For N2(g) + 3H2(g) -> 2NH3(g) at 300 K, taking gases as ideal (R = 8.314 J mol^-1K^-1), the value of Delta H - Delta U is closest to

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For $N X_{2} (g) + 3 H X_{2} (g) 2 NH X_{3} (g)$ at $300 K$ , taking gases as ideal ( $R = 8.314 J mo l^{- 1} K^{- 1}$ ), the value of $Δ H - Δ U$ is closest to

Δ H = Δ U + Δ n_{g} RT

with

Δ n_{g} = 2 - 4 = - 2

. So

Δ H - Δ U = - 2 (8.314) (300) = - 4988 J