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Standard XII

Chemistry

Gibb's Energy and Nernst Equation

DeltaH and De...

Question

$D e l t a H$ and $D e l t a S$ for the reaction $A g_{2} O_{(s)}$ $\to$ $2 A g_{(s)}$ + $\frac{1}{2}$ $O_{2 (g)}$ are 30.56 kJ $m o l^{- 1}$ 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:

463 K

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35440 K

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20 K

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483 K

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Solution

The correct option is A 463 K
According to Gibb's Helmholtz equation,
$Δ G = Δ H - T Δ S A t e q u i l i b r i u m, Δ G = 0 S o t h a t, 0 = Δ H - T Δ S o r Δ H = T Δ S o r T = \frac{Δ H}{Δ S} H e n c e, Δ H = 30.56 k J m o l^{- 1} = 30560 k J m o l^{- 1}, Δ S = 66.0 J K^{- 1} m o l^{- 1} ∴ T = \frac{30.560}{66.0} = 463 K$

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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 :

Q. 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:

Δ H

and

Δ S

for the reaction,

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

are

30.56 k J {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 forward above or below this temperature.

$△ H$ 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.

△ H a n d △ 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

66.0 J K^{- 1}

respectively. Calculate the temperature at which free energy change for the reaction will be zero. Predict whether the forward reaction will be favoured above or below this temperature (in K)

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DeltaH and DeltaS for the reaction Ag2O(s) → 2Ag(s)+12 O2(g) are 30.56 kJ mol−1 and 66.00 JK−1mol−1 respectively, the temperature at which the free energy change for the reaction will be zero is:

The correct option is A 463 KAccording to Gibb's Helmholtz equation, ΔG=ΔH−TΔSAt equilibrium,ΔG=0So that,0=ΔH−TΔS or ΔH=TΔS orT=ΔHΔSHence,ΔH=30.56kJmol−1=30560kJmol−1,ΔS=66.0JK−1mol−1∴T=30.56066.0=463K

$D e l t a H$ and $D e l t a S$ for the reaction $A g_{2} O_{(s)}$ $\to$ $2 A g_{(s)}$ + $\frac{1}{2}$ $O_{2 (g)}$ are 30.56 kJ $m o l^{- 1}$ 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: