   Chapter 5, Problem 20PS

Chapter
Section
Textbook Problem

Chloromethane, CH3CI, arises from microbial fermentation and is found throughout the environment. It is also produced industrially, is used in the manufacture of various chemicals, and has been used as a topical anesthetic. How much energy is required to convert 92.5 g of liquid to a vapor at its boiling point, ―24.09 °C? (The heat of vaporization of CH3Cl is 21.40 kJ/mol.)

Interpretation Introduction

Interpretation:

The energy required to convert CH3Cl of definite mass of liquid to vapor at its boiling point has to be calculated.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1k.Energy gained or lost can be calculated using the below equation.

q=C×m×ΔT

Where,

q= energy gained or lost for a given mass of substance (m),

C =specific heat capacity

ΔT= change in temperature

Explanation

Given,

Mass of liquid =92.5g

Boiling point=-24.090C

Heat of vaporization=21.40KJ/mol

To vaporize at -24

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