   Chapter 14.2, Problem 14.1SC ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
21 views

# trong>Exercise 14.1 Calculate the total energy required to melt 15 g of ice at 0   ° C , heat the water to 1 00   ° C , and vaporize it to steam at 1 00   ° C .

Interpretation Introduction

Interpretation:

The total energy required to melt 15g of ice at 0° C, heat the water at 100° C and vaporize it to steam at 100° C should be calculated.

Concept Introduction:

The amount of heat energy needed to melt 1 g of ice at 0° C is known as the heat of fusion. The value of heat of fusion of ice is 335J/g.

The amount of heat energy needed to increase the temperature of a given mass of water is calculated by the following equation:

Heat energy needed = m×s×Δt

Here,

• m = mass of water.
• s = specific heat of water =4.186 J/goC.
• Δt = change in temperature of water.

The amount of heat energy needed to vaporize 1 g of water at 100° C is known as the heat of vaporization. The value of heat of vaporization of water is 2260 J/g.

Explanation

Mass of ice at 0° C = 15 g

The amount of heat energy needed to melt 15 g of ice at 0° C

=335 J/g×15 g=5025 J

The amount of heat energy needed to increase the temperature of 15 g water from 0° C to 100° C =15×4.186×100 J=6279 J

The amount of heat energy needed to vap

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