According to Le $Chatelier$ principle,if heat is given to a solid-liquid system,then:

The exothermic formation of $ClF_3$ is represented by the equation
$Cl_{2(g)} + 3F_{2(g)} \rightleftharpoons 2ClF_{3(g)}$; $\Delta H_r = -329 \ kJ$
Which of the following will increase the quantity of $ClF_3$ in an equilibrium mixture of $Cl_2, F_2$ and $ClF_3$?

Under which of the following conditions of temperature and pressure will molecular hydrogen $(H_2)$ dissociate into atomic hydrogen $(H)$?

In the equilibrium $N_2 + 3H_2 \rightleftharpoons 2NH_3 + 22 \ kcal$,the formation of ammonia is favoured by

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

In the equilibrium reaction
$AgCl_{(s)} + 2NH_3(aq.) \rightleftharpoons [Ag(NH_3)_2]^+ (aq.) + Cl^{-} (aq.)$
Increase in the concentration of $Cl^{-} (aq.)$ causes