[Image] The synthesis of ammonia gas from nitrogen and hydrogen gases was an exe
ID: 858505 • Letter: #
Question
[Image]
The synthesis of ammonia gas from nitrogen and hydrogen gases was an exemplary case of a chemical reaction that was made economically feasible by optimizing kinetic and equilibrium factors. Explain how each of the factors below contributed to increase the reaction yield. (a) using an elevated temperature for the reaction (b) removing the NH3 from the reaction as soon as it is formed (c) using a catalyst (d) running the reaction @ high pressure Liquids A and B form an ideal solution. At 45degreeC, the vapor pressures of pure A and pure B are 66 and 88 Torr, respectively. Calculate the composition of the vapor in equilibrium with a solution containing XA=0.36.Explanation / Answer
N2(g) + 3H2(g) <....Fe........> 2NH3(g) DH = -92Kj/mol
a) it is an exo thermic reaction if we increase the temperature equilibroium shifts in the backward direction which leads to decrease in the formation of NH3
b) so if we remove the NH3 from the reaction the enquilibrium shifts in the forward direction to produce NH3
c) here the catalyst is Fe which can provide the surface for the N2+H2 to perticipate in the reaction and also decreases the time to reach the equilibrium. overal it increases the yield of NH3
d) more is the pressure the equilibrium shifts in the forward direction to yield more amount of NH3
2)
Total pressue = Pa + Pb
= 66 + 88
= 154 torr
mole fraction of B = 1- 0.36 = 0.64
mole fraction of B = no.of moles of B/ total no.of moles of solution
0.64 = no.of moles of B/ total no.of moles of solution
total no.of moles of solution = no.of moles of B/0.64
mole fraction of A = no.of moles of A/ total no.of moles of solution
0.36 = no.of moles of A*0.64 / no.of moles of B
no.of moles of A / no.of moles of B = 0.56
Related Questions
drjack9650@gmail.com
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.