Calculate Δ S univ (in J/K) for N 2 (g) + 3H 2 (g) → 2NH 3 (g); Δ H ° 300 = -90 kJ. Standard entropies of N 2 , H 2 and NH 3 are 192, 131 and 192 J/K-mol, respectively.

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ChemistryThermodynamics - IIDS in chemical reactionMedium2 minQB

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Calculate Δ S_univ (in J/K) for N₂(g) + 3H₂(g) → 2NH₃(g); Δ H^°₃₀₀ = -90 kJ. Standard entropies of N₂, H₂ and NH₃ are 192, 131 and 192 J/K-mol, respectively.

Answer:

99.00

Solution:

Δ S_sys = 2(192) - (192 + 3×131) = 384 - 585 = -201 J/K. Δ S_surr = 90000/300 = 300 J/K. Δ S_univ = 300 - 201 = 99 J/K. Ans = 0099.

Stream:JEESubject:ChemistryTopic:Thermodynamics - IISubtopic:DS in chemical reaction

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