The value of reaction quotient $(Q)$ , for the following cell,

$Z n (s) | Z n^{2 +} (0.01 M) | | A g^{+} (1.25 M) | A g (s)$ is:

156

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125

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1.25 \times 10^{- 2}

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6.4 \times 10^{- 3}

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Solution

The correct option is D $6.4 \times 10^{- 3}$
The cell reaction is
$Z n (s) \to Z n^{2 +} (0.01 M) + 2 e^{-}$ .....equation I

$A g^{+} + e^{-} \to A g (s) \times 2$ ......equation II

On adding equation I and II, we get-

$Z n (s) + 2 A g^{+} (1.25 M) \to Z n^{2 +} (0.01 M) + 2 A g (s)$

$∴ Q = \frac{[Z n^{2 +}]}{[A g^{+}]^{2}} = \frac{0.01}{(1.25)^{2}} = 6.4 \times 10^{- 3}$

$∴$ Value of $Q = 6.4 \times 10^{- 3}$ .

Hence, option D is correct.

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Similar questions

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△ G^{\circ}

Z n (s) + A g_{2} O (s) + H_{2} O (l) ⇌ Z n^{2 +} (a q) + 2 A g (s) + 2 O H^{-} (a q)

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E_{c e l l}

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