Nernst equation Knowledge-Based Practice

Questions

1. 1.

   A galvanic cell operates at 298 K according to the reaction $\text{Cu}(s) + 2\text{Ag}^+(aq) \rightarrow \text{Cu}^{2+}(aq) + 2\text{Ag}(s)$ with $E^\circ_{\text{cell}} = +0.46\text{ V}$. At what value of the ion concentration ratio $\frac{[\text{Cu}^{2+}]}{[\text{Ag}^+]^2}$ does the cell potential equal $+0.40\text{ V}$? (Use $\frac{2.303 RT}{F} = 0.060\text{ V}$ at 298 K.)

   • A) $1.0 \times 10^2$
   • B) $1.0 \times 10^1$
   • C) $1.0 \times 10^4$
   • D) $1.0 \times 10^{-2}$
2. 2.

   A silver concentration cell operates at 298 K with $[\text{Ag}^+] = 1.0 \times 10^{-4}\text{ M}$ in the anode compartment and $[\text{Ag}^+] = 0.10\text{ M}$ in the cathode compartment. What is the cell potential, $E_{\text{cell}}$, under these conditions? (Use $\frac{2.303RT}{F} = 0.059\text{ V}$ at 298 K.)

   • A) $-0.177\text{ V}$
   • B) $+0.089\text{ V}$
   • C) $+0.177\text{ V}$
   • D) $+0.059\text{ V}$
3. 3.

   A galvanic cell operates at 298 K according to the reaction $\text{Cd}(s) + \text{Ni}^{2+}(aq) \rightarrow \text{Cd}^{2+}(aq) + \text{Ni}(s)$ with $E^\circ_{\text{cell}} = +0.150\text{ V}$. If the measured cell potential is $+0.120\text{ V}$ when $[\text{Cd}^{2+}] = 0.10\text{ M}$, what is the concentration of $\text{Ni}^{2+}(aq)$? (Use $\frac{2.303 RT}{F} = 0.060\text{ V}$ at 298 K.)

   • A) 1.0 M
   • B) 0.10 M
   • C) 0.010 M
   • D) 0.0010 M
4. 4.

   A galvanic cell operates at 298 K according to the reaction $\text{Zn}(s) + 2\text{H}^+(aq) \rightarrow \text{Zn}^{2+}(aq) + \text{H}_2(g)$ with $E^\circ_{\text{cell}} = +0.760\text{ V}$. What is the cell potential when $[\text{Zn}^{2+}] = 1.0\text{ M}$, the partial pressure of $\text{H}_2$ is 1.0 atm, and the pH of the cathode compartment is 3.00? (Use $\frac{2.303 RT}{F} = 0.0592\text{ V}$ at 298 K.)

   • A) +0.938 V
   • B) +0.671 V
   • C) +0.405 V
   • D) +0.582 V
5. 5.

   A galvanic cell operates at 25 °C based on the reaction $\text{Sn}(s) + \text{Pb}^{2+}(aq) \rightarrow \text{Sn}^{2+}(aq) + \text{Pb}(s)$ with a standard cell potential $E^\circ_{\text{cell}} = +0.010\text{ V}$. If $[\text{Pb}^{2+}] = 0.10\text{ M}$ and $[\text{Sn}^{2+}] = 0.0010\text{ M}$, what is the cell potential $E_{\text{cell}}$ at this temperature? (Use $\frac{2.303 RT}{F} = 0.0592\text{ V}$ at 298 K.)

   • A) $-0.049\text{ V}$
   • B) $+0.039\text{ V}$
   • C) $-0.069\text{ V}$
   • D) $+0.069\text{ V}$

Answers and step-by-step solutions appear after you finish the test.