Electrochemistry

Practice Questions

High School Chemistry › Electrochemistry

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1

Consider the following electrolytic cell:

$Ni + Fe^{2+} \rightarrow Ni^{2+} + Fe$ $E^{\circ} = -0.21V$

What happens at the anode in the electrolytic cell?

2

Consider the following electrolytic cell:

$Ni + Fe^{2+} \rightarrow Ni^{2+} + Fe$ $E^{\circ} = -0.21V$

What happens at the anode in the electrolytic cell?

3

Toward which pole do the electrons travel in an electrolytic cell?

4

Toward which pole do the electrons travel in an electrolytic cell?

5

How does an electrolytic cell differ from a galvanic cell?

6

How does an electrolytic cell differ from a galvanic cell?

7

Which of the following species is being produced at the anode?

$Li^{+}_{(aq)} + K_{(s)} \rightarrow Li_{(s)} + K^{+}_{(aq)}$

8

Which of the following species is being produced at the anode?

$Li^{+}_{(aq)} + K_{(s)} \rightarrow Li_{(s)} + K^{+}_{(aq)}$

9

$Li^{+}_{(aq)} + e^- \rightarrow Li_{(s)}$ $\varepsilon ^o = -3.04$

$Mg^{2+}_{(aq)} +2e^- \rightarrow Mg_{(s)}$ $\varepsilon ^o= -2.38$

$Ni^{2+}_{(aq)}+ 2e^- \rightarrow Ni_{(s)}$ $\varepsilon ^o = -0.23$

$Ag^{2+}_{(aq)} + 2e^- \rightarrow Ag_{(s)}$ $\varepsilon ^o = 0.80$

$Cl_2_{(g)}+ 2e^- \rightarrow 2Cl^-_{(aq)}$ $\varepsilon ^o= 1.36$

Which of the following species would mostly likely be oxidized, if placed in a electrochemical cell with another species?

10

$Hg^{2+}_{(aq)} + 2e^- \rightarrow Hg_{(l)}$ $\varepsilon ^o = 0.85$

$Cu^{+}_{(aq)} +e^-\rightarrow Cu_{(s)}$ $\varepsilon ^o = 0.34$

$2H^{+}_{(aq)} + 2e^- \rightarrow H_2_{(g)}$ $\varepsilon ^o = 0$

$Zn^{2+}_{(aq)} + 2e^- \rightarrow Zn_{(s)}$ $\varepsilon ^o = -0.76$

$Cr^{3+}_{(aq)} + 3e^- \rightarrow Cr_{(s)}$ $\varepsilon ^o = -0.74$

Which of the following species would mostly likely be reduced, if placed in a galvanic cell with another species?

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