For water at 100°C and 1 bar, ΔᵥₐₚH - ΔᵥₐₚU = _______ × 10² J mol⁻¹ (Round off to the Nearest integer) [Use: R = 8.31 J mol⁻¹ K⁻¹] [Assume volume of H₂O(l) is much smaller than volume of H₂O(g). Assume H₂O(g) can be treated as an ideal gas]
For water at 100°C and 1 bar, ΔᵥₐₚH - ΔᵥₐₚU = _______ × 10² J mol⁻¹ (Round off to the Nearest integer) [Use: R = 8.31 J mol⁻¹ K⁻¹] [Assume volume of H₂O(l) is much smaller than volume of H₂O(g). Assume H₂O(g) can be treated as an ideal gas]
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1 Answer
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H? O (l) → H? O (g)
ΔH° = ΔU° + ΔngRT
ΔH° - ΔU° = ΔngRT
= 1 × 8.31 × 373
= 3099.63 J/mol
= 30.9963 × 10² J/mol
≈ 31 × 10² J/mol
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