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18 Dec 2019

A 0.407-g sample of benzil (C14H10O2) is burned in a bomb calorimeter and the temperature increases from 24.50 °C to 27.25 °C. The calorimeter contains 1000 g of water and the bomb has a heat capacity of 831 J/°C. The heat capacity of water is 4.184 J g-1°C-1. Based on this experiment, calculate ΔE for the combustion reaction per mole of benzil burned.

___ kJ/mol

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Irving Heathcote
Irving HeathcoteLv2
31 Dec 2019

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Related questions

A)A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.
Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter.
In the laboratory a student burns a 0.392-g sample of bisphenol A (C15H16O2) in a bomb calorimeter containing 1140. g of water. The temperature increases from 25.00 °C to 27.40 °C. The heat capacity of water is 4.184 J g-1°C-1.
The molar heat of combustion is −7821 kJ per mole of bisphenol A.

C15H16O2(s) + 18 O2(g) ------>15 CO2(g) + 8 H2O(l) + Energy

Calculate the heat capacity of the calorimeter.
heat capacity of calorimeter =_________ J/°C

B)

A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.

In an experiment, a 0.5574 g sample of benzil (C14H10O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.379×103 g of water. During the combustion the temperature increases from 26.36 to 28.99 °C. The heat capacity of water is 4.184 J g-1°C-1.
The heat capacity of the calorimeter was determined in a previous experiment to be 847.1 J/°C.
Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of benzil based on these data.
C14H10O2(s) + (31/2) O2(g) ------->5 H2O(l) + 14 CO2(g) + Energy
Molar Heat of Combustion = _________ kJ/mol



C)

A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.

In an experiment, a 0.9900 g sample of β-D-fructose (C6H12O6) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.292×103 g of water. During the combustion the temperature increases from 21.82 to 24.12 °C. The heat capacity of water is 4.184 J g-1°C-1.
The heat capacity of the calorimeter was determined in a previous experiment to be 991.1 J/°C.
Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of β-D-fructose based on these data.
C6H12O6(s) + 6O2(g) -------> 6 H2O(l) + 6 CO2(g) + Energy
Molar Heat of Combustion = ____________ kJ/mol


All three problems are a set for one question on my homework, so please answer all three. Thank you so much!

A 1.09-g sample of dimethyl oxalate (C4H6O4) is burned in a bomb calorimeter and the temperature increases from 25.10 °C to 28.14 °C. The calorimeter contains 1.09×103 g of water and the bomb has a heat capacity of 777 J/°C. The heat capacity of water is 4.184 J g-1°C-1. Based on this experiment, calculate ΔE for the combustion reaction per mole of dimethyl oxalate burned.

A 0.312-g sample of phenanthrene (C14H10) is burned in a bomb calorimeter and the temperature increases from 24.30 °C to 26.61 °C. The calorimeter contains 1.07×103 g of water and the bomb has a heat capacity of 919 J/°C. The heat capacity of water is 4.184 J g-1°C-1. Based on this experiment, calculate ΔE for the combustion reaction per mole of phenanthrene burned.

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