(B) The relationship between $E^0_{cell}$ and the equilibrium constant $K_c$ is given by the Nernst equation at $298 \text{ K}$:$E^0_{cell} = \frac{0.

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(B) The relationship between $E^0_{cell}$ and the equilibrium constant $K_c$ is given by the Nernst equation at $298 \text{ K}$:$E^0_{cell} = \frac{0.0591 \text{ V}}{n} \log K_c$Here, $n = 2$ (number of electrons transferred).$0.0296 = \frac{0.0591}{2} \log K_c$$0.0296 = 0.02955 \log K_c$Since $0.0296 \approx 0.02955$, we get $\log K_c \approx 1$.$K_c = 10^1 = 10$.

Class 12 Chemistry Electrochemistry Nernst equation and ECS

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For a certain redox reaction in a galvanic cell $X(s) + Y^{2+}_{(aq)} \rightarrow X^{2+}_{(aq)} + Y(s)$, $E^0_{cell}$ is $0.0296 \text{ V}$ at $298 \text{ K}$. What is the equilibrium constant of the reaction?

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$1$
B
$10$
C
$100$
D
$1000$

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At what $pH$,given half cell $MnO_4^{-} (0.1 \ M) \mid Mn^{2+} (0.001 \ M)$ will have electrode potential of $1.282 \ V$? (Nearest Integer) Given $E_{MnO_4^{-} / Mn^{2+}}^{o} = 1.54 \ V, \frac{2.303 RT}{F} = 0.059 \ V$

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At $298 \ K$, the $emf$ of the cell is ............ $V$.
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For a certain redox reaction in a galvanic cell $X(s) + Y^{2+}_{(aq)} \rightarrow X^{2+}_{(aq)} + Y(s)$, $E^0_{cell}$ is $0.0296 \text{ V}$ at $298 \text{ K}$. What is the equilibrium constant of the reaction?

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Consider the cell $Pt | H_2(P_1 \ atm) | H^{+}(X_1 \ M) || H^{+}(X_2 \ M) | H_2(P_2 \ atm) | Pt$. The cell reaction will be spontaneous if

For the cell reaction $Zn_{(s)} + Ni^{2+}_{(aq)} (a = 0.1) \rightarrow Zn^{2+}_{(aq)} (a = 1.0) + Ni_{(s)}$ at $298 \ K$,the $emf$ is observed to be $0.5105 \ V$. What is the standard $emf$ $(E^{\circ}_{cell})$ of the cell in $V$?

At what $pH$,given half cell $MnO_4^{-} (0.1 \ M) \mid Mn^{2+} (0.001 \ M)$ will have electrode potential of $1.282 \ V$? (Nearest Integer) Given $E_{MnO_4^{-} / Mn^{2+}}^{o} = 1.54 \ V, \frac{2.303 RT}{F} = 0.059 \ V$

At $298 \ K$, the $emf$ of the cell is ............ $V$.$Pt | H_{2(2 \ atm)} | H_{(0.02 \ M)}^{+} || H_{(0.1 \ M)}^{+} | H_{2(1 \ atm)} | Pt$

The reduction potential of a hydrogen half-cell will be negative if:

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At $298 \ K$, the $emf$ of the cell is ............ $V$.
$Pt | H_{2(2 \ atm)} | H_{(0.02 \ M)}^{+} || H_{(0.1 \ M)}^{+} | H_{2(1 \ atm)} | Pt$