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Calculate the mass of octane, C8H18(l), that must be burned in air to evolve the same quantity of energy as produced by the fusion of 1.0 g of hydrogen in the following fusion reaction:

4 + 2

Assume that all the products of the combustion of octane are in their gas phases. Use data from Exercise 21.50, Appendix C, and the inside covers of the text. The standard enthalpy of formation of octane is –250.1 kJ/mol.

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Casey Durgan
Casey DurganLv2
22 May 2020

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Related questions

2H2(g)+O2(g)=@H2O(l)

Calculate the volume of hydrogen gas at 25 celcius and 1.00atm required to produce an amount of energy equivalent to that produced by the combustion of a gallon of octane (C8H18). The density of octane is 2.66kg/gal, and its standard enthalpy of formation is -249.9kJ/mol.

Many power plants produce energy by burning carbon-based fuels, which also produces carbon dioxide. Carbon dioxide is a greenhouse gas, so over-production can have negative effects on the environment. Use enthalpy of formation data to calculate the number of moles of CO2(g) produced per megajoule of heat released from the combustion of each fuel under standard conditions (1 atm and 25 °C).

(a) coal, C(s, graphite);

(b) natural gas, CH4(g);

(c) propane, C3H8(g);

(d) octane, C8H18(l) (ΔHf° = –250.1 kJ ·mol–1)

UNITS: mol * MJ^-1

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