A 1.9862-g sample of benzoic acid burns in an excess of oxygen, in a bomb calorimeter. The temperature of the calorimeter rises from 24.94 C to 28.77 C. The calorimeter contains 2000.0 g of H2O, and the heat capacity of the calorimeter (excluding the water, but including the bomb, thermometer, and all mechanical parts) has the value C(cal) = 5.35 kJ/C. Use the given information to find the molar heat of combustion of benzoic acid (M(benzoic acid) = 122.1 g/mol).
2C6H5COOH(l) + 15O2(g) ----> 12CO2(g) + 6H2O(l)
no of mol of benzoicacid = w/mwt = 1.9862/122.1 = 0.163 mol
heat released(q) = mwater*swater*DT + Ccal*DT
= 2000*4.184*(28.77-24.94) + 5.35*10^3*(28.77-24.94)
= 52.54 kjoule
DH0com = -q/n = -52.54/0.163 = -322.33 kj/mol
A 1.9862-g sample of benzoic acid burns in an excess of oxygen, in a bomb calorimeter. The temperature of the calorimet...
7. A 2.529-g sample of glutaric acid, CsH.O.(132.12 g/mol) was burned in a bomb calorimeter with excess oxygen. The temperature of the calorimeter and the water before combustion was 23.63 °Cafter combustion the calorimeter and the water had a temperature of 32.48 °C. The calorimeter had a heat capacity of 747 J/K, and contained 0.926 kg of water. Use these data to calculate the molar heat of combustion (in kJ) of glutaric acid.
When a 0.245-g sample of benzoic acid is combusted in a bomb calorimeter, the temperature rises 1.644 ∘C . When a 0.275-g sample of caffeine, C8H10O2N4, is burned, the temperature rises 1.520 ∘C . Using the value 26.38 kJ/g for the heat of combustion of benzoic acid, calculate the heat of combustion per mole of caffeine at constant volume.
When a 0.235-g sample of benzoic acid is combusted in a bomb calorimeter, the temperature rises 1.643 ∘C . When a 0.270-g sample of caffeine, C8H10O2N4, is burned, the temperature rises 1.555 ∘C . Using the value 26.38 kJ/g for the heat of combustion of benzoic acid, calculate the heat of combustion per mole of caffeine at constant volume.
When a 0.225-g sample of benzoic acid is combusted in a bomb calorimeter, the temperature rises 1.643 ∘C . When a 0.265-g sample of caffeine, C8H10O2N4, is burned, the temperature rises 1.594 ∘C . Using the value 26.38 kJ/g for the heat of combustion of benzoic acid, calculate the heat of combustion per mole of caffeine at constant volume.
Thermometer Ignition wires heat sample Stirrer 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. Water In the laboratory a student burns a 1.22-g sample of fumaric acid (C4H10) in a bomb calorimeter containing 1040. g...
A 1.764-g sample of heptanoic acid, C7H14O2 (130.19 g/mol) was burned in a bomb calorimeter with excess oxygen. The temperature of the calorimeter and the water before combustion was 23.68 °C; after combustion the calorimeter and the water had a temperature of 32.12 °C. The calorimeter had a heat capacity of 500 J/K, and contained 1.462 kg of water. Use these data to calculate the molar heat of combustion (in kJ) of heptanoic acid.
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy sontent of foods. lastered 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 0.500-g sample of benzoic acid (C H02) in a bomb calorimeter containing 1030. g of water. The temperature increases...
2) 1.9 g of an unknown hydrocarbon (44 g/mol) burns in bomb calorimeter in excess oxygen. The heat capacity of the calorimeter, Cv, = 5.539 kJ/°C and AT =15.874 ºC. Find AE for this hydrocarbon in kJ/mol. (Hint: This is a bomb calorimeter, where the reaction is happening at constant volume: So, what is zero? How is AE related to q (heat)?) Identify: system = Surrounding =
Ignition wires heat sample Thermometer Stirrer 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 0.319-g sample of phenanthrene (C14H10 in a bomb calorimeter containing 1070. g of water....
Thermometer 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. Ignition wires heat sample Stirrer 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. Water In the laboratory a student burns a 0.568-g sample of tridecanedioic acid (C13H2404) in a bomb calorimeter containing 1080. g...