Question

The value of the equilibrium constant for a reaction is 2.65 x 10-6 at 35° Calculate the value of LaTeX: \DeltaΔG°rxn.

Answer 1

Answer:

The answer is "33.95 $\bold{ \frac{kj}{mol}}$".

Explanation:

Formula:

$\bigtriangleup G_0= -R \times T l_n \times K_{eq}$

where

$K_{eq} = \text{equilibrium constant}$

Given value:

$T =35^{\circ} C$

convert temperature celsius (°C) to Kelvin (K):

$= (273+45) \ kelvin \\\\= 318 \ Kelvin \\\\= 318 \ K$

$R = 8.314 \ \ \frac{J}{ mol \cdot K}$

$\bigtriangleup G_0= -(8.314 ) \times 31.8 \times l_n (2.65\times 10^{-6})$

        $=-(8.314 ) \times 31.8T l_n \times (2.65\times 10^{-6})$

After solving the value it will give:

        = 33.95  $\bold{ \frac{kj}{mol}}$