Question

A chemist fills a reaction vessel with 9.47 atm nitrogen monoxide (NO) gas, 2.61 atm chlorine (C12) gas, and 8.64 atm nitrosyl chloride (NOCI) gas at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction:
2NO(g) + Cl2(g) <=> 2NOCI (g)

Answer 1

Answer:

$\Delta _rG=2832.2J/mol$

Explanation:

Hello,

In this case, the Gibbs free energy of that reaction is computed by computing the equilibrium constant as:

$K=\frac{p_{NOCl}^2}{p_{NO}^2p_{Cl_2}} =\frac{8.64^2}{9.47^2*2.61}=0.319$

Hence the Gibbs free energy:

$\Delta _rG=-RTlog(K)=-8.314\frac{J}{mol*K}*298.15K*ln(0.319)\\\\\Delta _rG=2832.2J/mol$

Best regards.