NEET Chemistry Gibbs Free Energy MCQ Question
For a reaction at 298 K, the change in enthalpy (∆H sys) is -150 kJ/mol and the change in entropy (∆S sys) is 200 J/mol·K. Calculate the Gibbs free energy change (∆G) for the reaction. Which of the following values is correct?
-90 kJ/mol
-210 kJ/mol
-190 kJ/mol
-150 kJ/mol
Correct Answer
Detailed Explanation
Using the formula ∆G = ∆H sys - T∆S sys, convert ∆S sys to kJ (200 J/mol·K = 0.2 kJ/mol·K): ∆G = -150 kJ/mol - (298 K × 0.2 kJ/mol·K) = -150 kJ/mol - 59.6 kJ/mol = -90.4 kJ/mol, approximated to -90 kJ/mol.
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