The combustion of the fuel gas butane is given by:
2(C4H10) +13(O2) --> 8(CO2) + 10(H2O) del(H)= –5760kJ/mol
What mass of butane would be needed to produce 33440J of energy?
The Attempt at a Solution
First of all how do you interpret del(H)= –5760kJ/mol
Per mol of what?
I assume a mol is the complete reaction of
[2(C4H10) +13(O2) --> 8(CO2) + 10(H2O)]
33440J/(5760kJ/mol)=0.0058mol of the reaction
So a total of 0.0058*2=0.0116 moles of butane?
Which would be 0.012*(12.01*4 + 10.1)=0.675g of butane but the answers suggested 0.337g which is a half of what I worked out. Hence they didn’t multiply by 2. This confusion comes back to my first question. ‘Per mol of what?’ In del(H)= –5760kJ/mol