Another long Chem Question?

Question

Hydrogen cyanide is produced industrially from the reaction of gaseuous ammonia, oxygen and methane: 2NH3(g) + 3O2(g) +2CH4(g) --> 2HCN(g) +6H2O(g)
if 5,000 kg each of NH3, O2, and CH4 are reacted, what mass of HCN and of H2O will be poduced (assuming 100% yield)

Answer 1

Atomic weights: N = 14 H = 1 O = 16 C = 12 NH3 = 17 O2 = 32 CH4 = 16 HCN = 27 H2O = 18

First find the limiting reactant. Let kmol be kilogram molecular weight

5000kgNH3 x 1kmolNH3/17kgNH3 = 294kmolNH3
5000kgO2 x 1kmolO2/32kgO2 = 156kmolO2
5000kgCH4 x 1kmolCH4/16kgCH4 = 312kmolCH4

O2 is the limiting reactant, because 156kmol O2 would require 2/3 x 104kmol each of NH3 and CH4 according to the balanced equation. There are a lot more than 104 kmols of the other two reactants. So O2 will get used up first,

156kmolO2 x 2kmolHCN/3kmolO2 x 27kgHCN/1kmolHCN = (156)(2)(27)/(3) = 2808kgHCN

156kmolO2 x 6kmolH2O/3kmolO2 x 18kgH2O/1kmolH2O = (156)(6)(18)/((3) = 5616kgH2O

Answer 2

What grade are you in?

Are you in college?

What course are you in, plz tell me so i know what class NOT to get into ...lol