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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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If 10. J of heat is applied to 5.0-g samples of each of the sub stances listed in Table 10.1, which substance’s temperature will increase the most? Which substance’s temperature wilt increase the least?

Interpretation Introduction

Interpretation:

The substances which have the most and the least increase in temperature listed in the table should be determined.

Concept Introduction:

Energy is the ability to do work or produce heat. The specific heat capacity is the amount of heat per unit mass needed to raise the temperature by 10 C.

DT=Qm×swhere, Q = energy or heat appliedm = mass of the substanceDT = change in temperatures = specific heat capacity of substance.

Explanation

It is given that the mass of each substance is 5.0 g and energy is 10J. Specific heat capacity of each substance is also given in the table. Substituting these values in the formula above, we can calculate the change in temperature for each substance.

ΔT=Qm×s

For water(liquid), DT=Qm×s=10J5.0g×4.184J/goC=0.49oCFor water(ice), DT=Qm×s=10J5.0g×2.03J/goC=0.98oCFor water(steam), DT=Qm×s=10J5.0g×2.0J/goC=1oCFor Aluminum, DT=Qm×s=10J5.0g×0.89J/goC=2.2oCFor Iron, DT=Qm×s=10J5

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