Calculate the Gibbs free energy change (in kJ/mol) when Δ𝐻∘ = 910.1 kJ/mol, Δ𝑆∘ = 744.1 J/mol*K, and T = 261.3 K.
Question
Calculate the Gibbs free energy change (in kJ/mol) when Δ𝐻∘ = 910.1 kJ/mol, Δ𝑆∘ = 744.1 J/mol*K, and T = 261.3 K.
Solution
The Gibbs free energy change (ΔG) can be calculated using the formula:
ΔG = ΔH - TΔS
where: ΔH is the change in enthalpy, T is the absolute temperature in Kelvin, and ΔS is the change in entropy.
Given: ΔH = 910.1 kJ/mol, ΔS = 744.1 J/mol*K, and T = 261.3 K.
First, we need to convert ΔS from J/molK to kJ/molK because ΔH is given in kJ/mol.
1 kJ = 1000 J, so ΔS = 744.1/1000 = 0.7441 kJ/mol*K.
Now we can substitute the values into the formula:
ΔG = ΔH - TΔS = 910.1 kJ/mol - 261.3 K * 0.7441 kJ/mol*K = 910.1 kJ/mol - 194.4 kJ/mol = 715.7 kJ/mol
So, the Gibbs free energy change is 715.7 kJ/mol.
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