Which of the following cells give the cells potentials to be their standard values?

Z n_{(s)} | Z n_{a q}^{2 +} (0.01 M) | | H_{3} O_{(a q)}^{+} (0.01 M) | H_{2 (g)}

(1atm),Pt

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C u_{(s)} | C u_{(a q)}^{2 +} (0.25 M) | | A g_{(a q)}^{+} (0.5 M) | A g_{(s)}

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C d_{(s)} | C d_{(a q)}^{2 +} (0.01 M) | | p H = 1 | H_{2 (g)}

(1 atm), Pt

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Z n_{(s)} | Z n_{(a q)}^{2 +} (0.01 M) | | p H = 1 | H_{2 (g)}

(1 atm),Pt

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Solution

The correct option is C $C d_{(s)} | C d_{(a q)}^{2 +} (0.01 M) | | p H = 1 | H_{2 (g)}$ (1 atm), Pt

(a) Cell reaction :
$Z n_{(a q)}^{+} + Z n_{(s)} \to H_{2 (g)} + Z n_{(a q)}^{2 +}$
Reaction quotient,
$Q = \frac{P H_{2} \times [Z n^{2 +}]}{[H^{+}]^{2}} = \frac{1 \times 0.01}{{0.1}^{2}} = 1, l o g Q = 0$
(b) Cell reaction :
$2 A g_{(a q)}^{+} + C u_{(s)} \to C u_{(a q)}^{2 +} + 2 A g_{(s)}$
$Q = \frac{[C u^{2 +}]}{[A g^{+}]^{2}} = \frac{0.25}{(0.5)^{2}} = 1,$
(c) Cell reaction :
$2 H_{(a q)}^{+} + C d (s) \to H_{2} + C d_{(a q)}^{2 +} Q = \frac{P H_{2} \times [C d^{2 +}]}{[H^{+}]^{2}} = \frac{1 \times 0.01}{{0.1}^{2}} = 1$
(d) Cell reaction :
$2 H_{(a q)}^{+} + Z n (s) \to H_{2} + Z n_{(a q)}^{2 +}$
$Q = \frac{P H_{2} \times [Z n^{2 +}]}{[H^{+}]^{2}} = \frac{1 \times 0.01}{{0.1}^{2}} = 10$

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Similar questions

Which of the following cells give the cell potentials

to be their standard values ?

Following are the values of standard potentials of two half cells, which of the following will be the value of standard cell potential E^o_cell:

Ag, Cu, Co and Zn

0.799 V, 0.337 V, - 0.277 V, - 0.762 V

A g, C u, C o

Z n

0.799,

0.337,

- 0.277,

- 0.762

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