Question
I am given the following reaction:
2NH3(g) -----> N2(g) + 3H2(g)
6.4 mols of ammonia gas has been put into a 1.7 L flask and has been permitted to reach equilibrium in accordance to the reaction listed above. If the equilibrium mixture has 4.2 mols of nitrogen, what is the value of the equilibrium constantsupposed to be?
My question is, how do I arrive at the following in my answer:
[N2] = 2.7 moles in 2.2l = 1.22 moles/liter
Where did the 2.7 moles come from?
2NH3(g) -----> N2(g) + 3H2(g)
6.4 mols of ammonia gas has been put into a 1.7 L flask and has been permitted to reach equilibrium in accordance to the reaction listed above. If the equilibrium mixture has 4.2 mols of nitrogen, what is the value of the equilibrium constantsupposed to be?
My question is, how do I arrive at the following in my answer:
[N2] = 2.7 moles in 2.2l = 1.22 moles/liter
Where did the 2.7 moles come from?
Answers
drwls
If the reaction went to completion, the 6.4 mols of NH3 would produce 3.2 mols of N2 and three times as many of H2. I don't see how 4.2 mols of N2 could be formed. I also don't see where the 2.7 moles came from. Have you stated all numbers of the problem correctly?