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The decomposition of ammonia is: 2NH3(g) → N2(g) + 3H2(g). If Kp is 1.5×103 at 400°C, what is the partial pressure of ammonia at equilibrium when N2 is 0.40 atm and H2 is 0.15 atm?

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Alyssa Mae Remarim
Alyssa Mae RemarimLv10
18 Nov 2020

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Related questions

Calculate the free-energy change for ammonia synthesis at 25oC given the following sets of partial pressures:

(a) 1.0 atm N2, 3.0 atm H2, 0.020 atm NH3

(b) 0.010 atm N2, 0.030 atm H2, 2.0 atm NH3

N2(g) + 3H2(g)--->2NH3(g) DeltaG* = -33.0 kJ

Please explain

At 25 degrees C,Kp= 5.3*10^5 for the reaction

N2(g) + 3H2(g) = 2NH3(g).

When a cretain partial pressure of NH3 is put into an otherwiseempty rigid vessel at 25 degrees C, equilibrium is reached when 50%of the original ammonia has decomposed. What was the originalpartial pressure of ammonia before any decomposition occurred?

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