Question #88a40

1 Answer
Nov 5, 2017

The rate would increase.


It is good to start by saying that formation of Ammonia from Nitrogen and Hydrogen is quite difficult. As a matter of fact, the person who discovered this (I don't remember his name off the top of my head) found out that the reaction would only occur at very high temperatures and high pressure. Also, he found that it was really important to have a catalyst.

So the answer to your question is that high pressure would increase the rate of the reaction. The primary purpose of increasing the pressure is to increase the percentage of Ammonia in the equilibrium mixture.

It is also good to use the ideal gas equation in this situation:

#pV = nRT#

As long as the temperature is constant, that would make RT constant, which means you can rearrange the equation to have P (pressure) on one side of the equal sign, and then you'll see that pressure is directly proportional to the concentration:

#p = n/V * RT#

(#n/V#) is concentration.

Hope it helped (c: