For the redox reaction ZnS-Cu2-0-1M- Zn2-1M-Cus taking place in a cell- E0cell is 1-10 volt- Ecell for the cell will be - 2-303RT-F-0-0591

The correct option is B 1.07 V The Nernst equation for the emf of the cell is E _ cell ^ nbsp; nbsp;= nbsp; E _ cell ^ 0 nbsp; nbsp; 0. ...

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Nernst Equation

For the redox...

Question

For the redox reaction $Z n (S) + C u^{2 +} (0.1 M) \to Z n^{2 +} (1 M) + C u (s)$ taking place in a cell, $E_{c e l l}^{0}$ is 1.10 volt. $E_{c e l l}$ for the cell will be : $(2.303 \frac{R T}{F} = 0.0591)$

2.14 V

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1.80 V

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1.07 V

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0.82 V

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Z n (s) + {C u}^{2 +} (0.1 M) ⟶ {Z n}^{2 +} (1 M) + C u (s)

E_{c e l l}^{o}

1.10 V

E_{c e l l}

(2.303 \frac{R T}{F} = 0.0591)

Z n (s) + C u^{2 +} (0.1 M) \to Z n^{2 +} (1 M) + C u (s)

E_{c e l l}^{0}

E_{c e l l}

(2.303 \frac{R T}{F} = 0.0591)

Z n + C u_{(0.1 M)}^{2 +} \to Z n_{(1 M)}^{2 +} + C u

E_{c e l l}^{⊖} = 1.10

E_{C e l l}^{⊖}

Z n (s) + C u^{2 +} (a q .) ⇌ C u (s) + Z n^{2 +} (a q .)

Q = \frac{[Z n^{2 +}]}{[C u^{2 +}]}

E_{c e l l}

Q

O A = 1.10 v o l t . E_{c e l l} = 1.1591 v o l t

T = 298 K)

C u (s) | C u^{2 +} (1.0 M) | | A g^{+} (1.0 M) | A g (s) E_{c e l l}^{\circ} = 0.46 V

Z n (s) | Z n^{2 +} (1.0 M) | | C u^{2 +} (1.0 M) | C u (s) E_{c e l l}^{\circ} = 1.10 V

E_{c e l l}

Z n | Z n^{2 +} (0.1 M) | | A g^{+} (1.0 M | A g

298 K

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