Posted by Harold on Thursday, January 27, 2011 at 10:54am.
I have no clue
someone should answer this question please
a) 2.54
b) 1.12
c) 1.35
d) 1.46
Batman is correct.
Batman is indeed correct.
First write out the combustion reaction.
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.
batman saved me
typical batman. saving the day, as per usual.
Spiderman saved the day too by explaining how to do it!
TANK U BATMAN
thanks guys for the great help
BATMAN, you haved failed to explain yourself yet again! But thanks spider man, you're a much cooler hero... obviously...
Batman,... fuuck you for making me get the INCORRECT answer~ u TROLL!
Thank you Batman. I am forever in your debt. And thanks my friendly neighborhood Spiderman for helping me understand!
My teacher didn't do a good job explaining, help please!
Can someone write out the combustion reaction?
Okay, First write out all of the balanced equations of combustion(A combustion equation is just adding O2 to the reactant, and ending with CO2 in the products. Notice, if H is in the reactants, you'll need H2O to balance the products:
Coal:
C+O2-->CO2
Natural Gas:
CH4+2O2-->CO2+2H2O
Propane:
C3H8+5O2-->3CO2+4H2O
Octane:
2C8H18+25O2-->16CO2+18H2O
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