   Chapter 5, Problem 15PS

Chapter
Section
Textbook Problem

A 13.8-g piece of zinc is heated to 98.8 °C in boiling water and then dropped into a beaker containing 45.0 g of water at 25.0 °C. When the water and metal come to thermal equilibrium, the temperature is 27.1 °C. What is the specific heat capacity of zinc?

Interpretation Introduction

Interpretation:

At thermal equilibrium, the specific heat capacity for a given mass of zinc 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

Given,

Mass of zinc=13.8g

Mass of water=45g

Assume the sum of qzinc and qwater =0

[Cwater×Mwater(Tfinal-Tinitial)]+[CZn

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