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Nitromethane, CH3NO2, can be used as a fuel. When the liquid is burned, the (unbalanced) reaction is mainly

 

A. The standard enthalpy change of reaction (  ) for the balanced reaction  (with lowest whole-number coefficients) is -1288.5 kJ. What is the for nitromethane?

B. A 15.0-L flask containing a sample of nitromethane is filled with O2 and the flask is heated to 100oC. At this temperature, and after the reaction is complete, the total pressure of all the gases inside the flask is 950 torr. If the mole fraction of nitrogen (Xnitrogen) is 0.134 after the reaction is complete, what mass of nitrogen was produced?

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Christian Garcia
Christian GarciaLv10
5 Nov 2020

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Related questions

Nitromethane, CH3NO2, can be used as a fuel. When the liquid is burned, the (unbalanced) reaction is mainly
 
 
 
a. The standard enthalpy change of reaction (Δrxn) for the balanced reaction (with lowest whole-number coefficients) is -1288.5 kJ. Calculate Δfo for nitromethane.
 
b. A 15.0-L flask containing a sample of nitromethane is filled with O2 and the flask is heated to 100.ºC. At this temperature, and after the reaction is complete, the total pressure of all the gases inside the flask is 950. torr. If the mole fraction of nitrogen (χnitrogen) is 0.134 after the reaction is complete, what mass of nitrogen was produced?
 

Please show work and all parts. Thanks!

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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