00:02
Hey there.
00:02
To start this problem off, let's go ahead and write our equation.
00:06
We have 2nh3, which is a gas, and it's in equilibrium with n2, gas, and 3, h2, also gas.
00:28
So we can write an equilibrium constant based upon pressure for this.
00:33
So that would be kp.
00:36
And the way that we write the equilibrium expressions by putting the products over the reactants.
00:42
So we would take the partial pressure of the nitrogen and multiply that times the partial pressure of the hydrogen.
00:55
And since there's a coefficient of 3 on the h2, we need to write that as an exponent.
01:02
So the partial pressure of h2 cubed.
01:05
This is going to be over the part of h2.
01:07
Partial pressure of our reactant, our nh3.
01:13
And since that has a coefficient of two, that needs to be squared.
01:18
So coefficients become exponents in the equilibrium expression.
01:22
Okay, so given this expression, we have three of these four variables, and we can solve for the fourth.
01:27
So we're told that kp is 1 .5 times 10 to the third at this temperature.
01:35
So notice that's a very high kp.
01:37
It's a very large number, which means the products are favored.
01:42
So we would expect the partial pressure of the ammonia to be far less than that of the nitrogen or the hydrogen.
01:50
Okay, this is going to be equal to the partial pressure of the nitrogen, which is 0 .10 atmospheres, and the partial pressure of the hydrogen is 0 .15.
02:04
We need to cube this value.
02:10
This is all over the partial pressure of the nh3, which is what we're trying to find.
02:16
And that has to be squared...