[vlaplayer]

I am doing a worksheet and I am very stuck. Here is my problem:

Calculate the amount of heat produced when 52.4g of methane,CH₄, burns in an excess of air, according to the folowing equation:
            CH₄ +2O₂yields CO₂+2H₂O
           delta H=-890.2kJ

[vanklik]

I am doing a worksheet and I am very stuck. Here is my problem:

Calculate the amount of heat produced when 52.4g of methane,CH₄, burns in an excess of air, according to the folowing equation:
            CH₄ +2O₂yields CO₂+2H₂O
           delta H=-890.2kJ

I would do it in this way (I'm not sure it's correct though)
m(CH₄) = 52.4 g
Mr(CH₄) = 16
delta H=-890.2kJ
q=n*delta H  n=m/Mr = 52.4/16 = 3.275 mole
q= 3.275 * 890.2 = 2915.405 kJ
I hope this helps

P.S. I'm just learning, so there is a big possibility of mistake.

[matt1234]

1) Get a balanced equation
2) Use standard enthalpies of formation
3) delta h reaction = (sum of formation of products) - (sum of formation of reactants)

Note: enthaplies of formation for elements are 0


3) once you know delta H for the reaction find # moles methane and setup a ratio with delta h from the reaction and moles in the reaction.