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Electrochemical Series

Calculate the...

Question

Calculate the $E M F$ of the following cell:

$Z n | Z n^{2 +} (0.01 M) | | C u^{2 +}] (0.1 M) | C u$ at $298 K$

1.129 V

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0.00295 V

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0.0295 V

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2.95 V

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Solution

The correct option is A $1.129 V$
For this reaction
At anode :- $Z n (s) ⟶ {Z n}^{2 +} + 2 e^{-}$
At cathode :- ${C u}^{2 +} (a q) + {2 e}^{-} ⟶ C u (s)$
Nearest equation would be,
$E_{c e l l} = E_{c e l l}^{0} - \frac{2.303 R T}{2 F} l o g \frac{[{Z n}^{2 +}]}{[{C u}^{2 +}]}$
At $298 K$ , $E_{c e l l} = 1.1 - \frac{0.0591}{2} l o g \frac{0.01}{0.1}$
$= 1.1 - 0.0591 l o g 10^{- 1}$
$= 1.1 + 0.029 = 1.129 V$

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Below given are emf of three galvanic cells, represented by $E_{1}$ , $E_{2}$ and $E_{3}$ . Which of the following is true?

I. $Z n | Z n^{2 +} (1 M) | | C u^{2 +} (1 M) | C u$

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