Chemistry-Gibbs Free Energy
NEET Chemistry Gibbs Free Energy MCQ Question
Type: MCQ-numerical-Easy-Class 11
If 1 mole of water is vaporized at 1 bar pressure and 100°C, what is the change in internal energy (ΔU) given that the change in enthalpy (ΔH) is 41.00 kJ/mol and the gas constant (R) is 8.3 J/mol K?
A
37.904 kJ/mol
B
41.000 kJ/mol
C
096 kJ/mol
D
44.096 kJ/mol
Correct Answer
Option A
Detailed Explanation
Using the formula ΔU = ΔH - ΔngRT, where Δng is 1 and T is 373 K, we get ΔU = 41.00 kJ/mol - 3.096 kJ/mol = 37.904 kJ/mol.
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