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Gibb's Energy and Nernst Equation

The standard ...

Question

The standard emf of the cell $F e | F e^{2 +} (a q) | | C d^{2 +} (a q) | C d$ is 0.0372 V and temperature coefficient of the cell is $- 1.25 \times 10^{- 4} V K^{- 1}$ . Which is/are correct about the cell (at 300 K)?

A

Δ G ° = 7.18 k J, Δ H ° = - 14.42 k J

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B

Δ G ° = - 7.18 k J, Δ H ° = 57.50 J

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C

Δ G ° = - 7.18 k J, Δ H ° = - 14.42 k J

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D

Δ S ° = - 24.125 {JK}^{- 1}, reaction is spontaneous

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Solution

The correct option is D $Δ S ° = - 24.125 {JK}^{- 1}, reaction is spontaneous$
The standard emf of the cell
$F e | F e^{2 +} (a q) | | C d^{2 +} (a q) | C d$
$E ° =$ 0.0372 V
$Δ G ° = - nFE ° = - 7.18 kJ$
$Δ S ° = n \times F \times {(\frac{\partial E_{Cell}}{\partial T})}_{P}$
$Δ S ° = 2 \times 96500 \times (- 1.25 \times 10^{- 4}) = - 24.125 {JK}^{- 1}$
$Δ G ° = Δ H ° - T Δ S °$
$- 7180 = - Δ H ° - 300 \times (- 24.125)$
$Δ H ° = - 14417.5 J$

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Similar questions

Q. The standard emf of the cell

F e | F e^{2 +} (a q) | | C d^{2 +} (a q) | C d

is 0.0372 V and temperature coefficient of the cell is

- 1.25 \times 10^{- 4} V K^{- 1}

. Which is/are correct about the cell (at 300 K)?

Q. The standard emf of the cell

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

in which the cell-reaction is

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

273

0.6573

298

K. Calculate enthalpy change of the reaction at

298

Q. The standard emf of the cell,

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

In which the cell reaction is

C d_{(s)} + 2 A g C l_{(s)} \Rightarrow 2 A g_{(s)} + C d_{(a q)}^{2 +} + 2 C l_{(a q)}^{-}

0.6915 V

0^{o} C

0.6573

V

25^{o} C

The enthalpy change of the reaction at

25^{o} C

Q. The standard electrode potential

E^{⊖}

and its temperature coefficient

(\frac{d E^{⊖}}{d T})

2 V

- 5 \times 10^{- 4} V K^{- 1}

300 K

respectively. The cell reaction is

Z n (s) + C u^{2 +} (a q) \to Z n^{2 +} (a q + C u (s)

The standard reaction enthalpy

(△_{r} H^{⊖})

300 K

k J m o l^{- 1}

[U s e R = 8 j K^{- 1} m o l^{- 1}

F = 96, 000 C m o l^{- 1}]

For the following cell-reaction,

C u (s) + 2 A g^{+} (a q) \to 2 A g (s) + C u^{2 +} (a q)

E_{c e l l}

0.46 V

300 K

0.48 V

310 K

The temperature coefficient of the e.m.f of the cell in above questions is:

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