You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XI

Chemistry

Gibbs Free Energy & Spontaneity

H and S for t...

Question

$△ H$ 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.

298 K, above

No worries! We‘ve got your back. Try BYJU‘S free classes today!

300 K, below

No worries! We‘ve got your back. Try BYJU‘S free classes today!

373 K, above

No worries! We‘ve got your back. Try BYJU‘S free classes today!

463 K, above

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

Solution

The correct option is D
463 K, above

We know that, $△ G = △ H - T △ S$
At equilibrium, $△ G$ = 0
So that 0 = $△ H - T △ S$
or $T = \frac{△ H}{△ S}$
given that $△ H$ - 30.56 kJ $m o l^{- 1}$ = 30560 J $m o l^{- 1}$
$△ S$ = 66.0 J $K^{- 1} m o l^{- 1}$
T = $\frac{30560}{66}$ = 463 K
Above this temperature, $△ G$ will be negative and the process will be spontaneous in forward direction.

Suggest Corrections

Similar questions

△ 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 m o l^{- 1} K^{- 1}

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

△ 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)

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 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)

$△ H$ 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.

Join BYJU'S Learning Program

△H and △S for the reaction: Ag2O(s)→2Ag(s)+12O2(g) are 30.56 kJ mol−1 and 66.0 J K−1mol−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.