following balanced reaction, how many moles of HNO3 are formed from 8.44 moles
of NO2 if there is plenty of water present?
3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
A) 25.32 moles NO
B) 12.66 moles NO
C) 8.44 moles NO
D) 5.63 moles NO
E) 2.82 moles NO
3) Consider the following reaction. How many moles of oxygen are required to produce 10.0 moles of
water? Assume that there is excess C3H7SH present.
C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O(g)
A) 6.67 moles O2
B) 15.0 moles O2
C) 10.0 moles O2
D) 40.0 moles O2
E) 2.50 moles O2
4) According to the following balanced reaction, how many moles of KO are required to exactly react
with 5.44 moles of H2O?
4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g)
A) 5.44 moles H2O
B) 10.9 moles H2O
C) 21.8 moles H2O
D) 2.72 moles H2O
E) 1.36 moles H2O
5) According to the following balanced reaction, how many moles of KOH are required to exactly react
with 5.44 moles of H2O?
4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g)
A) 5.44 moles H2O
B) 10.9 moles H2O
C) 21.8 moles H2O
D) 2.72 moles H2O
E) 1.36 moles H2O
6) How many grams of oxygen are formed when 6.21 moles of KOH are formed?
4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g)
A) 6.21 g O2
B) 24.8 g O2
C) 49.7 g O2
D) 199 g O2
E) 99.4 g O2
7) How many molecules of HCl are formed when 80.0 g of water reacts according to the following
balanced reaction? Assume excess ICl3.
2 ICl3 + 3 H2O → ICl + HIO3 + 5 HCl
A) 4.46 × 1024 molecules HCl
B) 2.68 × 1024 molecules HCl
C) 8.04 × 1024 molecules HCl
D) 5.36 × 1024 molecules HCl
E) 4.46 × 1025 molecules HCl
8) Carbonic acid can form water and carbon dioxide upon heating. How much carbon dioxide is formed
from 24.8 g of carbonic acid?
H2CO3 → H2O + CO2
A) 17.6 g
B) 34.9 g
C) 24.8 g
D) 7.20 g
E) 85.4 g
9) Lithium and nitrogen react to produce lithium nitride:
6Li(s) + N2(g) → 2Li3N(s)
How many moles of N2 are needed to react with 0.500 mol of lithium?
A) 3.00
B) 0.500
C) 0.167
D) 1.50
E) 0.0833
10) Lithium and nitrogen react to produce lithium nitride:
6Li(s) + N2(g) → 2Li3N(s)
How many moles of lithium nitride are produced when 0.450 mol of lithium react in this fashion?
A) 0.150
B) 0.900
C) 0.0750
D) 1.35
E) 0.225
11) Lithium and nitrogen react in a combination reaction to produce lithium nitride:
6Li(s) + N2(g) → 2Li3N(s)
How many moles of lithium are needed to produce 0.60 mol of Li3N when the reaction is carried out in
the presence of excess nitrogen?
A) 0.30
B) 1.8
C) 0.20
D) 0.40
E) 3.6
12) Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements:
2NaN3(s) → 2Na(s) + 3N2 (g)
How many moles of N2 are produced by the decomposition of 2.88 mol of sodium azide?
A) 1.92
B) 8.64
C) 4.32
D) 0.960
E) 1.44
13) Magnesium burns in air with a dazzling brilliance to produce magnesium oxide:
2Mg(s) + O2(g) → 2MgO(s)
How many moles of O2 are consumed when 0.770 mol of magnesium burns?
A) 0.0317
B) 2.60
C) 0.770
D) 1.54
E) 0.385
14) Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements:
2NaN3(s) → 2Na(s) + 3N2 (g)
How many grams of sodium azide are required to produce 33.0 g of nitrogen?
A) 1.77
B) 0.785
C) 76.6
D) 51.1
E) 114.9
15) How many moles of CuO can be produced from 0.900 mol of Cu2O in the following reaction?
2 Cu2O(s) + O2(g) → 4 CuO(s)
A) 0.450 mol
B) 0.900 mol
C) 1.80 mol
D) 3.60 mol
16) How many moles of BCl3 are needed to produce 10.0 g of HCl(aq) in the following reaction?
BCl3(g) + 3 H2O(l) → 3 HCl(aq) + B(OH)3(aq)
A) 0.0914 mol
B) 0.274 mol
C) 0.823 mol
D) 10.9 mol
17) How many grams of calcium chloride are needed to produce 1.50 g of potassium chloride?
CaCl2(aq) + K2CO3(aq) → 2 KCl(aq) + CaCO3(aq)
A) 0.896 g
B) 1.12 g
C) 2.23 g
D) 4.47 g
18) Balance the chemical equation given below, and determine the number of moles of iodine that reacts
with 30.0 g of aluminum.
_____ Al(s) + _____ I2(s) → _____ Al2I6(s)
A) 0.741 mol
B) 1.67 mol
C) 2.22 mol
D) 3.33 mol
19) Balance the chemical equation given below, and determine the number of grams of MgO are needed
to produce 10.0 g of Fe2O3.
_____ MgO(s) + _____ Fe(s) → _____ Fe2O3(s) + _____ Mg(s)
A) 0.312 g
B) 0.841 g
C) 2.52 g
D) 7.57 g
20) Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas. How many grams of
oxygen are formed when 10.0 g of dinitrogen monoxide decomposes?
A) 0.275 g
B) 3.64 g
C) 7.27 g
D) 14.5 g
