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Nernst Equation

The EMF of th...

Question

The EMF of the cell :
$P t,$ $H_{2} (1 a t m) | H^{\oplus} (a q) ∥ A g C l | A g$ is 0.27 and 0.26 V at $25^{\circ} C$ and $35^{\circ} C$ , respectively. The posituve value of heat of the reaction occurring inside the cell at $25^{\circ} C$ ( $i n k J K^{- 1}$ ) is: ( write your answer to nearest integer)

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Solution

${(\frac{\partial E}{\partial T})}_{p} = (\frac{0.26 - 0.27}{35 - 25}) = \frac{- 0.07}{10} V K^{- 1} [n_{c e l l} = 1]$
$Δ H = - n F [E_{c e l l} (a t 25^{\circ} C) - T {(\frac{\partial E}{\partial T})}_{p}]$
$Δ H = - 1 \times 96500 [0.27 - 298 (- \frac{0.01}{10})]$
$Δ H = - 1 \times 96500 C \times 0.568 V K^{- 1} = - 54812 J K^{- 1}$
$= - 54.8 k J K^{- 1}$

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Similar questions

P t . H_{2} (1 a t m) | H^{+} (a q .) | | A g C l | A g

0.27 V

0.26 V

25^{\circ} C

35^{\circ} C

25^{\circ} C

P t | H_{2} (1 a t m) | H C l (0.01 M) | A g C l (s) | A g (s) a t 298 K

Δ G_{t}^{o}

^{o}

- 109.56 \frac{k J}{m o l}

- 130.79 \frac{k J}{m o l}

^{+}

^{-}

H_{2} (1 a t m) | H^{+} (p H = x) | |

25^{\circ} C

- 0.28 V

^{o}

^{o}

P t | H_{2} (g) | H C l (a q) | A g C l (s) | A g (s)

A g C l

^{o}

A g^{+} (a q) / A g (s)

^{o}

C d (s) | C d C l_{2} (a q, 0.1 M) | | A g C l (s) | A g (s)

C d (s) + 2 A g C l (s) \to 2 A g (s) + C d^{2 +} (a q) + 2 C l^{-} (a q)

0.6915 V

0.6753 V

Δ S

Δ H

F = 96485 C m o l^{- 1}

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