578,070 J of heat is requred to raise the temperature of 15.0 moles of liquid methanol, CH3OH, from 25.0 °C to its boiling point (64.6 °C) and then to completely evaporate the methanol at that temperature. The specific heat of liquid methanol is 2.53 J g-1 K-1 vaporisation of the compound. Calculate the enthalpy of vapourisation of the compound?
578,070 J of heat is requred to raise the temperature of 15.0 moles of liquid methanol, CH3OH, from 25.0 °C to its boiling point (64.6 °C) and then to completely evaporate the methanol at that temperature. The specific heat of liquid methanol is 2.53 J g-1 K-1 vaporisation of the compound. Calculate the enthalpy of vapourisation of the compound?
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter7: Chemical Energy
Section: Chapter Questions
Problem 62E: In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of...
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(i) 578,070 J of heat is requred to raise the temperature of 15.0 moles of liquid methanol, CH3OH, from 25.0 °C to its boiling point (64.6 °C) and then to completely evaporate the methanol at that temperature. The specific heat of liquid methanol is 2.53 J g-1 K-1 vaporisation of the compound. Calculate the enthalpy of vapourisation of the compound?
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