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An oxygen bomb calorimeter was calibrated using a 0.325 g of benzoic acid (delta Uc = -6316 cal/g), which gave a temperature rise of 1.48 degrees C. What is the calorimeter constant? A 0.69 g sample of gasoline was oxidized in the calorimeter, resulting in a temperature change of 4.89 degrees C. What is delta Uc for 1.0g of gasoline? Please show steps

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Casey Durgan
Casey DurganLv2
17 Dec 2019

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Related questions

Physical Chemistry Thermodynamics:

The enthalpy of combustion of benzoic acid (C6H5COOH) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be —3226.7 kJ mol-1, (a) When 0.9862 g of benzoic acid was oxidized, the temperature rose from 21.84°C to 25.67°C. What is the heat capacity of the calorimeter? (b) In a separate experiment, 0.4654 g of glucose (C6H1206) was oxidized in the same calorimeter, and the temperature rose from 21.22°C to 22.28°C. Calculate the enthalpy of combustion of glucose, the value of delta r U for the combustion, and the molar enthalpy of formation of glucose.

need help doing PART 2 please



this was giving by professor to help


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? ΔrU = -3230 kJ/(1 mol benzoic acid)

b. Nitromethane, (CH3NO2 M = 61.04 g/mol), commonly known as “nitro”, 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) → 4 CO2(g) + 6 H2O(l) + 2 N2(g) ΔrU= -3740 kJ/mol

Calculate ΔHf for nitromethane, in units of kJ/mol.

• Assume that ΔrH= ΔrU within the accuracy of this experiment.

•ΔfH°(gaseous CO2) = - 393.52 kJ/mol ΔfH°(liquid H2O) = - 285.83 kJ/mol.

d. It is assumed above that ΔrH= ΔrU 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.

•Is work done by the system, the surroundings, or neither?

•Justify whether the assumption is a valid one.

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