In a bomb calorimeter compartment surrounded by 945 g of water,the combustion of 1.048 g of benzene, C6H6( ), raised thetemperature of the water from 23.640degreeC to 32.692degreeC. Theheat capacity of the calorimeter is 891 J/degreeC. (a) Write thebalanced equation for the combustion reaction, assuming that C02(g)and H20( ) are the only products, (b) Use the calorimetric data tocalculate dalta E for the combustion of benzene in kj/g and inkj/mo

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Elin HesselLv2

10 Oct 2019

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In a bomb calorimeter compartment surrounded by 1.305 kg of water, the combustion of 1.148 g of benzene, C6H6 (l), raised the temperature of the water from 23.640Â°C to 32.692Â°C. The heat capacity of the calorimeter is 0.864 kJ/Â°C. What is âE for the reaction in kJ/mol of C6H6 (l), the specific heat of water is 4.184 J/gÂ°C. Enter the correct sign (+ or -).

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 0.3833 g sample of phenanthrene (C14H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.284Ã103 g of water. During the combustion the temperature increases from 22.04 to 24.54 Â°C. The heat capacity of water is 4.184 J g-1Â°C-1. The heat capacity of the calorimeter was determined in a previous experiment to be 909.2 J/Â°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of phenanthrene based on these data. C14H10(s) + (33/2) O2(g) 5 H2O(l) + 14 CO2(g) + Energy

Solve for Molar Heat of Combustion = kJ/mol

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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 Â°C to 27.40 Â°C. The heat capacity of water is 4.184 J g^-1Â°C^-1.
The molar heat of combustion is â7821 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/Â°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 0.5574 g sample of benzil (C₁₄H₁₀O₂) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.379Ã10³ g of water. During the combustion the temperature increases from 26.36 to 28.99 Â°C. The heat capacity of water is 4.184 J g^-1Â°C^-1.
The heat capacity of the calorimeter was determined in a previous experiment to be 847.1 J/Â°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.