   Chapter 10, Problem 74AP ### 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
90 views

# A 50.1)-g sample of water at 100. °C is poured into a 50.0-g sample of water at 25 °C. What will be the final temperature of the water?

Interpretation Introduction

Interpretation:

The final temperature of the 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

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)

Putting the values for sample 1:

Q1=(50 g)(4.184 J/g C)(T2100 C)

Similarly, for sample 2:

Q2=(50 g)(4.184 J/g C)(T225 C)

On adding both the samples, the temperature of same of sample 2 decreases and that of sample 1 increases, thus, the change is same but in opposite direction or, Q1=Q2

Or,

Q1+Q2=0

Putting the values,

(50 g)(4.184 J/g C)(T2100 C)+(50 g)(4

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