   Chapter 5, Problem 11PS

Chapter
Section
Textbook Problem

A 45.5-g sample of copper at 99.8 °C is dropped into a beaker containing 152 g of water at 18.5 °C. What is the final temperature when thermal equilibrium is reached?

Interpretation Introduction

Interpretation:

At thermal equilibrium, the final temperature for a given copper placed in a beaker containing water has to be determined.

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

Assume the sum of qcopper and qwater =0

Final temperature can be calculated as,

[Cwater×Mwater(Tfinal-Tinitial)]+[CCu×MCu(T

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