Calculate the amount of heat needed to transform, under standard conditions, 1.0 mol of liquid methanol...
Calculate the amount of heat needed to transform, under standard conditions, 1.0 mol of liquid methanol at 273 K to 1.0 mol of methanol vapor at 373 K. Assume that Cp,m for liquid methanol and for methanol vapor are independent of temperature. (Enthalpy of vaporization of methanol 35.3 KJ/mol-1, Cp,m of methanol 81.6 JK-1/mol)
Homework Answers
q1 = no of moles*Cp*
T
= 1*81.6*(373-273)
= 8160joules = 8.61KJ
q2 = no of moles*Enthalpy of vaporization of methanol
= 1*35.3 KJ/mol = 35.3KJ
q = q1 +q2
= 8.61 + 35.3
= 43.91Kj >>>>> answer
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