A question on acrylonitrile and partial pressures?

Question

An important process for the production of acrylonitrile C3H3N is given by the following reaction
2C3H6 + 2NH3 + 3O2 --> 2C3H3N + 6H2O
A 150 -L reactor is charged tot he following partial pressures at 25 C
P(C3H6) = .5 MPa
P(NH2) = .8 MPa
P(O2) = 1.5 MPa
What mass of acrylonitrile can be produced from this mixture (MPa = 10^6 Pa)?

How should i go about to complete this problem?
I'm thinking about converting all the reactants into moles and than using the one that gets used up first, see how much moles of acrylonitrile are forms and change that into grams for the answer.

Answer 1

you must examine your equation. You see that for 2 moles C3H6, you need 2 moles NH3 and 3 moles Of O2

The number of mole of each gas is prortional to its partial pressure.

You see that P(C3H6) is the lower and notice also that for 2moles of that product , you need moles of O2. So for 0.5moles, 0.75 molesO2

You see also that the number of moles of C3H3N is the same as C3H6.

So the pressure of C3H3N OBTAINED will also be 0.5 MPa

we will calculate the number of moles of that product

pV = nRT T= 273+25= 298 ;R= 8.31MKSa; V =150L =0.15m^3

n = pV/RT

n=0.5*10^6*0.15/(8.31*298)=30.3 moles

and as one mole= 53g you obtain= 1605g = 1.605 kg

Answer 2

Acrylonitrile Production Process