Question

An equimolar mixture of nitrogen and acetylene enters a steady-flow reactor at 25℃ and 1.0 bar. The reaction taking place in the reactor is N2(g) + C2H2(g) = 2 HCN(g). The product leaves the reactor at 600℃ and 1 bar and contains 24.2% of HCN by mole. Assuming that the gas mix in the reactor is an ideal gas with Cp = 43.1 J/mol-K and that no heat loss occurred, how much heat is supplied to the reactor for each mole of N2 input?

Answer 1

N2(g) + C2H2(g) = 2 HCN(g)

initial 1 mol 1 mol 0

when HCN leaves1-x 1-x 2x 2x/2=0.242 ; x=0.242 mol ; total number of mole = 2.

Molar heat capacity of the gas mixture = Cp = 43.1 J/mol-K

Heat supplied to the reactor = Heat of the reaction + heat required to raise the temperature of the system.

heat required to raise the temperature of the system= n*Cp*(600-25)=2*43.1*575=49.565 KJ

Heat supplied to the reactor = Heat of the reaction+49.565 KJ; heat of reaction is not provided.

if you have that data, just add it to above equation.