CHM 2045 F18 Test 2 Learning Objective Practices
Chapter 4
7. Define and identify: reduction, oxidation, reducing agent, oxidizing agent and redox
reactions. (4.2)
(1) In the reaction Cl2 (aq) + 2 I− (aq) → 2 Cl− (aq) + I2 (aq), the oxidizing agent is:
A) I2 B) I− C) Cl2 D) H2O E) Cl−
(2) Considering the following reaction, which statement is incorrect?
Cu (s) + 4 H+ (aq) + 2 NO3− (aq) → Cu2+ (aq) + 2 NO2(g) + 2 H2O(l)
2+
A) Cu is the result of an oxidation.
B) Cu is the reducing agent.
C) NO3- is reduced.
D) Cu is reduced.
E) NO3- is the oxidizing agent.
(3) Which reaction type is incorrectly labeled?
A) Ca2+(aq) + SO42-(aq) → CaSO4 (s), acid-base reaction
B) C2H4 (g) + 3 O2 (g) → 2 CO2 (g) + 2 H2O (g), oxidation-reduction
C) Fe (s) + 2 H+ (aq) → Fe2+ (aq) + H2 (g), oxidation-reduction
D) Fe3+ (aq) + PO43- (aq) → FePO4 (s), precipitation
E) NH3 (aq) + HCl(aq) → NH4+(aq) + Cl−(aq), acid-base reaction
(4) Which is the reducing agent in the following redox reaction:
5 Fe2+(aq) + MnO4-(aq) + 8 H+(aq) → Mn2+(aq) + 5 Fe3+(aq) + 4 H2O(l)?
A) Fe2+(aq) B) MnO4-(aq) C) Mn2+(aq) D) H+(aq)
8. Assign oxidation numbers to any chemical. (4.2)
(1) In which compound is the oxidation state of oxygen not –2?
A) Al2O3 B) Li2O C) K2O2 D) MgO E) CO
(2) What is the oxidation number of chromium in Cr2O72-?
A) +2 B) -3 C) +3 D) +4 E) +6
9. Given the mass of any compound in a chemical reaction, solve for the mass of any
other compound in the reaction (4.3)
Consider the following balanced reaction. What mass (in g) of CO2 can be formed from
0.288 g 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 B) 0.209 g C) 0.792 g D) 0.126 g E) 0.198 g
10. Perform stoichiometric calculations for reactions in aqueous solutions (4.3)
1) 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
2) Based on the balanced chemical equation shown below, what volume of 0.250 M
K2S2O3(aq) is needed to completely react with 37.8 mL of 0.125 M KI3(aq)?
2 K2S2O3(aq) + KI3(aq) → K2S4O6(aq) + 3 KI(aq).
A) 37.8 mL B) 19.9 mL C) 75.6 mL D) 49.8 mL
3) Given the following balanced chemical equation,
CuCl2(aq) + 2 KOH(aq) → Cu(OH)2(s) + 2 KCl(aq)
how many moles of Cu(OH)2 can form from 275.0 mL of 0.350 M KOH solution?
Assume that CuCl2 is in excess.
A) 48.1 moles
B) 0.0241 moles
C) 0.0481 moles
D) 19.9 moles
E) 24.1 moles
11. Given the mass of two reactants in a chemical reaction, solve for the mass produced of
any product, determine which reactant is limiting and determine the mass remaining of
the excess reactant (4.4)
(1) 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. Molar mass BCl3 of is 117.16 g/mol.
BCl3(g) + 3 H2O(l) → H3BO3(s) + 3 HCl(g)
A) 75.9 g HCl B) 132 g HCl C) 18.7 g HCl D) 56.0 g HCl E) 25.3 g HCl
Chapter 4
7. Define and identify: reduction, oxidation, reducing agent, oxidizing agent and redox
reactions. (4.2)
(1) In the reaction Cl2 (aq) + 2 I− (aq) → 2 Cl− (aq) + I2 (aq), the oxidizing agent is:
A) I2 B) I− C) Cl2 D) H2O E) Cl−
(2) Considering the following reaction, which statement is incorrect?
Cu (s) + 4 H+ (aq) + 2 NO3− (aq) → Cu2+ (aq) + 2 NO2(g) + 2 H2O(l)
2+
A) Cu is the result of an oxidation.
B) Cu is the reducing agent.
C) NO3- is reduced.
D) Cu is reduced.
E) NO3- is the oxidizing agent.
(3) Which reaction type is incorrectly labeled?
A) Ca2+(aq) + SO42-(aq) → CaSO4 (s), acid-base reaction
B) C2H4 (g) + 3 O2 (g) → 2 CO2 (g) + 2 H2O (g), oxidation-reduction
C) Fe (s) + 2 H+ (aq) → Fe2+ (aq) + H2 (g), oxidation-reduction
D) Fe3+ (aq) + PO43- (aq) → FePO4 (s), precipitation
E) NH3 (aq) + HCl(aq) → NH4+(aq) + Cl−(aq), acid-base reaction
(4) Which is the reducing agent in the following redox reaction:
5 Fe2+(aq) + MnO4-(aq) + 8 H+(aq) → Mn2+(aq) + 5 Fe3+(aq) + 4 H2O(l)?
A) Fe2+(aq) B) MnO4-(aq) C) Mn2+(aq) D) H+(aq)
8. Assign oxidation numbers to any chemical. (4.2)
(1) In which compound is the oxidation state of oxygen not –2?
A) Al2O3 B) Li2O C) K2O2 D) MgO E) CO
(2) What is the oxidation number of chromium in Cr2O72-?
A) +2 B) -3 C) +3 D) +4 E) +6
9. Given the mass of any compound in a chemical reaction, solve for the mass of any
other compound in the reaction (4.3)
Consider the following balanced reaction. What mass (in g) of CO2 can be formed from
0.288 g 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 B) 0.209 g C) 0.792 g D) 0.126 g E) 0.198 g
10. Perform stoichiometric calculations for reactions in aqueous solutions (4.3)
1) 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
2) Based on the balanced chemical equation shown below, what volume of 0.250 M
K2S2O3(aq) is needed to completely react with 37.8 mL of 0.125 M KI3(aq)?
2 K2S2O3(aq) + KI3(aq) → K2S4O6(aq) + 3 KI(aq).
A) 37.8 mL B) 19.9 mL C) 75.6 mL D) 49.8 mL
3) Given the following balanced chemical equation,
CuCl2(aq) + 2 KOH(aq) → Cu(OH)2(s) + 2 KCl(aq)
how many moles of Cu(OH)2 can form from 275.0 mL of 0.350 M KOH solution?
Assume that CuCl2 is in excess.
A) 48.1 moles
B) 0.0241 moles
C) 0.0481 moles
D) 19.9 moles
E) 24.1 moles
11. Given the mass of two reactants in a chemical reaction, solve for the mass produced of
any product, determine which reactant is limiting and determine the mass remaining of
the excess reactant (4.4)
(1) 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. Molar mass BCl3 of is 117.16 g/mol.
BCl3(g) + 3 H2O(l) → H3BO3(s) + 3 HCl(g)
A) 75.9 g HCl B) 132 g HCl C) 18.7 g HCl D) 56.0 g HCl E) 25.3 g HCl
