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Topic 11: Redox and electrochemistry

14. Redox equations: Determining oxidized or reduced species from redox equation

1. In the redox reaction:

Ni + CuSO4 ------ > NiSO4 + Cu

Which substance is oxidized?
2+
2+
1) Ni 2) Cu 3) Ni 4) Cu

2. Given the oxidation-reduction reaction equation below:

Na + H2O -------- > NaOH + H2
Which substance is oxidized?
+
2-
1) H2 2) O 3) H 4) Na

3. In the reaction
2H2O --------------- > 2H2 + O2
Teacher Preview Copy
Which species is reduced? 2- +

1) H2 2) O 3) H 4) O2

4. Given the redox reaction
Fe + 2AgCl ------ > 2Ag + FeCl2
The species oxidized is
1) Fe 2) Fe 3) Cl - 4) Ag +
0
3+

5. Consider the redox reaction below:
2KBr + F2 -------- > 2KF + Br2

Which substance is the oxidizing agent
+

3) F2

2) K
1) Br2 Teacher Preview Copy 4) Br -

6. Given the oxidation-reduction reaction.
C(s) + H2O(g) -------- > CO(g) + H2(g)
The reducing agent in this reaction is 2+

+
1) C 2) H 3) C 4) H2

7. In the redox reaction 0
3Ni(NO3)2 + 2Al ------- > 3Ni + 2Al(NO3)3
Which species is the oxidizing agent?
1) Ni 2) Al 3) Ni 4) Al
2+
0
0
3+

8. In the redox reaction CuO + CO --------------- > CO2 + Cu
Which species is losing electrons?
2+
4+
1) Cu 2) Cu 3) C 4) C
2+

9. Given the oxidation-reduction reaction below:
4HCl + MnO2 ------- > MnCl2 + H2O + Cl2
Which of species in this reaction is gaining electrons?
4+
2+
+
1) H 2) Cl - 3) Mn 4) Mn

10. Given the redox reaction
Ag + 2HNO3 ------------ > AgNO3 + NO + H2O
Which substance is losing electrons?

0
+
2-
+
1) Ag 2) H 3) Ag 4) O

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