00:01
So in the reaction that we're given in this problem, if we read it forward as we normally would for a chemical reaction, we would have our reactants that's eye colored in red, which are a and b, and then we'll have our products c and d.
00:17
So let's start by answering the first part of the question.
00:21
I wrote one.
00:22
It's actually part a.
00:23
But the first part of the question is telling us that we are going to increase the concentration of a.
00:32
And then we are going to allow this mixture to go to equilibrium once again.
00:39
When we increase the concentration of a reactant, in this case a, equilibrium, the equilibrium is going to favor the products side of the reaction.
01:04
So it will favor the products.
01:18
And what that actually means is that it will shift right.
01:26
And this follows le chateailliers principle where we want to restore equilibrium.
01:38
And what we've done is we've added an excess amount of a.
01:42
So to get rid of that excess we need to move forward and allow that excess a to react with the b in order to produce more c and d.
01:51
And then once that happens, the excess is gone.
01:54
And equilibrium is restored.
01:56
So what's going to end up happening to the concentrations? well for a, a is kind of a special case because a we added, initially we added.
02:08
So the concentration of a is going to be increased, but this is compared to original.
02:17
So that's before we added a.
02:30
So i'll abbreviate original...