Answer:
0.2 kcal/mol is the value of [tex]\Delta G[/tex] for this reaction.
Explanation:
The formula used for is:
[tex]\Delta G_{rxn}=\Delta G^o+RT\ln Q[/tex]
[tex]\Delta G^o=-RT\ln K[/tex]
where,
[tex]\Delta G_{rxn}[/tex] = Gibbs free energy for the reaction
[tex]\Delta G_^o[/tex] = standard Gibbs free energy
R =Universal gas constant
T = temperature
Q = reaction quotient
k = Equilibrium constant
We have :
Reaction quotient of the reaction = Q = 46
Equilibrium constant of reaction = K = 35
Temperature of reaction = T = 25°C = 25 + 273 K = 298 K
R = 1.987 cal/K mol
[tex]\Delta G_{rxn}=-RT\ln K+RT\ln Q[/tex]
[tex]=-1.987 cal/K mol\times 298 K\ln [35]+1.987 cal/K mol\times 298K\times \ln [46][/tex]
[tex]=-2,105.21 cal/mol+2,267.04 cal/mol=161.82 cal/mol=0.16182 kcal/mol\approx 0.2 kcal/mol[/tex]
1 cal = 0.001 kcal
0.2 kcal/mol is the value of [tex]\Delta G[/tex] for this reaction.
