Question

Nitromethane (CH3NO2) burns in air to produce significant amounts of heat.
2CH3NO2(l)+3/2O2(g)→2CO2(g)+3H2O(l)+N2(g)
ΔHorxn = -1418 kJ
How much heat is produced by the complete reaction of 5.85 kg of nitromethane?

Answer 1

@V1r3z try this haha

Answer 2

@nmagnuson

Answer 3

I believe this is how you complete this: since this shows the change in enthalpy in the combustion of 2 moles of nitromethane, we need to halve that value to find the change in enthalpy per mole of nitromethane first. This gives us -709 kJ. Next find out how many moles of nitromethane equates to 5.85 kg of nitromethane by multiplying 5.85 by 1000 to get 5850 g of nitromethane, and then do \[5850 g Nitro. *\frac{ 1 mol Nitro. }{ 61.01 g Nitro } = 95.84 moles of Nitromethane\] Finally, multiply 95.84 moles of nitromethane by mass with -709 kJ (709000J) of heat to get 67950560 J or 67950 kJ of heat, or 6.79*10^4 kJ of heat (with significant figures). I'm not 100% positive that this is right, but if I remember correctly this is how you do it.

Answer 4

it was right c: Thank you!

Answer 5

Glad I could help :)