   Chapter 5, Problem 23PS

Chapter
Section
Textbook Problem

Ethanol, C2HsOH, boils at 78.29 °C. How much energy, in joules, is required to raise the temperature of 1.00 kg of ethanol from 20.0 °C to the boiling point and then to change the liquid to vapor at that temperature? (The specific heat capacity of liquid ethanol is 2.44 J/g · K, and its enthalpy of vaporization is 855 J/g.)

Interpretation Introduction

Interpretation:

The energy needed to raise the temperature of ethanol to its boiling point and then to vaporize 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,

Boiling point of ethanol= 78.290C

Specific heat capacity=2.44JK/g

Heat of vaporization=855J/g

Mass=1Kg =1000g

q1= To increase the temperature from 200C to 78.290C

q=C×m×ΔT

Substitute for the equation as

q1=2.44JK/g×1000g(351.29K-293K)

q1=142227.6J

q2= Vaporize from 78

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