For the reaction $aA + bB \rightleftharpoons cC + dD$,if the equilibrium shifts in the backward direction at low pressure and high temperature,which of the following is correct?

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

For the equilibrium $C_{(diamond)} \rightleftharpoons C_{(graphite)}$,the densities of diamond and graphite are $3.5 \ g/mL$ and $2.3 \ g/mL$ respectively. What happens to the equilibrium upon increasing the pressure?

The equilibrium of the reaction $2A_{(s)} + 3B_{(g)} \rightleftharpoons 3C_{(g)} + D_{(g)} + Q$ is represented as shown. If the pressure on the system is reduced to half of its original value,then:

In a vessel containing $SO_3$,$SO_2$,and $O_2$ at equilibrium,some helium gas is introduced so that the total pressure increases while temperature and volume remain constant. According to Le Chatelier's principle,the dissociation of $SO_3$:

Aqueous solution of ferric nitrate when mixed with aqueous solution of potassium thiocyanate gives a red coloured solution. The intensity of the red colour becomes constant upon attaining equilibrium. Choose the correct statement when the following chemicals are added to the above solution at equilibrium:
$I$. Oxalic acid
$II$. Mercuric chloride