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13 Dec 2019

Top fuel dragsters and funny cars burn nitromethane as fuel according to the following balanced combustion equation:
2CH3NO2(l)+3/2O2(g)→2CO2(g)+3H2O(g)+N2(g)
The standard enthalpy of combustion for nitromethane is −709.2kJ/mol.

Calculate the standard enthalpy of formation (ΔH∘f) for nitromethane.

Express your answer using four significant figures.

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Reid Wolff
Reid WolffLv2
17 Dec 2019

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Related questions

1. Nitromethane (CH3NO2)burns in air to produce significant amounts of heat.
2CH3NO2(l)+3/2O2(g)?2CO2(g)+3H2O(l)+N2(g)
?Horxn = -1418kJ

How much heat is produced by the completereaction of 3.09kg ofnitromethane?
Express your answer to threesignificant figures and include the appropriate units.


2. Use the standard reaction enthalpies given below to determine?H

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.

Benzene (C6H6) burns according to the following balanced equation: C6H6(l)+152O2(g)?6CO2(g)+3H2O(g)

Calculate ?H?rxn for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of liquid benzene is 49.1 kJ/mol.)

express answer using five significant figures.

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