00:01
Hi, so to solve for this, the concepts that you have to remember is that when the equilibrium constant, in this case equilibrium constant based on partial pressure, is greater than the reaction quotient, then it will favor the forward reaction.
00:22
Forward reaction.
00:25
If the equilibrium constant is less than the reaction quotient, then it will favor the reverse reaction.
00:36
And if the equilibrium constant is equivalent to the reaction quotient, then the reaction is at equilibrium.
00:44
So first, in order to answer this question, we need to calculate the reaction quotient based on partial pressure.
00:51
This will be equivalent to the partial pressure of the product we have, icl, and then we need to raise this to the power of 2 because the coefficient is 2 based on our balance equation.
01:03
Over the partial pressure of the reactants, we have iodine, and then the partial pressure of cl2.
01:10
Let's plug in the information that we have.
01:12
We have 0 .28, then squared, over 0 .28 multiplied by 0 .28...