In the reaction ${A_2}_{(g)} + 4{B_2}_{(g)} \rightleftharpoons 2A{B_4}_{(g)}$ where $\Delta H < 0$,the formation of $AB_{4(g)}$ will be favoured by:

Explain the effect of temperature on equilibrium using a suitable experiment.

The value of $\Delta H$ for the reaction $X_{2(g)} + 4Y_{2(g)} \rightleftharpoons 2XY_{4(g)}$ is less than zero. Formation of $XY_{4(g)}$ will be favoured at

The following reaction occurs in the blast furnace where iron ore is reduced to iron metal:
$Fe_2O_{3(s)} + 3CO_{(g)} \rightleftharpoons 2Fe_{(l)} + 3CO_{2(g)}$
Using Le Chatelier's principle,predict which one of the following will not disturb the equilibrium.

For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,the forward reaction is favored at constant temperature by: $(1)$ Adding an inert gas at constant volume $(2)$ Adding $Cl_{2(g)}$ at constant volume $(3)$ Adding an inert gas at constant pressure $(4)$ Increasing the volume of the container $(5)$ Adding $PCl_{5(g)}$ at constant volume

For the reaction $aA \rightleftharpoons lL + mM$,if the volume is suddenly increased,the degree of dissociation decreases. What does this indicate?