Question

Calculate the free energy change if the ratio of the concentrations of the products to the concentrations of the reactants is 22.7 and the temperature is 37.0 ° C ? Δ G ° ' for the reaction is − 16.7 kJ/mol .

Answer 1

Answer : The value of $\Delta G_{rxn}$ is -8.65 kJ/mol

Explanation :

The formula used for $\Delta G_{rxn}$ is:

$\Delta G_{rxn}=\Delta G^o+RT\ln Q$    ............(1)

where,

$\Delta G_{rxn}$ = Gibbs free energy for the reaction  = ?

$\Delta G_^o$ =  standard Gibbs free energy  = -16.7 kJ/mol

R = gas constant = $8.314\times 10^{-3}kJ/mole.K$

T = temperature = $37.0^oC=273+37.0=310K$

Q = reaction quotient = 22.7

Now put all the given values in the above formula 1, we get:

$\Delta G_{rxn}=(-16.7kJ/mol)+[(8.314\times 10^{-3}kJ/mole.K)\times (310K)\times \ln (22.7)$

$\Delta G_{rxn}=-8.65kJ/mol$

Therefore, the value of $\Delta G_{rxn}$ is -8.65 kJ/mol