A bomb calorimetry experiment is performed with xylose, C_5H_10O_5(s), as the co

Question

A bomb calorimetry experiment is performed with xylose, C_5H_10O_5(s), as the combustible substance. The data obtained are mass of xylose burned: 1.183 g heat capacity of calorimeter: 4.728 kJ/C degree initial calorimeter temperature: 23.28 C degree final calorimeter temperature: 27.19 C degree What is the heat of combustion of xylose, in kilojoules per mole? Write the chemical equation for the complete combustion of xylose. Express your answer as a chemical equation. Identify all of the phases in your answer.

Explanation / Answer

A)

heat = heat capacity of calorimeter x temperature change

so

Q = C x dT

Q = C x ( Tf - Ti)

given

C = 4.728

Tf = 27.19

Ti = 23.28

using these values

we get

Q = 4.728 x ( 27.19 - 23.28)

Q = 18.48648 KJ

now

given 1.183 g of xylose

so

heat per gram = heat / mass

heat per gram of xylose = 18.48648 / 1.183

heat per gram of xylose = 15.2678

now

heat per mole of xylose = heat per g x molar mass

we know that

molar mass of xylose = 150 g/mol

so

heat per mole = 15.2678 x 150

heat per mole of xylose = 2344

so

heat of combustion of xylose is 2344 KJ /mol

B)

the reaction is

C5H10O5 + 5O2 ---> 5H2O + 5CO2

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