   # The specific heat capacity of silver is 0.24 J/ºC · g. a. Calculate the energy required to raise the temperature of 150.0 g Ag from 273 K to 298 K. b. Calculate the energy required to raise the temperature of 1.0 mole of Ag by l.0°C (called the molar heat capacity of silver). c. It takes 1.25 kJ of energy to heat a sample of pure silver from 12.0°C to 15.2°C. Calculate the mass of the sample of silver. ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 7, Problem 50E
Textbook Problem
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## The specific heat capacity of silver is 0.24 J/ºC·g.a. Calculate the energy required to raise the temperature of 150.0 g Ag from 273 K to 298 K.b. Calculate the energy required to raise the temperature of 1.0 mole of Ag by l.0°C (called the molar heat capacity of silver).c. It takes 1.25 kJ of energy to heat a sample of pure silver from 12.0°C to 15.2°C. Calculate the mass of the sample of silver.

(a)

Interpretation Introduction

Interpretation: The temperature change, absorbed heat and mass of silver should be determined.

Concept Introduction: The heat capacity C is defined as the ratio of heat absorbed to the temperature change. It can be given by,

C = heat absorbed/ temperature change

• Require heat for one gram of substance raise to its temperature by one degree Celsius is called specific heat capacity.

Specific heat capacity =  Absorbed heat (J)/ Temperature change(c)×mass ofsubstance (g)...(1)

Molar heat capacity =  Absorbed heat (J)/ Temperature change(c)×moleofsubstance (m)...(2)

From the above equation heat is:

q = S×M×T....(3)

q is heat (J)

M is mass of sample (g)

S is heat capacity

T is temperature change (C)

### Explanation of Solution

Given data:

Temperature change is 273 k to 298 k.

Mass of silver is 150 g.

Heat absorbed is 1.25 KJ.

Temperature change of pure silver 12.0°C to 15.2°C.

Atomic mass of silver is 107.9 g.

To determine: The amount of heat absorbs...

b)

Interpretation Introduction

Interpretation: The temperature change, absorbed heat and mass of silver should be determined.

Concept Introduction: The heat capacity C is defined as the ratio of heat absorbed to the temperature change. It can be given by,

C = heat absorbed/ temperature change

• Require heat for one gram of substance raise to its temperature by one degree Celsius is called specific heat capacity.

Specific heat capacity =  Absorbed heat (J)/ Temperature change(c)×mass ofsubstance (g)...(1)

Molar heat capacity =  Absorbed heat (J)/ Temperature change(c)×moleofsubstance (m)...(2)

From the above equation heat is:

q = S×M×T....(3)

q is heat (J)

M is mass of sample (g)

S is heat capacity

T is temperature change (C)

c)

Interpretation Introduction

Interpretation: The temperature change, absorbed heat and mass of silver should be determined.

Concept Introduction: The heat capacity C is defined as the ratio of heat absorbed to the temperature change. It can be given by,

C = heat absorbed/ temperature change

• Require heat for one gram of substance raise to its temperature by one degree Celsius is called specific heat capacity.

Specific heat capacity =  Absorbed heat (J)/ Temperature change(c)×mass ofsubstance (g)...(1)

Molar heat capacity =  Absorbed heat (J)/ Temperature change(c)×moleofsubstance (m)...(2)

From the above equation heat is:

q = S×M×T....(3)

q is heat (J)

M is mass of sample (g)

S is heat capacity

T is temperature change (C)

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