a 0.2 gram sample of a candy bar is combusted in a bomb calorimeter, increasing the temperature of the 2000 g of water from 25.00◦c to 25.47◦c. what is ∆u in kj/g? ignore any heat loss or gain by the calorimeter itself.

The HHV of a biomass fuel is calculated using a bomb calorimeter, which measures the heat released during the combustion of a specific amount of biomass sample. Following each test, a small amount of sample fuel is ground and diluted so that it will fit inside a capsule and be used in a bomb.

Mass of Candy = 0.2g

Mass of water = 2000 g

specific heat of water = 4.184 5g⁻¹°c⁻¹

Initial temperature = 25.00°C

final temperature = 25.47°C

Change in temperature = final- Initial

Change in temperature = 25.47-25.00

ΔT = 0.47°C

specific heat of calorimeter = 700J/k

Thus, Heat produced by the combustion of candy is absorbed by water and calorimeter.

Hence,

ΔU = Heat absorbed by water + Heat absorbed by calorimeter

ΔU = mass × specific heat × ΔT + specific heat × ΔT

ΔU = 2000 × 4.184 × 0.79 + 700 × 0.79

ΔU = 6.604 kJ + 0.532kJ

ΔU = 7.136kJ.

Thus, 0.2g of candy produced heat = 7.136kJ

1g of candy produced heat = 7.136/0.2 = 35.68kJ/g

Thus ΔU for candy = 35.68kJ/g.

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