Question

If a reaction at 37°C has a ΔH of 23 kJ/mol and a ΔS of 337 J/Kmol, what is the ΔG for the reaction?

a) 310 kJ/mol
b) -310 kJ/mol
c) 13.7 kJ/mol
d) -13.7 kJ/mol

Answer 1

The standard Gibbs free energy change (ΔG) for a reaction at a given temperature can be calculated using the equation ΔG = ΔH - TΔS. In this case, the ΔG value is -13.7 kJ/mol.

Step-by-step explanation:

The standard Gibbs free energy change (ΔG) for a reaction at a given temperature can be calculated using the equation ΔG = ΔH - TΔS, where ΔH is the enthalpy change, ΔS is the entropy change, and T is the temperature in Kelvin.

In this case, the given values are ΔH = 23 kJ/mol and ΔS = 337 J/Kmol. To calculate ΔG, we need to convert the units of ΔS to kJ/Kmol by dividing by 1000. Substituting the values into the equation, we get: ΔG = 23 kJ/mol - (37°C + 273.15 K) * (337 J/Kmol / 1000 J/kcal) = -13.7 kJ/mol.

Therefore, the answer is (d) -13.7 kJ/mol.