First slide

Nernst Equation

Question

For the reaction Pt /H₂(1atm) / H⁺_(aq) // Cl^–_(aq)/AgCl/Ag K_c (equilibrium constant) is represented as

Moderate

A

$K_{c} = \frac{[{Cl}^{-}] [AgCl]}{[H^{+}] [H_{2}]}$
B

$K_{c} = [H^{+}] [{Cl}^{-}]$
C

$K_{c} = \frac{[H^{+}] [H_{2}]}{[{Cl}^{-}] [AgCl]}$
D

$K_{c} = \frac{[H_{2}]}{[Ag]}$

Solution

From the given cell notation the cell reaction is
$Anode : \frac{1}{2} H_{2 (1 atm)} ⇌ H_{(aq)}^{+} + e^{-}$
$Cathode: {AgCl}_{(s)} + e^{-} ⇌ {Ag}_{(s)} + {Cl}_{(aq)}^{-}$
${AgCl}_{(s)} + \frac{1}{2} H_{2 (1 atm)} ⇌ H_{(aq)}^{+} + {Cl}_{(aq)}^{-} + {Ag}_{(s)}$
$K_{C} = [H^{+}] [{Cl}^{-}]$
For all Solids and pure liquids, active mass = 1

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