Two questions for everyone.
First is the answer 6.36atm for the question: The reaction 2NO + Br2 -> 2NOBr has Kp = 109 at 25 degrees C. If the equilibrium partial pressure of Br2 is 0.0159atm and the equilibrium partial pressure of NOBr is 0.0768atm, calculate the partial pressure of NO at equilibrium.
The second question is how do you figure out this problem?: 3H2 + N2 -> 2NH3. At 200 degrees C in a closed container, 1.00atm of nitrogen gas is mixed with 2.00atm of hydrogen gas. At equilibrium, the total partial pressure is 2.00atm. Calculate the partial pressure of hydrogen gas at equilibrium
2007-03-08 14:33:07 · 1 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
1. Looks suspect to me: If I remember my equilibrium right,
[NOBr]^2 / { [NO]^2[Br2] } =109
did you work with this?
2. Let P be the pp of nitrogen in atm. Then
1-P + 2-3P + 2P =2
(nitrogen) (hydrogen) (ammonia)
P= 0.5, and partial pressure of hydrogen gas= 0.5 atm.
2007-03-08 14:48:53 · answer #1 · answered by cattbarf 7 · 0⤊ 0⤋