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Question 10:
A reversible reaction is a chemical reaction that proceeds in both the forward and reverse directions, represented by the equilibrium symbol $\rightleftharpoons$.

Example:
$\ce{N2(g) + 3H2(g) <=> 2NH3(g)}$

Question 11:
Chemical equilibrium is referred to as "dynamic" equilibrium because the forward and reverse reactions continue to occur at the same rate, even though the concentrations of reactants and products remain constant over time.

Question 12:
According to Le Chatelier's Principle, if the temperature of a system at equilibrium is increased, the equilibrium shifts in the direction that absorbs heat (endothermic direction). For an exothermic reaction, increasing temperature shifts the equilibrium to the left (towards reactants); for an endothermic reaction, it shifts to the right (towards products). Decreasing temperature shifts the equilibrium in the opposite direction.

Example (exothermic):
$\ce{N2(g) + 3H2(g) <=> 2NH3(g)} \quad \Delta H < 0$
Increasing temperature shifts left.

Question 13:
According to Le Chatelier's Principle, increasing the pressure on a gaseous equilibrium shifts the position of equilibrium towards the side with fewer moles of gas. Decreasing pressure shifts it towards the side with more moles of gas. Pressure changes do not affect equilibria involving only solids or liquids.

Example:
$\ce{N2(g) + 3H2(g) <=> 2NH3(g)}$
4 moles (left) $\rightleftharpoons$ 2 moles (right). Increasing pressure shifts right.