Use enthalpy of formation data to calculate the number of moles of CO2 (g) produced per mega joule of heat released from the combustion of each fuel under standard conditions.
a) Coal c (s, graphite)
b) Natural gas, CH4 (g)
c) propane, C3H8 (g)
d) Octane, C8H18 (l) delta H f = -250 kJ Mol -1
Second calculate the energy released (delta Hf).
Third divide 1MJ = 1000kJ by the energy released in step 2 to obtain the number of complete reactions needed to release 1MJ.
Fourth, multiply by the coefficient of CO2, to get the moles of CO2 produced in total for all the reactions in step 3.
Batman very much so has the correct answers.
Then find the energy released for both the products and the reactants. Since Octane was given to us in the question, I’ll use that as an example for the equation:
[2C8H18(-250.1)+25O2(0)]-[16CO2(-393.5)+18H2O(-285.8)] = 10940.2 KJ
(assuming reaction is under standard conditions of 1 atm, and about 25 deg C.)
Now take the coefficient of CO2 that was formed in the product and divide it by the number of J found.
(16/10940.2) = 1.46*10^-3
Then multiply it by 1000 KJ to get it into MJ.
(1.46*10^-3)1000 = 1.46 mol/MJ
a. 2.54 mol/MJ
b. 1.25 mol/MJ
c. 1.47 mol/MJ
d. 1.58 mol/MJ
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