The bomb calorimeter in Exercise 102 is filled with 987 g water. The initial temperature of the calorimeter contents is 23.32°C. A 1.056-g sample of benzoic acid (∆ E comb = −26.42 kJ/g) is combusted in the calorimeter. What is the final temperature of the calorimeter contents?

Q: Expert Answer

Interpretation Introduction Interpretation: Final temperature of calorimeter content has to be calculated. Concept introduction Calorimeter: The apparatus used to measure heat that involved in chemical reactions. Specific heat capacity: The specific heat capacity defined as quantity of heat required to raise temperature of the substance per unit mass. Explanation Explanation Record the given data Amount of water filled in bomb calorimeter =987g Initial temperature of calorimeter content =23 .32 0 C Quantity of combusted benzoic acid =1 .056g Change in energy of combustion =26 .42 kJ/g Specific heat of water = 4 .18 J/ 0 C Total heat capacity of the calorimeter = 6 .66 0 C (calculated in excercise number 102) Amount of water in bomb calorimeter, Initial temperature of calorimeter, amount of combusted benzoic acid and change in energy of combustion recorded as shown above. To calculate amount of heat released when 1.056 g benzoic acid combusted . Heat released = 1 .056g×26 .42 kJ/g = 27 .90 kJ The amount of heat released when 1.056g benzoic acid combusted has calculated by multiplying the value of energy change in combustion of benzoic acid with amount of benzoic acid. That is heat gain by water and calorimeter. To calculate temperature change. The heat gained by calorimeter which is equal to heat released when 1.056g benzoic acid combusted. To covert: Gram into Kilogram 9 .87g = 0 .987kg Heat gain= ( 4 .18 kJ 0 C kg ×0

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Chemistry: An Atoms First Approach

2nd Edition

Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

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Chemistry: An Atoms First Approach

2nd Edition

Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

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Interpretation Introduction

Interpretation: Final temperature of calorimeter content has to be calculated.

Concept introduction

Calorimeter: The apparatus used to measure heat that involved in chemical reactions.

Specific heat capacity: The specific heat capacity defined as quantity of heat required to raise temperature of the substance per unit mass.

Explanation of Solution

Explanation

Record the given data

Amount of water filled in bomb calorimeter =987g

Initial temperature of calorimeter content =23.320C

Quantity of combusted benzoic acid =1.056g

Change in energy of combustion =26.42 kJ/g

Specific heat of water = 4.18 J/0C

Total heat capacity of the calorimeter =6.660C (calculated in excercise number 102)

Amount of water in bomb calorimeter, Initial temperature of calorimeter, amount of combusted benzoic acid and change in energy of combustion recorded as shown above.

To calculate amount of heat released when 1.056 g benzoic acid combusted.

Heat released =1.056g×26.42 kJ/g

=27.90 kJ

The amount of heat released when 1.056g benzoic acid combusted has calculated by multiplying the value of energy change in combustion of benzoic acid with amount of benzoic acid. That is heat gain by water and calorimeter.

To calculate temperature change.

The heat gained by calorimeter which is equal to heat released when 1.056g benzoic acid combusted.

To covert: Gram into Kilogram

9.87g = 0.987kg

Heat gain=(4.18 kJ0C kg×0

The bomb calorimeter in Exercise 102 is filled with 987 g water. The initial temperature of the calorimeter contents is 23.32°C. A 1.056-g sample of benzoic acid (∆ E comb = −26.42 kJ/g) is combusted in the calorimeter. What is the final temperature of the calorimeter contents?

Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach