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 $\%$)

The vapour density of a gas is $11.2$. The volume occupied by $11.2 \ g$ of the gas at $STP$ will be.....$L$

If in the reaction $N_2O_4 \rightleftharpoons 2NO_2$,$\alpha$ is the fraction of $N_2O_4$ that dissociates,then the total number of moles at equilibrium is:

In a $100 \ L$ vessel,$3 \ moles$ of nitrogen and $3 \ moles$ of $PCl_5$ are taken and heated to $500 \ K$. The equilibrium pressure is $3.28 \ atm$. The percentage degree of dissociation of $PCl_5$ is : (Assume ideal behaviour for all gases).

$A_{(g)} \rightleftharpoons 2B_{(g)} + C_{(g)}$
For the given reaction,if the initial pressure is $450 \ mm \ Hg$ and the total pressure at time $t$ is $720 \ mm \ Hg$ at a constant temperature $T$ and constant volume $V$. The fraction of $A_{(g)}$ decomposed under these conditions is $x \times 10^{-1}$. The value of $x$ is $......$. (nearest integer)

In a Victor Meyer's experiment,$0.23 \ g$ of a volatile solute displaces $112 \ mL$ of air at $NTP$. What is the vapor density of the substance?