   Chapter 10, Problem 87CP ### 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
28 views

# A swimming pool, 10.0 in by 4.0 m, is filled with water to a depth of 3.0 m at a temperature of 20.2 °C. How much energy is required to raise the temperature of the water to 24.6 °C?

Interpretation Introduction

Interpretation:

The heat required to raise the temperature of water should be calculated.

Concept Introduction:

The specific heat is defined as the amount of heat per unit mass needed to raise the temperature by one degree Celsius.

It is mathematically represented as follows:

Q=msΔT

Here, Q is heat, m is mass, s is specific heat capacity and ΔT is change in temperature.

Explanation

Given Information:

The length, width and depth of swimming pool is 10.0 m, 4.0 m and 3.0 m respectively. The initial temperature of water is 20.2 C and final temperature is 24.6 C

Calculation:

From table 10.1, the specific heat capacity of water (liquid) is 4.184 J/g C

The heat required can be calculated using the following equation:

Q=msΔT

Or,

Q=ms(T2T1)

To calculate the heat required, first calculate the mass of water.

It is related to density as follows:

d=mV

The volume of water will be equal to the volume of the swimming pool. It is calculated as follows:

V=l×w×d

Here, l is length, w is width and d is depth.

Putting the values,

V=(10.0 m)(4.0 m)(3

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