   Chapter 5.6, Problem 5.8CYU

Chapter
Section
Textbook Problem

A 1.00-g sample of ordinary table sugar (sucrose, C12H22O11) is burned in a bomb calorimeter. The temperature of 1.50 × 103 g of water in the calorimeter rises from 25.00 °C to 27.32 °C. The heat capacity of the bomb is 837 J/K, and the specific heat capacity of the water is 4.20 J/g · K. Calculate (a) the heat evolved per gram of sucrose and (b) the heat evolved per mole of sucrose.

(a)

Interpretation Introduction

Interpretation:

Heat of combustion per gram of sucrose should be calculated.

Concept Introduction:

Standard enthalpy

Standard enthalpy of the reaction,ΔrHo, is the change in enthalpy that happens when matter is transformed by a given chemical reaction, when all reactants and products are in their standard states.

Enthalpy of the reaction,ΔrH, is the change in enthalpy that happens when matter is transformed by a given chemical reaction

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,

Specific heat capacity of bomb, Cbomb is 837JK

Specific heat capacity of bomb, Cwater is 4.20JK/g

Mass of water=1.50×103g

ΔT= 25.000C-27.320C=2.320C=2.32K

Assume qr+ qwater+ qbomb= 0

Heat of combustion per gram can be calculated from q = C × m × ΔT, as

qwater= Cwater × mwater × ΔT

Substitute the values for the above equation,

qwater =4

(b)

Interpretation Introduction

Interpretation:

Heat of combustion per mole of sucrose should be identified.

Concept Introduction:

Standard enthalpy

Standard enthalpy of the reaction,ΔrHo, is the change in enthalpy that happens when matter is transformed by a given chemical reaction, when all reactants and products are in their standard states.

Enthalpy of the reaction,ΔrH, is the change in enthalpy that happens when matter is transformed by a given chemical reaction

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.

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