00:01
In this question we are supposed to consider a system that is an equation is given 4nh3 in gaseous state plus 3 oxygens in gaseous state 2n2 in gaseous state and then we have 6h2o in the liquid state.
00:20
So this is the equation or the system that is given to us.
00:24
Now we have to find how will the amount of ammonia at equilibrium be affected.
00:30
How will the amount of ammonia be affected by changing some things in the equation or changing some environmental conditions.
00:43
What first that we are given is removing oxygen.
00:48
If you remove oxygen, now oxygen you can see oxygen is one of the reactants.
00:56
Now if you see according to the equation given to us oxygen is a reactant.
01:04
So in this question we basically use le chatelier's principle.
01:13
And according to the equation if you see, oxygen is nothing but it is a reactant.
01:24
So according to le chatelier's principle what happens is if a reactant is removed from the system that is oxygen over here is removed from the system, the equilibrium will shift in the direction that replaces the reactant.
01:37
Equilibrium will shift in the direction that can replace the reactant.
01:41
So in this case removing oxygen will shift equilibrium towards reactant.
01:54
So therefore equilibrium will shift towards which direction? towards the reactant.
02:01
Because this is the direction that can replace the reactant.
02:07
So somehow your equation, your equilibrium should now replace the reactant.
02:11
So that is why the equilibrium will shift towards the reactant.
02:15
So equilibrium will shift towards reactant.
02:18
As a result what will happen? there will be as a result what happens? there will be increase in the amount of ammonia because the reaction is shifted towards the reactant.
02:31
So amount of ammonia will now increase because ammonia is also on the reactant side.
02:37
Ammonia if you see in the equation ammonia is on the reactant side and now the equation are shifted to the reactant side.
02:44
So there will be increase in the amount of ammonia at equilibrium.
02:50
So this will be for the first part.
02:52
Similarly we have three four conditions and we have to find what happens in all of those conditions.
02:58
If you go for the second part adding water you add water not adding water second is adding n2 adding n2 sorry second is adding n2 n2 gas.
03:12
Now if you see similarly like the first one n2 but now n2 is in the product side.
03:18
So here what happened is we are increasing the product.
03:22
Okay so according to le chatelier's principle again according to so here in this question for each of the parts we use le chatelier's principle.
03:30
So again according to le chatelier's principle when product is added the equilibrium will shift in the direction that reduces the concentration of the product.
03:37
So now product is increasing so i have to reduce the product.
03:40
So for that reason according to le chatelier's principle the equilibrium will shift in the direction that reduces the concentration of the product and in this case the equilibrium will shift where the equilibrium will shift again towards the will shift towards the reactant again towards the reactant because why i have to reduce the amount of product that is why again the equilibrium will shift towards or in the direction of the reactants.
04:11
Okay so what happens when a product is added the equilibrium will shift in the direction that reduces the concentration of the product...