NEET Chemistry MCQs

A gaseous organic compound has an empirical formula $C_xH_y$. When 0.150 g of the compound is completely combusted, it produces 0.225 g of $CO_2$ and 0.090 g of $H_2O$. Given the vapor density of the compound is 29, what is the molecular formula?

The vapour density of completely dissociated ${\rm{N}}{{\rm{H}}_4}{\rm{Cl}}$ would be:

The vapour density of undecomposed ${{\rm{N}}_2}{{\rm{O}}_4}$ is 46. When heated, vapour density decreases to 24.5 due to its dissociation to ${\rm{N}}{{\rm{O}}_2}.$ The per cent dissociation of ${{\rm{N}}_2}{{\rm{O}}_4}$ at the final temperature is :

The vapour density of undecomposed ${{\rm{N}}_2}{{\rm{O}}_4}$ is 46. When heated, vapour density decreases to 24.5 due to its dissociation to ${\rm{N}}{{\rm{O}}_2}.$ The per cent dissociation of ${{\rm{N}}_2}{{\rm{O}}_4}$ at the final temperature is :

The vapour density of ${\rm{PC}}{{\rm{l}}_5}$ is 104.16, but when heated at 230℃. Its vapour density is reduced to 62. The percentage of dissociation of ${\rm{PC}}{{\rm{l}}_5}$ at this temperature will be

The vapour density of ${\rm{PC}}{{\rm{l}}_5}$ is 104.16, but when heated at 230℃. Its vapour density is reduced to 62. The percentage of dissociation of ${\rm{PC}}{{\rm{l}}_5}$ at this temperature will be