There is more than one reaction in which nitric oxide,NO, could be a reactant of product. Which reaction is your question about? What is the chemical equation for it?
i. I answered the effect of increasing pressure previously.
N2 + O2 ==> 2NO
Since mole on the left (2) equals moles on the right (2), pressure has no effect on the equilibrium; i.e., the reaction will not shift either direction as the result of increasing or decreasing P.
ii. Here is a site that gives Kp for the reaction at 530 C and a Kp for the reaction at 25 C. From these data you should be able to figure out how the yield will be affected by increasing T.
iii. Since increasing T increases the motion of molecules and that will increase the chances for collisions, the rate of reaction should increase.
That isn't 250 words, but it tells you what is going on. Now put all of that into a nice sounding two pages (about 125 words to a page handwritten) and you will be done.
iii. The effect of increasing T, should provide more energy to the molecules, that
By the way, if the reaction you are studying is different from that which I described previously and above, my pat answers above may change.
Here are some guidelines on equilibria involving gases:
1. Increasing the pressure causes a shift toward the side with the smallest number of gas molecules.
2. Increasing the temperature causes a shift in the direction of the endothermic change. That could be the forward or the reverse reaction. I assume you were told which.
3. Increasing the temperature increases both reaction rates (forward and reverse). The rate increase will be larger for the rate that would help reestablish equilibrium.