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For the chemical reaction $X\: \rightleftharpoons \: Y$ , the standered reaction Gibbs energy depend on temperature T (in K) as

$\Delta _{r}G^{0} \left ( in \: k\: mol^{-1} \right )\: = \: 120\: -\frac{3}{8}T$ .

The major component of the reaction mixture at T is :

Option 1)

Y if T = 300 K
Option 2)

Y if T = 280 K
Option 3)

X if T = 350 K
Option 4)

X if T = 315 K

Answers (1)

best_answer

Δ G for reversible reaction -

$\Delta G= \Delta G^{0}+2.303 RT \log Q$

- wherein

$\Delta G\Rightarrow$ Gibb's free energy at standard condition

$R\Rightarrow$ Universe gas constant

$T\Rightarrow$ Temperature

$Q\Rightarrow$ Reaction Quotient

Δ G of equilibrium -

$\Delta G_{0}= -2.303 RT \log K_{c}$

- wherein

At Equilibrum

$\Delta G= 0$

and $Q= K_{c}$

Spontanous process -

$\Delta G=\Delta H-T\Delta S$

- wherein

For spontanouse process $\Delta G$ must be negative.

As we learnd

At $T=315K,X$ will be major component

$\Delta G= 120-\frac{3}{8}\times 315= 1.875> 0$

amount of $X$ will be greater at this temperature at equilibirium

Option 1)

Y if T = 300 K

Option 2)

Y if T = 280 K

Option 3)

X if T = 350 K

Option 4)

X if T = 315 K

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