(a) What volume of NH3(g) can be produced from 257 L of H2(g) if the gases are measured at 315°C and 5.01 atm?

Question

The Haber process is the principal method for fixing nitrogen (converting N2 to nitrogen compounds).
N2(g) + 3 H2(g) 2 NH3(g)

Assume that the reactant gases are completely converted to NH3(g) and that the gases behave ideally.

(a) What volume of NH3(g) can be produced from 257 L of H2(g) if the gases are measured at 315°C and 5.01 atm?

(b) What volume of NH3(g), measured at 25°C and 727 mmHg, can be produced from 257 L H2(g), measured at 315°C and 5.01 atm?

i found the b part to be
455 L

is that correct?

Answer 1

a) you see from the equation that 3moles of H2 correspond to 2 moles of NH3. As the content in moles is proportional to that of volumes , you have two volumes of NH3 for three of NH3
so 257L of H2 give 2*257/3 =171.3L of NH3

b) you use pV=nrT so V=nRT/p

in conditions1 V1=nRT1/P1 cond 2 V2=nRT2/P2

cond1 T1 =25+273=298 P1= 727mmHg
cond2 T2= 315+273=588 P2=5.01*760=3876mmHg

V1/V2=T1*P2/T2P1= 298*3876/588*727=2.702

and V1=2.702*V2=257*2.702=694L

Answer 2

Sounds like homework. I used to check the back of my textbook, sometimes they have the answers there. If not, I just copy off my friend before class started. Ofcourse, you could just read the material...