Under the appropriate conditions, NO forms NO2 and N2O:

Question

3NO(g) <--> N2O(g) + NO2(g)

Use the values for delta G naught for the following reactions to calculate the value of Kp for the above reaction at 500.0 C

2NO(g) + O2(g) <--> 2NO(g)
delta g=-69.7 kJ

2N2O(g) <--> 2NO(g) + N2(g)
delta g= -33.8 kJ

N2(g) +O2(g) <--> 2NO(g)
delta g= 173.2 kJ

Kp=??

Answer 1

Check that post. 2NO + O2 ==> 2NO isn't balanced. I didn't check the rest of the post.

Answer 2

Its supposed to be 2NO + O2 <--> 2NO2. I forgot the 2.

Answer 3

eqn 1 as is
eqn 2 reversed.
eqn 3 reversed.
Add 1+2+3 to find total equn which will give you twice the numbers for coefficients. Divide everything by 2.
For dH, keep 1 as is, change the sign on 2 and 3 and add them, then divide by 2 to find dGo rxn
Then dGo = -RTlnK
you know dGo, R is 8.314, T is 500 C (change to kelvin), solve for Kp. .

Answer 4

so to invert the equation to get k by itself its ln(dGo/-RT) ?? that's my answer?

Answer 5

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