   Chapter 5, Problem 98IL

Chapter
Section
Textbook Problem

A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction isC2H5OH(ℓ) + 3 O2(g) → 2 CO2(g) + 3 H2O(ℓ)The bomb had a heat capacity of 550 J/K, and the calorimeter contained 650 g of water. Burning 4.20 g of ethanol, C2HsOH(ℓ) resulted in a rise in temperature from 18.5 °C to 22.3 °C. Calculate ΔU for the combustion of ethanol, in kJ/mosl.

Interpretation Introduction

Interpretation:

The change in internal energy for the combustion of ethanol has to be determined.

Concept Introduction:

Sum of all energies transferred as heat in the system

qr+qbomb+qwater=0

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=550J/K

Mass of ethanol=4.20g

Mass of water=650g

qwater=4.184JK/g(650g)(3.8K)=10334J= 10.334kJ

qbomb=550J/K×3.8K =2090J=2

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