NEET 2023 Phase 1 · ChemistryPrevious Year Question

Which amongst the following options is the correct relation between change in enthalpy and change in internal energy?

Answer: (B) $Δ H = Δ U + Δ n_{g} R T$ . \textbf{Answer:} (B) $Δ H = Δ U + Δ n_{g} R T$ \textbf{Solution:} Enthalpy is defined as $H = U + p V$ .

A. $Δ H = Δ U - Δ n_{g} R T$
B. $Δ H = Δ U + Δ n_{g} R T$ ✓
C. $Δ H - Δ U = - Δ n_{g} R T$
D. $Δ H + Δ U = Δ n_{g} R$

Correct Answer

(B) $Δ H = Δ U + Δ n_{g} R T$

Solution & Explanation

\textbf{Answer:} (B) $Δ H = Δ U + Δ n_{g} R T$ \textbf{Solution:} Enthalpy is defined as $H = U + p V$ . For reactions involving ideal gases at constant temperature and pressure, $Δ (p V) = Δ (n_{g} R T) = Δ n_{g} R T$ , where $Δ n_{g}$ is the change in the number of moles of gas. Therefore $Δ H = Δ U + Δ n_{g} R T$ . Mapped: source lowercase answer 'b' → option B.

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