   Chapter 12, Problem 36PS

Chapter
Section
Textbook Problem

The specific heat capacity of silver is 0.235 J/g · K. Its melting point is 962 °C, and its enthalpy of fusion is 11.3 kJ/mol. What quantity of energy, in joules, is required to change 5.00 g of silver from a solid at 25 °C to a liquid at 962 °C?

Interpretation Introduction

Interpretation:

The quantity of energy has to be calculated.

Concept introduction:

The energy can be calculated by using following formula,

q =m × c × ΔT

Explanation

The energy can be calculated by using following formula, q =m × c × ΔT Mass (m)=5.00 g/molec=0.235J/g.KΔT =962-(25)=937oC=937Kq1 =m × c × ΔT q1 =5g × 0.235J/g.K × 937K=1100.97q1 =1100.97

The energy can be calculated by using following formula, q =m × c × ΔT Mass (m)=5

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