Calculate the standard cell potential at 25 ∘c for the reaction x(s)+2y+(aq)→x2+(aq)+2y(s) where δh∘ = -793 kj and δs∘ = -319 j/k . express your answer to three significant figures and include the appropriate

First we will calculate free energy change:
ΔG₀ = ΔH₀ - (T * ΔS₀)
= - 793 kJ - (298 * - 0.319 kJ/K) = - 698 kJ
We know the relation between free energy change and cell potential is:
ΔG₀ = - n F E⁰ where
F = Faraday's constant = 96485 C/mol
n = 2 (given by equation that the electrons involved is 2)
ΔG₀ = - 2 x 96485 x E⁰
- 698 kJ = - 2 x 96485 x E⁰
E⁰ = (698 x 1000) / (2 x 96485) = 3.62 volts

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batolisis batolisis · Answer 2 · 2022-03-17T15:46:09+01:00

The standard cell potential at 25°C is : 3.62 volts

Given data :

Δ h = -793 kJ

Δ s = -319 J/k = 0.319 kJ/k

Temperature = 25°C = 298 k

Determine the standard cell potential

We will apply the relation below

ΔG = Δh - TΔ s

= - 793 - 298 * - 0.319

= -697.938 KJ/mole

= -697938 J/mole

X (s) + 2Y⁺(aq) ---> X²⁺(aq) + 2Y(s)

n = 2

Final step : Calculate the standard cell potential ( EoCell )

ΔGo = -n * Eocell * F

-697938 = -2 * Eocell * 96500

therefore : Eocell = - 697938 / ( -2 * 96500 )

= -697938 / -193000

= 3.62 V

Hence we can conclude that the standard cell potential at 25°C = 3.62 V

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