For reaction- Ag 2 O s - 2Ag s - 1 - 2 O 2 g - the value of - H-30-56 kJ mol -1 and - S-66 J K -1 mol -1- Temperature at which free energy change for reaction will be zero- is-

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Standard XII

Chemistry

Gibbs Free Energy & Spontaneity

For reaction,...

Question

For reaction, ${A g}_{2} O (s) \to 2 A g (s) + (1 / 2) O_{2} (g)$ , the value of $Δ H = 30.56 k J {m o l}^{- 1}$ and $Δ S = 66 J K^{- 1} {m o l}^{- 1}$ . Temperature at which free energy change for reaction will be zero, is:

373 K

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413 K

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463 K

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493 K

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Solution

The correct option is C $463 K$
As we know at $Δ G = 0$ , the equilibrium is attained.
$Δ G = Δ H - T Δ S$
$T Δ S = Δ H$ ( as $Δ G = 0$ )
$T = \frac{Δ H}{Δ S}$
$T = \frac{30.56 \times 10^{3}}{66} K$ .
So, the temperature at which free energy change for the reaction will be zero is 463 K.

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Similar questions

Δ H

and

Δ S

for the reaction,

A g_{2} O_{(s)} \to 2 A g (s) + \frac{1}{2} O_{2} (g)

, are

30.56 k J m o l^{- 1}

and

66.00 J K^{- 1} m o l^{- 1}

respectively. The temperature at which the free energy change for the reaction will be zero is :

$△ H$ and $△ S$ for the reaction: $A g_{2} O (s) \to 2 A g (s) + \frac{1}{2} O_{2} (g)$ are 30.56 kJ $m o l^{- 1}$ and 66.0 J $K^{- 1} m o l^{- 1}$ respectively. Calculate the temperature at which free energy change for the reaction will be zero. Predict whether the forward reaction will be favored above or below this temperature.