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Using the standard half-cell potential listed, calculate the equilibrium constant for the reaction :
\[
\begin{array}{c}
\mathrm{Co}(s)+2 \mathrm{H}^{+}(a q) \longrightarrow \mathrm{Co}^{2+}(a q)+\mathrm{H}_{2}(g) \text { at } 298 \mathrm{~K} \\
\mathrm{Co}^{2+}(a q)+2 e^{-} \longrightarrow \mathrm{Co}(s) \quad E^{\circ}=-0.277 \mathrm{~V}
\end{array}
\]
(a) \( 2.3 \times 10^{9} \)
(b) \( 4.8 \times 10^{4} \)
(c) \( 4.8 \times 10^{7} \)
(d) \( 4.8 \times 10^{11} \)
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