Question

The equilibrium concentrations of the species in the reaction \[ \mathrm{A} + \mathrm{B} \rightleftharpoons \mathrm{C} + \mathrm{D} \] are 2, 3, 10 and 6 mol L^-1, respectively at 300 K. ΔGº for the reaction is (R = 2 cal/mol K)

विकल्प

• -137.26 cal

• -1381.80 cal

• -13.73 cal

• 1372.60 cal

Answer 1

-1381.80 cal

Explanation:

The given reaction is \[ \mathrm{A} + \mathrm{B} \rightleftharpoons \mathrm{C} + \mathrm{D} \]

[A] = 2 mol L^-1 

[B] = 3 mol L^-1

[C] = 10 mol L^-1

[D] = 6 mol L^-1

\[\Delta G^{0}=-2.303\mathrm{RT}\log\mathrm{K}_{\mathrm{cq}}\]

\[=-2.303\mathrm{RT}\log\frac{[C][D]}{[A][B]}\]

\[=-2.303\times2\times300\times\log\frac{10\times6}{2\times3}\]

= - 2.303 × 2 × 300 × log 10 

= - 1381.8 cal