Respuesta :
Answer:
The value of ΔG° of the reaction is 5704.82 J/mol.
Explanation:
A + B ⇄ C + D
Equilibrium concentrations of reactants an products:
[A] = 10 μM, [B] = 15 μM, [C] = 3 μM, and [D] = 5 μM
An equilibrium constant of the reaction can be written as:
[tex]K=\frac{[C][D]}{[A][B]}[/tex]
[tex]K=\frac{3 \mu M\times 5 \mu M}{10 \mu M\times 15 \mu M}=0.1[/tex]
[tex]\Delta G^o=-RT\ln K_1[/tex]
where,
R = Gas constant = [tex]8.314J/K mol[/tex]
T = temperature = [tex]25^oC=[273+25]K=298K[/tex]
[tex]K_1[/tex] = equilibrium constant at 25°C = 0.1
Putting values in above equation, we get:
[tex]\Delta G^o=-(8.314J/Kmol)\times 298K\times \ln (0.1)[/tex]
[tex]\Delta G^o=5704.82 J/mol[/tex]
The value of ΔG° of the reaction is 5704.82 J/mol.
