00:02
In this problem, we're going to consider the following exothermic equilibrium and how the changes would affect the equilibrium mixture of the gases.
00:12
A catalyst is added to the mixture.
00:15
This will not affect the equilibrium mixture, except equilibrium will be reached faster, although the concentrations will not change.
00:25
This is because a catalyst lowers the activation energy, but it does not affect the position of equilibrium.
00:30
For b, carbon dioxide is added to the system.
00:35
This will cause the equilibrium to shift left because based on the chalachalier's principle, the equilibrium will shift to offset any change to the equilibrium.
00:48
If we increase the concentration of the products, it will shift towards reactants to use the products.
00:55
So for c, we add reactant carbon monoxide.
01:00
So in this case, it will shift to the right towards the products to use up carbon monoxide.
01:07
The reaction mixture is heated.
01:09
So if we heat this reaction, the reaction will shift away from the side of the heat.
01:14
This is exothermic, so heat is on the product side...