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

In which of the following reactions will an increase in pressure shift the equilibrium in the backward direction?

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 $ClF_3$?

Based on Le Chatelier's principle,which of the following information is obtained?

Adding an inert gas to the system $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ at equilibrium at constant volume will lead to: