A flask initially contains 2.00 atm of NH3, 2.00 atm of N2, and 3.00 atm of H2 at 673 Kelvin.
-What is the delta G for the reaction?
-What is the equilibrium partial pressures of each gas at 673 Kelvin?
So I figured out how to do the first question with relevant values:
: delta G standard = -170.202
: delta G = -152
: Q = 27
: Kp = 2.09 x 10^ 13
And I believe the chemical equation is
[atm] 2NH3(g) <--> 2N2(g) + 3H2(g)
I 2.0 2.00 3.00
C -2 +2 +2
E 0 4 5
------------------------------------
I 0 4 5
C +2x -2x -3x
E 2x 4-2x 5-3x
Kp= [((4-2x)^2) ((5-3x)^2)]
/ [2x^2]
But the answer that I was told was correct was that:
[NH3] = 1.4 x 10^-3 atm
[N2] = 4 atm
[H2] = 6 atm
2 answers
Your equation is not balanced and Q is not 27; therefore, those initial values you have are incorrect. Correct those and try the last part again. Also, is that -170 what? kJ? kJ/mol? kJ/rxn?
Hello Dr. Bob,
I see the mistake that I have made, but the initial values that were in my first sentence were given, I just think my coefficients in the equation were wrong. Do the answers at the bottom make sense though?
I see the mistake that I have made, but the initial values that were in my first sentence were given, I just think my coefficients in the equation were wrong. Do the answers at the bottom make sense though?
27 answers