The combustion of 1.793 g of fructose, C,H,0,(s), in a bomb calorimeter with a heat capacity of 5.30 kJ/°C results in an increase in the temperature of the calorimeter and its contents from 22.25 °C to 27.53 °C. What is the internal energy change, AU, for the combustion of 1.793 g of fructose? AU = kJ Calculate the enthalpy of combustion, AHc, of fructose in kilojoules per mole. ΔΗ, kJ/mol

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What is the internal energy change, Δ?Δ⁢U, for the combustion of 1.7931.793 g of fructose?

Calculate the enthalpy of combustion, Δ?cΔ⁢Hc, of fructose in kilojoules per mole.

The combustion of 1.793 g of fructose, C,H,,0, (s), in a bomb calorimeter with a heat capacity of 5.30 kJ/°C results in an
increase in the temperature of the calorimeter and its contents from 22.25 °C to 27.53 °C. What is the internal energy change,
AU, for the combustion of 1.793 g of fructose?
AU =
kJ
Calculate the enthalpy of combustion, AHc, of fructose in kilojoules per mole.
ΔΗ, -
kJ/mol
Transcribed Image Text:The combustion of 1.793 g of fructose, C,H,,0, (s), in a bomb calorimeter with a heat capacity of 5.30 kJ/°C results in an increase in the temperature of the calorimeter and its contents from 22.25 °C to 27.53 °C. What is the internal energy change, AU, for the combustion of 1.793 g of fructose? AU = kJ Calculate the enthalpy of combustion, AHc, of fructose in kilojoules per mole. ΔΗ, - kJ/mol
Expert Solution
Step 1

Given,

mass of fructose =1.793 g

heat capacity = 5.30kJ°C

Initial  temperature = 22.25°C

Final temperature = 27.53 °C

Change in temperature =(27.53-22.25)°C=5.28°C

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