Question

........

Answer 1

So we have to make 2 equations?

Answer 2

yes i think we have to make to separate equation

Answer 3

Because methane burns in oxygen, not in water.

Answer 4

but i don't know how to do this problem

Answer 5

I think there's some mistake in the question.

Answer 6

well maybe, but this is a homework question and its in the book

Answer 7

sorry

Answer 8

Oh. lol. My bad then.

Answer 9

oh don't worry

Answer 10

so you don't know how to do it?

Answer 11

Sorry no.

Answer 12

And we can find amount of heat by bond energies or by Q=mcT.

Answer 13

This is the hint given when i enter the answer, determine the heats of combustion for both methane and water gas, where the gas can be treated as the sum of the heats of combustion of water and CO individually. For the water gas, two moles total of product are made, so the sum of the heats of combustion must be manipulated to give a value for one mole.

Answer 14

Wait! Have they given you values for the formation of CO2 and H2O?
Or values for combustion for C or H?

Answer 15

noo, they didn't gave me any values

Answer 16

Then how on the Earth they want us to solve this? D:

Answer 17

yeah i know, this question are not clear

Answer 18

Hmmm. :/

Answer 19

Hydrocarbon + O2 => H2O + CO2
heat

Answer 20

ok, the heat of combustion for hydrogen is -285.8 KJ/mol

Answer 21

Meaning, the formation of H2O is that..

Answer 22

Unfortunately, i have to leave. I'll see this problem tomow if you have time.

Answer 23

yes

Answer 24

Oh man. :/
Sorry. If you get a chance, post it's solution here.
-Cheers.

Answer 25

hmm i don't know if i would be able to get the solution :/

Answer 26

Alright then. No prob. :)