On cooling the following system at equilibrium:
$CO_{2(s)} \rightleftharpoons CO_{2(g)}$

$A$ reversible reaction is in equilibrium. If a factor is changed which affects it,then:

In the equilibrium $2A_{(g)} + 3B_{(g)} \rightleftharpoons 3C_{(g)} + 2D_{(g)}$,an increase in pressure will:

For which of the following reactions will a change in the volume of the system $NOT$ result in a change in the number of moles of the components?

When $KOH$ is dissolved in water,heat is evolved. If the temperature is raised,the solubility of $KOH$

The reaction $C_2H_{6(g)} \rightleftharpoons C_2H_{4(g)} + H_{2(g)}$ is at equilibrium in a closed vessel at $1000 \ K$. The enthalpy change $(\Delta H)$ for the reaction is $137.0 \ kJ \ mol^{-1}$. Which one of the following actions would shift the equilibrium to the right?