For the hypothetical reaction: A(g) + B(g) → AB(g); ΔC P [J K -1 ] = 3.0 × 10 -2 T [/K] and ΔH 200 = -4.80 kJ/mol. Estimate the absolute temperature (in K) at which ΔH = 0 for this reaction.

ΔH T = ΔH 200 + ∫ 200 T 3.0×10 -2 T dT = -4800 + 1.5×10 -2 (T 2 - 200 2 ) J. Set to zero: T 2 - 40000 = 4800/0.015 = 320000, so T 2 = 360000 and T = 600 K. The answer is 0600.

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Chemistry - Thermochemistry Question with Solution | TestHub

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For the hypothetical reaction: A(g) + B(g) → AB(g); ΔC_P [J K^-1] = 3.0 × 10^-2 T [/K] and ΔH₂₀₀ = -4.80 kJ/mol. Estimate the absolute temperature (in K) at which ΔH = 0 for this reaction.

Answer:

600.00

Solution:

ΔH_T = ΔH₂₀₀ + ∫₂₀₀^T 3.0×10^-2 T dT = -4800 + 1.5×10^-2 (T² - 200²) J. Set to zero: T² - 40000 = 4800/0.015 = 320000, so T² = 360000 and T = 600 K. The answer is 0600.

Stream:JEESubject:ChemistryTopic:ThermochemistrySubtopic:Enthalpy of Reaction

⏱ 2mℹ️ Source: QB

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