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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\RightarrowGibb'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,Xwill be major component

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

amount ofX 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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