At equilibrium,what happens to the boiling point of $H_2O$ when pressure is increased?

Explain the effect of a catalyst on chemical equilibrium with examples.

For the reaction: $A + B + Q \rightleftharpoons C + D$,if the temperature is increased,then the concentration of the products will

Consider the following reactions. In which cases is product formation favoured by decreased temperature?
$(a) \ N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}; \ \Delta H^o = 181 \ kJ$
$(b) \ 2CO_{2(g)} \rightleftharpoons 2CO_{(g)} + O_{2(g)}; \ \Delta H^o = 566 \ kJ$
$(c) \ H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}; \ \Delta H^o = -9.4 \ kJ$
$(d) \ H_{2(g)} + F_{2(g)} \rightleftharpoons 2HF_{(g)}; \ \Delta H^o = -541 \ kJ$

When $NaNO_{3(s)}$ is heated in a closed vessel,$O_{2(g)}$ is released and $NaNO_{2(s)}$ remains. The equilibrium is: $NaNO_{3(s)} \rightleftharpoons NaNO_{2(s)} + 1/2 O_{2(g)}$. Which of the following is correct?

For the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3 + 21.9 \, kcal$,under which conditions is the production of ammonia favored according to Le Chatelier's principle?