chemistry help

Can someone please explain to me how to do the following question?

5N2O4(l) + 4CH3NHNH2(l) → 4CO2(g) + 12H2O(l) + 9N2(g) ∆H = −5116 kJ
The energy released when 2 moles of each reactant are mixed and ignited is
A 2046 kJ
B 2558 kJ
C 4093 kJ
D 5116kJ.

there are 2 moles of each reactant, still reacting in a 5:4 ratio
5( N2O4) : 4 ( CH3NHNH2 )
so multiply both sides by 2/5, to get the ratio as 2( N2O4) : 8/5 ( CH3NHNH2 )
this means that when 2 moles of each reactant are mixed, all the N2O4 reacts, but 2/5 moles of the CH3NHNH2 are left unreacted

put this value into ∆H= −q/n

so q= 5116*2/5
which is 2046