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Topic 11: Redox and electrochemistry

13. Redox equations: Determining oxidized or reduced species from net ionic redox equation

1. Consider the oxidation-reaction reaction. 2+ 0
0
2+

Co + Cu -------- > Co + Cu

Which species is reduced?
2+
0
0
1) Co 2) Cu 3) Co 4) Cu 2+

2. Given the redox reaction below
2+
3+
3+
2Fe + Sn --------- > 2Fe + Sn 4+
Which species is reduced? 2+ 2+ 4+
3+
1) Fe 2) Sn 3) Fe 4) Sn

3. In the reaction below,
3+
+
2+
H2 + 2Fe ----------- > 2H + 2Fe
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Which species is gaining electrons? 3) Fe 4) H2
3+
+2
+
2) H
1) Fe

4. Consider the following redox reaction: 2+ 2
4+

Ni + Sn ----------- > Ni + Sn
The species oxidized is
2+
4+
1) Sn 2) Sn 3) Ni 4) Ni 2+

5. Given the redox reaction:
2+
3+
2Cr(s) + 3Sn (aq) ------- > 2Cr (aq) + 3Sn (s)
The species undergoing oxidation is
1) Sn (aq) 2) Cr(s) 3) Sn(s) 4) Cr (aq)
3+
2+

1) Cu (aq) Teacher Preview Copy
6. In the oxidation-reduction reaction below: 2+
2+

Zn + Ni --------- > Zn + Ni
Which species is losing electrons?
1) Zn 2) Ni 3) Zn 4) Ni
2+
2+

7. In the oxidation-reduction reaction below: 2+ 0
2-
3+
2 Fe + S ------------- > 2Fe + 2S
Which species acts as a reducing agent?
0
2+
3+
1) Fe 2) Fe 3) S 4) S 2-

8. Consider the following equation. 2+ 2+

Zn(s) + Cu (aq) ------- > Zn (aq) + Cu(s)

The reducing agent is
2+ 2+
2) Zn(s) 3) Cu (s) 4) Zn (aq)
9. In the oxidation-reduction reaction below,
3+
2+
2Al + 3Ni --------- > 2Al + 3Ni
Which species acts as an oxidizing agent?
2+
3+
1) Al 2) Al 3) Ni 4) Ni

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