Calculate the delta H rxn of the following reaction? Need to figure this out by tonight please!

I don't even know where to start with this question. Somebody help please? If you can help with either one that'd be great. Thanks in advance!

2. Calculate DeltaHrxn for the following reaction:

CH4(g) + 4Cl2 (g) --- CCl4(g) + 4HCl(g)

Use the following reactions and given delta H's:

C(s) + 2H2 (g) --- Ch4 (g) Delta H = -74.6 kj
C(s) + 2Cl2 (g) --- CCl4 (g) Delta H = -95.7 kj
H2(g) + Cl2 (g) --- 2HCl (g) Delta H = -184.6 kj

You can use Hess' law to solve this problem.

Basically, you use these three equations to create one equation that matches the one you need to solve.

In this case, you reverse equation 1, you keep equation 2 the same, and you multiply equation 3 by 2. This gives you:

CH4(g) --> C(s) + 2H2(g) H = 76.6 kJ (change the sign of H when you reverse the rxn)
C(s) + 2Cl2(g) --> CCl4(g) H = -95.7kJ
2H2(g) + 2Cl2(g) --> 4HCl(g) H = 2(-184.6) kJ (multiply the whole thing by 2, including H)

Add them together and this gives you:

CH4(g) + C(s) + 2Cl2(g) + 2H2(g) + 2Cl2(g) --> C(s) + 2H2(g) + CCl4(g) + 4HCl(g)

Remove duplicate species from each side:

CH4(g) + 4Cl2(g) --> CCl4(g) + 4HCl(g)

Which is your original equation. Now just add up the delta H's as they are now arranged:

76.6 kJ + (-95.7) kJ + 2(-184.6) kJ = -388.3 kJ

To 3 significant figures, the answer is -388 kJ

I got -390.3 kJ by doing what the other person above me did...and in sig figs. that would be -390. kJ Make sure that the answer is asking for kJ and not Joules.
By the way, is this a problem on quest?