Homework SourseShow work to receive credit 1 At 2273 K the equilibrium cons
Show work to receive credit!
1. At 2273 K the equilibrium constant for the reaction
What would be the equilibrium concentration of N2 if the initial concentration of NO was 0.1339 M?
2. What would Qc be if the pressure of the container increased by a factor of 4.147 for the following reaction?
at 1400oC
| 2 NO(g) « N2(g) + O2(g) | KC = 2400 |
Solution
1.
N2 + O2 --> 2NO, Kc = 2400
Kc = 2400 = [NO]^2 / [N2][O2]
NOÂ º = 0.1339M
Kc = (0.1339-2x)^2 / x^2
solve
[N2] = x M
2.
Kp = Kc(RT)^(delta n)
For (RT)^(delta n), which I assume I solve normally, I just plug in numbers for it so I get,
(RT)^(delta n) = (0.0821)(1673)^(2)
So, the only thing I need to compare is Kc and Kp.
pressure is increasing by 4.147, so
I multiply Kc by 4.147
Kp = ((4.147)(0.07520))((0.0821)(353)^(2))
