A bomb calorimeter was calibrated by burning 1.031 g of benzoic acid (C6H5COOH, M = 122.13g/mol) in excess oxygen. The temperature inside the calorimeter rose from 23.2°C to 36.7°C.
a. What is the heat capacity of the bomb calorimeter, in units of kJ/°C? ÎrU = -3230 kJ/(1 mol benzoic acid)
b. Nitromethane, (CH3NO2 M = 61.04 g/mol), commonly known as ânitroâ, is the fuel used in racing cars. Write the formation reaction for liquid nitromethane.
c. A sample of nitromethane was burned in the bomb calorimeter calibrated above. The following energy value was determined for the balanced reaction:
4CH3NO2(l) + 3 O2(g) â 4 CO2(g) + 6 H2O(l) + 2 N2(g) ÎrU= -3740 kJ/mol
Calculate ÎHf for nitromethane, in units of kJ/mol.
⢠Assume that ÎrH= ÎrU within the accuracy of this experiment.
â¢ÎfH°(gaseous CO2) = - 393.52 kJ/mol ÎfH°(liquid H2O) = - 285.83 kJ/mol.
d. It is assumed above that ÎrH= ÎrU for the combustion of nitromethane.
⢠Estimate how much work is done, in units of kJ/mol, for the combustion reaction as written in part c at 298 K.
â¢Is work done by the system, the surroundings, or neither?
â¢Justify whether the assumption is a valid one.
A bomb calorimeter was calibrated by burning 1.031 g of benzoic acid (C6H5COOH, M = 122.13g/mol) in excess oxygen. The temperature inside the calorimeter rose from 23.2°C to 36.7°C.
a. What is the heat capacity of the bomb calorimeter, in units of kJ/°C? ÎrU = -3230 kJ/(1 mol benzoic acid)
b. Nitromethane, (CH3NO2 M = 61.04 g/mol), commonly known as ânitroâ, is the fuel used in racing cars. Write the formation reaction for liquid nitromethane.
c. A sample of nitromethane was burned in the bomb calorimeter calibrated above. The following energy value was determined for the balanced reaction:
4CH3NO2(l) + 3 O2(g) â 4 CO2(g) + 6 H2O(l) + 2 N2(g) ÎrU= -3740 kJ/mol
Calculate ÎHf for nitromethane, in units of kJ/mol.
⢠Assume that ÎrH= ÎrU within the accuracy of this experiment.
â¢ÎfH°(gaseous CO2) = - 393.52 kJ/mol ÎfH°(liquid H2O) = - 285.83 kJ/mol.
d. It is assumed above that ÎrH= ÎrU for the combustion of nitromethane.
⢠Estimate how much work is done, in units of kJ/mol, for the combustion reaction as written in part c at 298 K.
â¢Is work done by the system, the surroundings, or neither?
â¢Justify whether the assumption is a valid one.