AP Chemistry
9.9 Cell Potential and Free Energy
9.5 Free Energy and Equilibrium
9.3 Gibbs Free Energy and Thermodynamic Favorability
A student investigates the standard thermodynamic and electrochemical properties of the reaction represented by the following equation at \(298\text{ K}\):
\[ \text{Sn(s)} + 2\,\text{Ag}^+\text{(aq)} \rightleftharpoons \text{Sn}^{2+}\text{(aq)} + 2\,\text{Ag(s)} \quad E^\circ_{\text{cell}} = +0.94\text{ V} \]
Which of the following correctly identifies the sign of \(\Delta G^\circ\) and the magnitude of \(K\) relative to \(1\), along with the appropriate justification?
\[ \text{Sn(s)} + 2\,\text{Ag}^+\text{(aq)} \rightleftharpoons \text{Sn}^{2+}\text{(aq)} + 2\,\text{Ag(s)} \quad E^\circ_{\text{cell}} = +0.94\text{ V} \]
Which of the following correctly identifies the sign of \(\Delta G^\circ\) and the magnitude of \(K\) relative to \(1\), along with the appropriate justification?
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