[silladuckaroo]

Hello,
Can someone help me on this quick question, please?
Please see my work below....

Consider the gas phase reaction
     NO + (1/2)O2  <-->NO2
for which  H° = -57.0 kJ and K = 1.5 x 106 at 25°C.
What would be the effect on the amount of NO present of compressing the equilibrium system to a smaller volume, while keeping the temperature constant?
A.   The amount of NO will increase.
B.   The amount of NO will decrease.
C.   The amount of NO will remain the same.
D.   Not sure.

I think the answer is B, that the NO will decrease. This is because Ho is negative and that there are more moles on the left side. Is this correct?
Please tell me if I am taking the right approach to this problem. Thank you!
I really appreciate your *delete me*

[Mitch]

You have to solve for the equilibrium constant in terms of partial pressures. That's a much better way to approach this problem.