Consider the galvanic cell:

Zn(s) | Zn^{2+} (0.010 M) || Cu^{2+} (0.50 M) | Cu(s) at 298 K.

Standard reduction potentials are $E^{\circ}(\text{Cu}^{2+}/\text{Cu})=+0.34\text{ V}$ and $E^{\circ}(\text{Zn}^{2+}/\text{Zn})=-0.76\text{ V}$.

(a) Calculate the cell emf under the given conditions using the Nernst equation.

(b) If 0.025 mol of electrons pass through the cell, how many grams of copper are deposited on the cathode? (Give your answer to three significant figures.)

Question

Consider the galvanic cell:

Zn(s) | Zn^{2+} (0.010 M) || Cu^{2+} (0.50 M) | Cu(s) at 298 K.

Standard reduction potentials are $E^{\circ}(\text{Cu}^{2+}/\text{Cu})=+0.34\text{ V}$ and $E^{\circ}(\text{Zn}^{2+}/\text{Zn})=-0.76\text{ V}$.

(a) Calculate the cell emf under the given conditions using the Nernst equation.

(b) If 0.025 mol of electrons pass through the cell, how many grams of copper are deposited on the cathode? (Give your answer to three significant figures.)

Accepted Answer

E = 1.15 V; mass of Cu = 0.794 g

Gce Model Questions Vol1 2017 Chemistry Question 17

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