Which of the following is not favourable for $SO_3$ formation in the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}; \Delta H = -45.0 \ kcal$?

For the equilibrium $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)} + 21.9 \ kcal$,an increase in temperature will:

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

For a reaction if $K_p > K_c$,the forward reaction is favoured by

For the reaction $CO_{(g)} + H_2O_{(g)} \rightleftharpoons CO_{2(g)} + H_{2(g)}$,the equilibrium amount of $CO_{2(g)}$ increases by:

In which reaction will an increase in the volume of the container favour the formation of products?