Consider a galvanic cell where the following reaction occurs: $ \text{Zn(s)} + \text{Cu}^{2+}(aq) \rightarrow \text{Zn}^{2+}(aq) + \text{Cu(s)} $. The cell is set up with \( [\text{Cu}^{2+}] = 0.5 \

Question

Consider a galvanic cell where the following reaction occurs: $ \text{Zn(s)} + \text{Cu}^{2+}(aq) \rightarrow \text{Zn}^{2+}(aq) + \text{Cu(s)} $. The cell is set up with $ [\text{Cu}^{2+}] = 0.5 \text{M} $ and $ [\text{Zn}^{2+}] = 0.01 \text{M} $. Using the Nernst equation, which of the following expressions correctly represents the cell potential $ E_{cell} $?

Accepted Answer

E_{cell} = E^{\circ}_{cell} - \frac{0.059}{2} \log \left( \frac{0.01}{0.5} \right)

Answer

E_{cell} = E^{\circ}_{cell} - \frac{0.059}{2} \log \left( \frac{0.5}{0.01} \right)

Answer

E_{cell} = E^{\circ}_{cell} + \frac{0.059}{2} \log \left( \frac{0.5}{0.01} \right)

Answer

E_{cell} = E^{\circ}_{cell} + \frac{0.059}{2} \log \left( \frac{0.01}{0.5} \right)

NEET Chemistry Nernst Equation MCQ Question

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