Question

For the cell reaction \( 4Br^- + O_2 + 4H^+ \rightarrow 2Br_2 + 2H_2O \) at \( 298\,K \), the \( E^0_{\text{cell}} = 0.16\,V \). What would be the \( K_c \) (Equilibrium constant) value if the reverse reaction were to take place?

• A. \( 2.012 \times 10^{-10} \)
• B. \( 8.47 \times 10^{-9} \)
• C. \( 1.422 \times 10^{-11} \)
• D. \( 7.031 \times 10^{-10} \)

Hint:

For electrochemical cells, use \( E^0_{\text{cell}}=\frac{0.0591}{n}\log K \) at \(298K\). For reverse reaction, equilibrium constant becomes reciprocal.

Answer 1

The Correct Option is C