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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.
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Solution 1

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/m Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.

Knowee AI  is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI  is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI  is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI  is a powerful AI-powered study tool designed to help you to solve study problem.
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