Equilibria: describe question

The formation of methanol from carbon monoxide and hydrogen is a reversible reaction that reaches dynamic equilibrium. $\ce{CO(g) + 2H2(g) <=> CH3OH(g)}$ The forward reaction is exothermic. Describe the meaning of dynamic equilibrium in terms of the rates of reaction and the concentrations of reactants and products. Explain why a closed system is necessary for dynamic equilibrium to be established. Using Le Chatelier's principle, predict the effect of increasing the temperature and of increasing the pressure on the yield of methanol at equilibrium. Deduce the expression for the equilibrium constant in terms of concentration, Kc, and the expression for the equilibrium constant in terms of partial pressures, Kp, for this reaction. Ensure that your Kp expression shows how the partial pressures are expressed in terms of mole fractions and total pressure.