   Chapter 11.6, Problem 11.5CYU

Chapter
Section
Textbook Problem

The molar enthalpy of vaporization of methanol, CH3OH, is 35.2 kJ/mol at 64.6 °C How much energy is required to evaporate 1.00 kg of methanol at 64.6 °C?

Interpretation Introduction

Interpretation:

The energy required to vaporize the given volume of water is to be identified.

Concept Introduction:

Clausius-Clapeyron Equation: This equation relates the heat of transformation of vaporization or condensation to the rate of change of vapour pressure with temperature.

The energy required to overcome the intermolecular forces of attraction for 1mol of a substance is called standard enthalpy of vaporization,ΔvapH0

Explanation

The molar enthalpy of vaporization

The amount of heat is required 1 mole of the substance at boiling point.

Given density=0.958g/cm3

Volume=1Kg =1×103g

ΔvapH0=+35

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