Answer: -7956 J
Explanation:
Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as [tex]K_{eq}[/tex]
[tex]CO_2(g)+CCl_4(g)\rightleftharpoons 2COCl_2(g)[/tex]
The expression for [tex]K_{eq}[/tex] is written as:
[tex]K_{eq}=\frac{(p_{COCl_2})^2}{p_{CO_2}\times p_{CCl_4}^1}[/tex]
[tex]K_{eq}=\frac{[0.745]^2}{0.140\times 0.160}[/tex]
[tex]K_{eq}=24.8[/tex]
The Gibbs free energy is related to equilibrium constant by following relation:
[tex]\Delta G=-2.303RTlog K[/tex]
R = gas constant = 8.314 J/Kmol
T = temperature in kelvin =[tex]25^0C=25+273=298K[/tex]
K = equilibrium constant
[tex]\Delta G=-2.303RTlog K[/tex]
[tex]\Delta G=-2.303\times 8.314\times 298\times log(24.8)[/tex]
[tex]\Delta G=-7956J[/tex]
Thus ΔG for this reaction at 25 ∘C is -7956 J
