Calculate standard free energy change for the reaction 1-2 Cu s -1-2 Cl 2 g -1-2 Cu 2- Cl -taking place at in a cell whose standard e-m-f- is 1-02 volts A- -98430 JB- 98430 JC- -49215 JD- 96500 J

The correct option is A 98430 JΔ G= nFE^∘ ⇒Δ G = 1 × 96500 × 1.02 ⇒Δ G = 98430 ...

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Gibb's Energy and Nernst Equation

Calculate sta...

Question

Calculate standard free energy change for the reaction $\frac{1}{2} C u (s) + \frac{1}{2} C l_{2} (g) ⇌ \frac{1}{2} C u^{2 +} + C l^{-}$ taking place at in a cell whose standard e.m.f. is $1.02 v o l t s$

- 98430 J

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98430 J

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96500 J

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- 49215 J

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\frac{1}{2} C u (s) + \frac{1}{2} C l_{2} (g) ⇌ \frac{1}{2} C u^{2 +} + C l^{-}

1.02 v o l t s

N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g) a t 298 K .

△ H^{o} = - 92.4 k J m o l^{- 1}

△ S^{o} = - 198.3 J K^{- 1} m o l^{- 1}

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

- 10.26 k c a l m o l^{- 1}

25^{\circ} C

25^{\circ} C

P_{H_{2}} = 1 a t m . [H^{+}]

[C l^{-}] = 0.1

2.0 \times 10^{- 7}

P C l_{5 (g)} ⇌ P C l_{3 (g)} + C l_{2 (g)}

△ H^{o} = 28.40 k J m o l^{- 1} .

K_{c}

Δ G^{o} in k J m o l^{- 1}

K

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