(B) The standard cell potential is calculated using the formula:$E_{cell}^o = E_{cathode}^o - E_{anode}^o$Here,the cathode is the $N^{+}/N$ electrode

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The standard $EMF$ of the cell is $-0.27 \ V$.

(B) The standard cell potential is calculated using the formula:$E_{cell}^o = E_{cathode}^o - E_{anode}^o$Here,the cathode is the $N^{+}/N$ electrode and the anode is the $M^{+}/M$ electrode.$E_{cell}^o = E_{N^{+}/N}^o - E_{M^{+}/M}^o$$E_{cell}^o = 0.25 \ V - 0.52 \ V = -0.27 \ V$Since $E_{cell}^o < 0$,the cell reaction is non-spontaneous.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Medium

Given that the standard reduction potentials for $M^{+}/M$ and $N^{+}/N$ electrodes at $298 \ K$ are $0.52 \ V$ and $0.25 \ V$ respectively. Which of the following is correct in respect of the following electrochemical cell?
$M | M^{+} || N^{+} | N$

AIIMS 2016 All AIIMS

A
The overall cell reaction is a spontaneous reaction.
B
The standard $EMF$ of the cell is $-0.27 \ V$.
C
The standard $EMF$ of the cell is $0.77 \ V$.
D
The standard $EMF$ of the cell is $-0.77 \ V$.

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Electrochemistry

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Electrode potential and ECell

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What is cell potential and $emf$? Explain with suitable examples.

Difficult

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Electrode potential data are given below :
$Fe^{3+}_{(aq)} + e^- \to Fe^{2+}_{(aq)}; \, E^o = +0.77 \, V$
$Al^{3+}_{(aq)} + 3e^- \to Al_{(s)}; \, E^o = -1.66 \, V$
$Br_{2(aq)} + 2e^- \to 2Br^{-}_{(aq)}; \, E^o = +1.08 \, V$
Based on the data given above,the reducing power of $Fe^{2+}$,$Al$ and $Br^{-}$ will increase in the order:

Easy

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If the cell potential value is negative for a cell constructed by attaching a standard hydrogen electrode to another half-cell,then the other half-cell will be:
$(i)$ Anode or cathode?
$(ii)$ Positive or negative?
$(iii)$ On left side or right side?

Easy

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The $E^{0}_{Red}$ values for $Li, Zn, H,$ and $Ag$ are $-3.05 \ V, -0.76 \ V, 0.00 \ V,$ and $0.80 \ V$ respectively. Which of these has the highest reducing power?

Medium

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Standard electrode potential of three metals $X$,$Y$ and $Z$ are $-1.2 \, V$,$+0.5 \, V$ and $-3.0 \, V$ respectively. The reducing power of these metals will be

MediumAIPMT 2011

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Given that the standard reduction potentials for $M^{+}/M$ and $N^{+}/N$ electrodes at $298 \ K$ are $0.52 \ V$ and $0.25 \ V$ respectively. Which of the following is correct in respect of the following electrochemical cell?$M | M^{+} || N^{+} | N$

Similar Questions

What is cell potential and $emf$? Explain with suitable examples.

If the cell potential value is negative for a cell constructed by attaching a standard hydrogen electrode to another half-cell,then the other half-cell will be:$(i)$ Anode or cathode?$(ii)$ Positive or negative?$(iii)$ On left side or right side?

The $E^{0}_{Red}$ values for $Li, Zn, H,$ and $Ag$ are $-3.05 \ V, -0.76 \ V, 0.00 \ V,$ and $0.80 \ V$ respectively. Which of these has the highest reducing power?

Standard electrode potential of three metals $X$,$Y$ and $Z$ are $-1.2 \, V$,$+0.5 \, V$ and $-3.0 \, V$ respectively. The reducing power of these metals will be

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Given that the standard reduction potentials for $M^{+}/M$ and $N^{+}/N$ electrodes at $298 \ K$ are $0.52 \ V$ and $0.25 \ V$ respectively. Which of the following is correct in respect of the following electrochemical cell?
$M | M^{+} || N^{+} | N$

If the cell potential value is negative for a cell constructed by attaching a standard hydrogen electrode to another half-cell,then the other half-cell will be:
$(i)$ Anode or cathode?
$(ii)$ Positive or negative?
$(iii)$ On left side or right side?