AP Chemistry
9.8 Galvanic (Voltaic) and Electrolytic Cells
A student constructs a galvanic cell operating under standard conditions using the two half-reactions shown below.
\(\text{Ag}^+\text{(aq)} + e^- \rightarrow \text{Ag(s)} \quad E^\circ = +0.80 \text{ V}\)
\(\text{Zn}^{2+}\text{(aq)} + 2 e^- \rightarrow \text{Zn(s)} \quad E^\circ = -0.76 \text{ V}\)
Which of the following balanced net-ionic equations represents the overall spontaneous reaction occurring in the cell?
\(\text{Ag}^+\text{(aq)} + e^- \rightarrow \text{Ag(s)} \quad E^\circ = +0.80 \text{ V}\)
\(\text{Zn}^{2+}\text{(aq)} + 2 e^- \rightarrow \text{Zn(s)} \quad E^\circ = -0.76 \text{ V}\)
Which of the following balanced net-ionic equations represents the overall spontaneous reaction occurring in the cell?
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