(B) The cell reaction is: $H_2(P_1) \rightarrow 2H^{+} + 2e^{-}$ (Anode) and $2H^{+} + 2e^{-} \rightarrow H_2(P_2)$ (Cathode).Overall reaction: $H_2(P

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$\frac{RT}{2F} \ln \frac{P_1}{P_2}$

(B) The cell reaction is: $H_2(P_1) \rightarrow 2H^{+} + 2e^{-}$ (Anode) and $2H^{+} + 2e^{-} \rightarrow H_2(P_2)$ (Cathode).Overall reaction: $H_2(P_1) \rightarrow H_2(P_2)$.Using the Nernst equation: $E_{cell} = E^{\circ}_{cell} - \frac{RT}{nF} \ln Q$.Here,$E^{\circ}_{cell} = 0 \ V$,$n = 2$,and $Q = \frac{P_2}{P_1}$.$E_{cell} = 0 - \frac{RT}{2F} \ln \frac{P_2}{P_1}$.$E_{cell} = \frac{RT}{2F} \ln \frac{P_1}{P_2}$.

Class 12 Chemistry Electrochemistry Nernst equation and ECS

Medium

What will be the $EMF$ for the given cell?
$Pt | H_2(g, P_1) | H^{+}(aq.) (1 \ M) || H^{+}(aq.) (1 \ M) | H_2(g, P_2) | Pt$

A
$\frac{RT}{F} \ln \frac{P_1}{P_2}$
B
$\frac{RT}{2F} \ln \frac{P_1}{P_2}$
C
$\frac{RT}{F} \ln \frac{P_2}{P_1}$
D
$\frac{RT}{2F} \ln \frac{P_2}{P_1}$

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Class 12

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Electrochemistry

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Nernst equation and ECS

Consider a Daniell cell operating under non-standard state conditions. Suppose that the cell's reaction is multiplied by $2$. Which of the following will double its initial value?

Easy

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Find the $emf$ of the cell in which the following reaction takes place at $298 \ K$ (in $V$):
$Ni_{(s)} + 2Ag^{+}(0.001 \ M) \rightarrow Ni^{2+}(0.001 \ M) + 2Ag_{(s)}$
(Given that $E_{cell}^{\circ} = 10.5 \ V$,$\frac{2.303 RT}{F} = 0.059$ at $298 \ K$)

MediumNEET 2022

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Calculate the potential of a hydrogen electrode in contact with a solution whose $pH = 10$.

EasyGUJCET 2024

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What is the potential of a cell containing two hydrogen electrodes,the negative one in contact with $10^{-8} \ M \ H^{+}$ and the positive one in contact with $0.025 \ M \ H^{+}$? (in $V$)

Medium

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

MediumAIEEE 2011

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What will be the $EMF$ for the given cell?$Pt | H_2(g, P_1) | H^{+}(aq.) (1 \ M) || H^{+}(aq.) (1 \ M) | H_2(g, P_2) | Pt$

Similar Questions

Consider a Daniell cell operating under non-standard state conditions. Suppose that the cell's reaction is multiplied by $2$. Which of the following will double its initial value?

Find the $emf$ of the cell in which the following reaction takes place at $298 \ K$ (in $V$):$Ni_{(s)} + 2Ag^{+}(0.001 \ M) \rightarrow Ni^{2+}(0.001 \ M) + 2Ag_{(s)}$(Given that $E_{cell}^{\circ} = 10.5 \ V$,$\frac{2.303 RT}{F} = 0.059$ at $298 \ K$)

Calculate the potential of a hydrogen electrode in contact with a solution whose $pH = 10$.

What is the potential of a cell containing two hydrogen electrodes,the negative one in contact with $10^{-8} \ M \ H^{+}$ and the positive one in contact with $0.025 \ M \ H^{+}$? (in $V$)

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

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What will be the $EMF$ for the given cell?
$Pt | H_2(g, P_1) | H^{+}(aq.) (1 \ M) || H^{+}(aq.) (1 \ M) | H_2(g, P_2) | Pt$

Find the $emf$ of the cell in which the following reaction takes place at $298 \ K$ (in $V$):
$Ni_{(s)} + 2Ag^{+}(0.001 \ M) \rightarrow Ni^{2+}(0.001 \ M) + 2Ag_{(s)}$
(Given that $E_{cell}^{\circ} = 10.5 \ V$,$\frac{2.303 RT}{F} = 0.059$ at $298 \ K$)