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Gibbs Free Energy & Spontaneity

For the react...

Question

For the reaction, ${A g}_{2} O (s) ⇌ 2 A g (s) + \frac{1}{2} O_{2} (g)$
$Δ H, Δ S, Δ T$ are $40.63 k J {m o l}^{- 1}, 1.808 J K^{- 1} {m o l}^{- 1}$ and $373.4 K$ respectively. Free energy change $Δ G$ of the reaction will be:

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Solution

$A g O (s) ⇌ 2 A g (s) + O_{2} (g)$
$△ G = △ H - T △ S$
$△ G = 40.63 * 10^{3} - 373.4 * 1.808$
$△ G = 675.103 J$
If $△_{r} G^{o} = 0$ , the reaction is at equilibrium
Therefore, $K C = 1$ , therefore, Concentration of reactants is equal to concentration of products.

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Similar questions

Δ H

Δ S

for the reaction,

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

30.56 k J m o l^{- 1}

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 :

Q. For reaction,

{A g}_{2} O (s) \to 2 A g (s) + (1 / 2) O_{2} (g)

Δ H = 30.56 k J {m o l}^{- 1}

Δ S = 66 J K^{- 1} {m o l}^{- 1}

. Temperature at which free energy change for reaction will be zero, is:

Δ H

Δ S

for the reaction,

{A g}_{2} O (s) ⟶ 2 A g (s) + \frac{1}{2} O_{2} (g)

30.56 k J {m o l}^{- 1}

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 forward above or below this temperature.

D e l t a H

D e l t a S

for the reaction

A g_{2} O_{(s)}

\to

2 A g_{(s)}

\frac{1}{2}

O_{2 (g)}

m o l^{- 1}

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

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

Q. For the reaction,

{A g}_{2} O ⇌ 2 A g (s) + \frac{1}{2} O_{2} (g)

Calculate the temperature at which free energy change is zero. At a temperature lower than this, predict whether the forward of the reverse reaction will be forward. Give reason
(

Δ H = + 30.56 k J; Δ S == + 0.066 k J K^{- 1} {m o l}^{- 1}

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