AP Chemistry
9.9 Cell Potential and Free Energy
A student constructs a standard galvanic cell operating at \(298\text{ K}\) based on the half-reactions represented below.
\(\text{Zn}^{2+}\text{(aq)} + 2e^- \rightarrow \text{Zn(s)} \quad E^\circ = -0.76\text{ V}\)
\(\text{Cu}^{2+}\text{(aq)} + 2e^- \rightarrow \text{Cu(s)} \quad E^\circ = +0.34\text{ V}\)
The overall reaction occurring in the cell is \(\text{Zn(s)} + \text{Cu}^{2+}\text{(aq)} \rightarrow \text{Zn}^{2+}\text{(aq)} + \text{Cu(s)}\). What is the value of the standard Gibbs free energy change, \(\Delta G^\circ\), for the reaction at \(298\text{ K}\)?
\(\text{Zn}^{2+}\text{(aq)} + 2e^- \rightarrow \text{Zn(s)} \quad E^\circ = -0.76\text{ V}\)
\(\text{Cu}^{2+}\text{(aq)} + 2e^- \rightarrow \text{Cu(s)} \quad E^\circ = +0.34\text{ V}\)
The overall reaction occurring in the cell is \(\text{Zn(s)} + \text{Cu}^{2+}\text{(aq)} \rightarrow \text{Zn}^{2+}\text{(aq)} + \text{Cu(s)}\). What is the value of the standard Gibbs free energy change, \(\Delta G^\circ\), for the reaction at \(298\text{ K}\)?
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