The vapor density of a gas is $11.2$. At $N.T.P.$,$11.2 \ g$ of this gas occupies a volume of ............. $litres$.

At $T \, ^\circ C$,the vapour density of $PCl_5$ is $104.25$. The degree of dissociation of $PCl_5$ is ....$\%$

In a $Victor \ Meyer$ experiment,$0.23 \ g$ of a volatile substance displaces $112 \ mL$ of air at $STP$. Calculate the vapor density of the substance.

In a closed vessel,the dissociation of phosphorus pentachloride occurs as: $PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$. If the total pressure at equilibrium is $P$ and the degree of dissociation of $PCl_5$ is $x$,then the partial pressure of $PCl_3$ will be:

For the equilibrium reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the value of $K_p$ is $2$. Calculate the percentage dissociation of $N_2O_{4(g)}$ at a total pressure of $0.5 \ atm$. (in $\%$)

Ammonium carbamate $(NH_4COONH_2)$ when heated to $200 \ ^oC$ gives a mixture of $NH_3$ and $CO_2$ with a vapour density of $26$ at equilibrium. What is the degree of dissociation of ammonium carbamate?