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

From the balanced reaction, we are given that 1418 kJ of heat is released for every 2 moles of nitromethane (CH3NO2) reacted.

So first calculate the moles of CH3NO2:

moles CH3NO2 = 5560 g / (61.04 g/mol)

moles CH3NO2 = 91.1 mol

 

So total heat released is:

total heat = (-1418 kJ / 2mol) * 91.1 mol

total heat = -129,162.52 kJ = -129.16 MJ

Answer 2

Answer:

6.46 x 10^4 kJ

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