The logarithm of equilibrium constant for the reaction $Pd ^{2+}+4 Cl ^{-} \rightleftharpoons PdCl _4^{2-}$ is (Nearest integer) Given : $\frac{230RT }{ F }=006 V$ $Pd _{\text {(aq) }}^{2+}+2 e ^{-} \rightleftharpoons Pd ( s ) \quad E ^{\ominus}=083 V$ $PdCl _4^{2-} \text { (aq) }+2 e ^{-} \rightleftharpoons Pd ( s )+4 Cl ^{-} \text {(aq) } E ^{\ominus}=065 V$
The logarithm of equilibrium constant for the reaction $Pd ^{2+}+4 Cl ^{-} \rightleftharpoons PdCl _4^{2-}$ is (Nearest integer) Given : $\frac{230RT }{ F }=006 V$ $Pd _{\text {(aq) }}^{2+}+2 e ^{-} \rightleftharpoons Pd ( s ) \quad E ^{\ominus}=083 V$ $PdCl _4^{2-} \text { (aq) }+2 e ^{-} \rightleftharpoons Pd ( s )+4 Cl ^{-} \text {(aq) } E ^{\ominus}=065 V$
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Correct Answer: 6
Solution and Explanation
\[ \Delta G^o = -RT \ln K \]
The equation for the cell potential is:\[ \text{E}_\text{cell} = \text{E}_\text{cathode} - \text{E}_\text{anode} \]
For the reaction:\[ \text{Pd}^{2+} (aq) + 2e^- \rightarrow \text{Pd}(s) \quad E^\circ = 0.83\, \text{V} \]
\[ \text{PdCl}_4^{2-} (aq) + 2e^- \rightarrow \text{Pd}(s) + 4\text{Cl}^- (aq) \quad E^\circ = 0.65\, \text{V} \]
The net reaction is:\[ \text{Pd}^{2+} (aq) + 4\text{Cl}^- (aq) \rightleftharpoons \text{PdCl}_4^{2-} (aq) \]
Using the Nernst equation:\[ \text{E}_\text{cell} = \text{E}_\text{cathode} - \text{E}_\text{anode} = 0.83 - 0.65 = 0.18\, \text{V} \]
Thus, by using the equation \( \Delta G^o = -nFE^\circ \) and solving for the logarithm of the equilibrium constant \( K \), we get:\[ \log K = 6 \]
This result shows the relationship between the standard cell potential and the equilibrium constant. A higher \( K \) value indicates a more spontaneous reaction, which can be derived from the Nernst equation.Top JEE Main Chemistry Questions
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Electrochemical Cells
An electrochemical cell is a device that is used to create electrical energy through the chemical reactions which are involved in it. The electrical energy supplied to electrochemical cells is used to smooth the chemical reactions. In the electrochemical cell, the involved devices have the ability to convert the chemical energy to electrical energy or vice-versa.
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Anode
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Electrolytic cells
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