   Chapter 5, Problem 94IL

Chapter
Section
Textbook Problem

A 192-g piece of copper is heated to 100.0 °C in a boiling water bath and then dropped into a beaker containing 751 g of water (density = 1.00 g/cm3) at 4.0 °C. What was the final temperature of the copper and water after thermal equilibrium was reached? (CCu = 0.385 J/g · K.)

Interpretation Introduction

Interpretation:

At thermal equilibrium final temperature of copper and water 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 values are:

Mass of the copper is 192g

Specific heat capacity of water is 0.385J/gK

Mass of water is 751g

Initial temperature of copper is 1000C

Initial temperature of copper is 40C

Assume qmetal=-qwater

Substitute values in q=C×m×ΔT

192g×0

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