$A$ gas has the formula $[CO]_x$. If its vapor density is $70$,what is the value of $x$?

The equilibrium constant for the decomposition of $H_2O_{(g)}$: $H_2O_{(g)} \rightleftharpoons H_{2(g)} + \frac{1}{2} O_{2(g)}$ $(\Delta G^{\circ} = 92.34 \ kJ \ mol^{-1})$ is $8.0 \times 10^{-3}$ at $2300 \ K$ and the total pressure at equilibrium is $1 \ bar$. Under this condition,the degree of dissociation $(\alpha)$ of water is $............ \times 10^{-2}$ (nearest integer value). [Assume $\alpha$ is negligible with respect to $1$]

$3.2 \text{ moles of hydrogen iodide are heated in a closed vessel at } 444^{\circ}C \text{ until equilibrium is reached. If the degree of dissociation at this temperature is } 22\%, \text{ then the number of moles of hydrogen iodide remaining at equilibrium will be:}$

At $STP$,the density of air is $0.001293 \ g \ mL^{-1}$. Its vapour density is $---$.

At temperature,$T$,a compound $AB_{2(g)}$ dissociates according to the reaction; $2AB_{2(g)} \rightleftharpoons 2AB_{(g)} + B_{2(g)}$ with a degree of dissociation $x$,which is small compared with unity. The expression for $K_p$,in terms of $x$ and the total pressure,$P$ is

For the reaction $A \rightleftharpoons \frac{1}{2} B + C$,the degree of dissociation $\alpha$ in terms of vapour density $D_t$ (theoretical) and $D_o$ (observed) is given by: