According to Le Chatelier's principle, in the reaction $\mathrm{CO}(\mathrm{g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons \mathrm{CH}_4(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}(\mathrm{g})$, the formation of methane is favoured by
(a) Increasing the concentration of CO
(b) Increasing the concentration of $\mathrm{H}_2 \mathrm{O}$
(c) Decreasing the concentration of $\mathrm{CH}_4$
(d) Decreasing the concentration of $\mathrm{H}_2$
The equilibrium constant at 298 K for the reaction $\mathrm{A}+\mathrm{B} \rightleftharpoons \mathrm{C}+\mathrm{D}$ is 100 . If the initial concentrations of all the four species were 1 M each, then equilibrium concentration of D (in $\mathrm{mol} \mathrm{L}^{-1}$ ) will be
Among the following 0.1 m aqueous solutions, which one will exhibit the lowest boiling point elevation, assuming complete ionization of the compound in solution?
Variation of solubility with temperature t for a gas in liquid is shown by the following graphs. The correct representation is



