Question

Nitromethane (ch3no2) burns in air to produce significant amounts of heat. 2 ch3no2(l) + 3 2 o2( g) ¡ 2 co2( g) + 3 h2o(l) + n2( g) δh° rxn= -1418 kj how much heat is produced by the complete reaction of 5.56 kg of nitromethane

Answer 1

6.46 x 10^4 kJ

Step-by-step explanation:

Calculate moles of CH3NO2:

kg to g:

5.56 kg x 1000 = 5560 g

molar mass of CH3NO2:

12.01 + 3.024 + 14.01 + 32.00 = 61.04 g

moles= mass / molar mass

moles = 5560 g / 61.04 g/ mol

moles = 91.1

Then calculate total heat

Total heat = (delta H / 2 mol) x moles of CH3NO2

Plug into calculator just like this

Total heat = (-1418/2) x 91.1

Total heat = 64589.9 kJ

move the decimal over 4 places:

6.46 x 10^4 kJ is the result