Assuming that water vapor is an ideal gas, the internal energy change (ΔUΔU) when 1 mole of water is vaporized at 1 bar pressure and 100∘C100∘C (molar enthalpy of vaporization of water at 1 bar and 373 K = 41 kJ/mol and R = 8.314 J/Kmol) will be
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Answered by
9
It can be solved by the formula
∆U=∆H-∆ngRT
here, ∆H is 41KJ/mol.
please mark it as brainliest answer
∆U=∆H-∆ngRT
here, ∆H is 41KJ/mol.
please mark it as brainliest answer
Answered by
15
Answer:
37.904
Explanation:
by solving in the formula
∆ u = ∆ h- ∆ nrt
= 41 -1× 8.3×373×10^-3
= 37.904
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