Le Chatelier's Principle

According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will respond by shifting the equilibrium position. If the concentration of $A$ in the reaction $A \rightleftharpoons B$ is increased, what will happen to the equilibrium position?

In the reaction $N_{2}(g) + 3H_{2}(g) \rightleftharpoons 2NH_{3}(g)$, if the pressure is increased, what will happen to the equilibrium position?

What happens to the equilibrium position of the reaction $C(s) + 2H_{2}(g) \rightleftharpoons CH_{4}(g)$ if the temperature is increased and the reaction is endothermic?

In the reaction $2SO_{2}(g) + O_{2}(g) \rightleftharpoons 2SO_{3}(g)$, which of the following changes will shift the equilibrium to the right?

For the reaction $A(g) \rightleftharpoons B(g)$, if the volume of the container is decreased, what will be the effect on the equilibrium position?

Which of the following changes will not affect the position of equilibrium for the reaction $P(g) + Q(g) \rightleftharpoons R(g)$?

In the reaction $D(g) \rightleftharpoons E(g) + F(g)$, if $F$ is removed from the system, what will happen to the equilibrium position?

For the equilibrium reaction $X(aq) \rightleftharpoons Y(aq)$, if the temperature is decreased and the reaction is exothermic, what will happen to the equilibrium?