(Solved): A) B) Thank you so much! Use standard reduction potentials to calculate the equilibrium const ...

A)

B)

Thank you so much!

Use standard reduction potentials to calculate the equilibrium constant for the reaction: \[ 2 \mathrm{H}^{+}(a q)+\mathrm{Pb}(s) \rightarrow \mathrm{H}_{2}(g)+\mathrm{Pb}^{2+}(a q) \] Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at \( 298 \mathrm{~K} \) : \( \Delta G^{\circ} \) for this reaction would be than zero. Use standard reduction potentials to calculate the equilibrium constant for the reaction: \[ 2 \mathrm{H}^{+}(a q)+2 \mathrm{Ag}(s) \rightarrow \mathrm{H}_{2}(s)+2 \mathrm{Ag}^{+}(a q) \] From the table of standard reduction potentials: \( E_{\mathrm{H}^{+} / \mathrm{H}_{2}}^{\mathrm{o}}=0.000 \mathrm{~V} \), \( E_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\mathrm{o}}=0.799 \mathrm{~V} \) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at \( 298 \mathrm{~K} \) : \( \Delta G^{\circ} \) for this reaction would be than zero.