the following equilibrium: 4NH_3(g) + 3H_2(g) delta G degree = 34. kJ Now suppos
ID: 524318 • Letter: T
Question
the following equilibrium: 4NH_3(g) + 3H_2(g) delta G degree = 34. kJ Now suppose a reaction vessel is filled with 8.92 atm of ammonia (NH_3) and 2.35 atm of nitrogen (N_2) at 72 degree C. Answer the following questions about this system: Under these conditions, will the pressure of NH_3 tend to rise to fall? rise fall Is it possible to reverse this tendency by adding H_2? In other changed words, if you said the pressure of NH_3 will tend to rise, can that be changed to a tendency to fall by adding H_2? Similarity, if you said the pressure of NH_3 will tend to fall, can that be changed to a tendency to rise by adding H_2? yes no If you said the tendency can be reversed in the second question, calculate the minimum pressure H_2 needed to reverse it. Round your answer to 2 significant digits. AtmExplanation / Answer
Q1.
Under these conditions, we should expect some NH3 to decrease, since there are only NH3, N2... They must react in order to favour H2 production, so this is forward direction, NH3 decrease in P
Q2.
If we add more H2, then we can make an equilibrium, and eventually, favour NH3 production, so NH3 increas in pressure
Q3.
Q > 1
1 = (2.35)(H2)^3 / (8.92^4)
H2 = ((8.92^4) / 2.35 ) ^(1/3) = 13.9143 atm
So any Pressure above H2 > 13.9143 atm will do
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.