I'm going to hazard a guess because I haven't done this for a while...
1. An equilibrium is when a reversible reaction is balanced and the overall chemical concentrations and activity of both the reactants and the products has no overall net change. In an equilibrium, a forward and backward reaction occurs.
2. (Just so you know, in a equilibrium reaction, you can either go from turning the reactants into products or you can go backwards by changing the products back into the reactants.)
If you shift the equilibrium position to the right, then you are producing more product by forcing the reaction to go in the direction of the arrow facing right.
If you shift the equilibrium position to the left, then you are turning more of the product back into the reactant(s) by forcing the reaction to go in the direction of the arrow facing left.
3. In an equilibrium, one way the reaction is going to be exothermic and the other way it will be endothermic. Thus, when you increase the temperature, the reaction will want to lower the temperature and therefore the endothermic reaction will occur more to counterbalance this. Therefore, if you decrease the temperature, the exothermic reaction will occur more.
If you increase the pressure, the equilibrium system will shift so the least number of gas molecules are formed because the more gas molecules there are, the more collisions there are because these collisions and the presence of gas molecules are what cause the pressure to increase. Therefore, a decrease in pressure will force the reaction in the direction of more number of gas molecules.
A catalyst increases the rate of reaction but this would not effect the equilibrium itself so it will remain balanced.
I hope this helps and actually makes sense. I also hope that it's right
