Question

I feel like this question is pretty easy, but I can't seem to figure out how to go about solving it. It's like the solution is on the tip of my tongue:

Nitromethane (CH3NO2) burns in air to produce significan amounts of heat.

2 CH3NO2(l) + 3/2 O2(g) -> 2 CO2(g) + 3 H2O(l) + N2(g)
ΔHo rxn = -1418kJ

How much heat is produced by the complete reaction of 6.90kg of nitromethane?

Answer 1

So you get 1418 kJ for every 2*61 g nitromethane. How much will you get for 6900 g.
1418 kJ x (6900/2*61) = ?

Answer 2

Just as I thought, it was much easier than I was making it out to be haha

Thank you!