burning methane?

Question

CH4+O2 -----> CO2+H2O

what are the multiples of this reaction?
and how many kilos of methane do you need to release 890MJ of energy, when the burningtemp. of methane is 890kJ/mol?

Please help me with this, I've tried SO many times, and just seem to get stuck over and over again. Big hug for the one that solves this.

Answer 1

CH4 + 2O2 --> CO2 + 2H2O

I did factor labeling.
890 MJ (1 KJ/ .001 MJ) (1 mol CH4/ 890 KJ) (.016 kg CH4 / 1 mol CH4) = 16 kg CH4

explanation:
890 MJ is given
conversion btw kilojules to megajules
1 mol of methane over 890 KJ is given
molar mass, but instead of in grams, i converted to kgs
C = 12 molar mass
H = 1 molar mass (times 4 b/c there are 4 hydrogens)
then multiply all of that together and it's 16 kgs of methane
could someone verify this?

Answer 2

CH4 + 2O2 ===> CO2 + 2H2O (Is that what you mean?)

890MJ x 1000kJ/1MJ x 1molCH4/890kJ x 16gCH4/1molCH4 x 1kgCH4/1000gCH4 = (890)(1000)(16)/(890)(1000) = 16kgCH4

When you set it up this way, you see right off that all kinds of stuff cancels.