For the equilibrium $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)} + 14.6 \ kcal$,the increase in temperature would

For the exothermic reaction $Cl_{2(g)} + 3F_{2(g)} \rightleftharpoons 2ClF_{3(g)}$,$\Delta_r H = -329 \ kJ$,which of the following will increase the quantity of $ClF_3$ in the equilibrium mixture?

Consider the following reaction:
$N_{2}O_{4(g)} \rightleftharpoons 2NO_{2(g)} ; \Delta H^{0} = +58 \ kJ$
For each of the following cases $(a, b)$,determine the direction in which the equilibrium shifts:
$(a)$ Temperature is decreased
$(b)$ Pressure is increased by adding $N_{2}$ at constant $T$ and constant $V$

For the reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$,$\Delta H^o = -198 \, kJ$. According to Le Chatelier's principle,the favorable conditions for the forward reaction are:

The following gaseous reaction is taking place in a vessel: $C_2H_4(g) + H_2(g) \rightleftharpoons C_2H_6(g)$; $\Delta H = -32.7 \ kcal$. Which of the following will increase the equilibrium concentration of $C_2H_6$?

For the reaction $2X_{(g)} + Y_{(g)} \rightleftharpoons 2Z_{(g)} + 80 \ kcal$,which conditions of temperature and pressure will yield more $Z$ at equilibrium?