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jybe
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Homework Statement
For the reaction below, the constant pressure heat of reaction is qp = −3256 kJ mol−1 at 25 °C. What is the constant volume heat of reaction, qV , at 25 °C?
16 CO(g) + 33 H2(g) ⟶ C16H34(l) + 16 H2O(l)
Enter your answer in kJ mol−1, rounded to the nearest kilojoule.
Homework Equations
At constant pressure, the heat of reaction is equal to the enthalpy change
At constant volume, the heat of reaction is equal to the internal energy change: ΔH = ΔU + ΔnRT
ΔU = ΔH - ΔnRT
The Attempt at a Solution
ΔU = -3256kJ/mol - ΔnRT
Edit:
ΔU = -3256kJ/mol - (-49)(8.314x10^-3)(298.15)
ΔU = -3135 kJ/mol
Have I done it correctly?
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