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Question: one mole of npentane liquid is in a cylinder with...

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One mole of n-pentane liquid is in a cylinder with a piston at the top. Above the piston is atmospheric pressure. The piston moves to keep the pressure constant. The system is initially at 25 C. At the start of the process, the system is heated to its boiling point (36 C), and then the liquid is converted to vapor. The heating continues until the system reaches 50 C. This completes the process. If you assume no heat loss to the surroundings, how much heat is required for this process? Note: Make simplifying assumptions (state them) to help you solve the problem. See the book Appendix for the molar volume of the n-pentane. See the table below for potentially-useful data

Property (for n-pentane)

Value

Units

Enthalpy of vaporization (at 1 bar)

25790

J/mol

Internal energy of vaporization (at 1 bar)

23357

J/mol

Heat capacity of the liquid, constant pressure

167.19

J/mol-K

Heat capacity of the liquid, constant volume

128.13

J/mol-K

Heat capacity of the vapor, constant pressure

127.27

J/mol-K

Heat capacity of the vapor, constant volume

116.88

J/mol-K

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