For an exothermic reaction at constant pressure, what is the relationship between Δ H and Δ U?

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Question

For an exothermic reaction at constant pressure, what is the relationship between Δ H and Δ U?

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Δ H = Δ U Δ H < Δ U if Δ n_g < 0 Correct Δ H > Δ U if Δ n_g < 0 Δ H > Δ U if Δ n_g > 0

Explanation

For an exothermic reaction, Δ H < 0. If Δ n_g < 0 (fewer gas moles in products), Δ H < Δ U because Δ H = Δ U + Δ n_g RT and Δ n_g RT < 0. This follows from latest NCERT 2026-27 principle explaining the concept clearly for NEET students in simple steps as per rationalized syllabus.

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