States of Matte...

For the two compounds, the vapour pressure of (2) at a particular temperature is expected to be:-

$$100\space g$$ of liquid $$A$$(molar mass $$140\space g { mol }^{ -1 })$$ was dissolved in $$1000\space g$$ of liquid $$B$$ (molar mass $$180 \space g { mol }^{ -1 })$$. The vapour pressure of pure liquid $$B$$ was found to be $$500 \space torr.$$ Calculate the vapour of pure liquid $$A$$ and its vapour pressure in the solution if the total vapour pressure of the solution is $$475 \space torr$$.

In a gaseous mixture at $${20}^{o}C$$ the partial pressure of the components are
$${H}_{2}:150$$ Torr  $${CH}_{4}:300$$ Torr
$${CO}_{2}:200$$ Torr  $${C}_{2}{H}_{4}:100$$ Torr
Volume percent of $${H}_{2}$$ is:

A $$1.0\ g$$ sample of air consists of approximately $$0.76\ g$$ of nitrogen and $$0.24\ g$$ of oxygen. This sample occupies a $$1.0\ L$$ vessel at $$20^{o}C$$. Then:

The K.E of $$N$$ molecule of $$O_{2}$$ is $$xjoules$$ at__ $${123}^{o}C$$. Another sample of $$O_{2}$$ at $${327}^{o}C$$ has a K.E of $$2x$$ joules. The latter sample contains:

$$0.5\ \text{mole}$$ of each $$H_{2},SO_{2}$$ and $$CH_{4}$$ are kept in a container. A hole was made in the container. After 3 hours, decreasing order of partial pressures of gases in the container will be:

$$N_{2}$$ is found in a litre flask under $$100\ kPa$$ pressure and $$O_{2}$$ is found in another $$3$$ litre flask under $$320\ kPa$$ pressure. If the two flask are connected, the resultant pressure is:

The density of a gas $$A$$ is twice that of $$B$$. Molar mass of $$A$$ is half that of $$B$$. The ratio of partial pressure of $$A$$ to $$B$$ is:

A container is divided into two compartment. One compartment contains $$2$$ mole of $$N_{2}$$ gas at $$1$$ atm and $$300\ K$$ & other compartment contains $$H_{2}$$ gas at the same temperature and pressure. Volume of $$H_{2}$$ compartment is four times the volume of $$N_{2}$$ compartment. [assume no reaction under these condition]
If the container containing $$N_{2}$$ and $$H_{2}$$ are further heated to $$1000\ K$$ forming $$NH_{3}$$ with $$100\%$$ yield. Calculate the final total pressure.

A glass tube of volume $$112ml$$. containing a gas is partially evacuated till the pressure in it drops to $$3.8 \times 10^{-5}\ torr$$ at $$0^{o}C$$. The number of molecules of the gas remaining in the tube is?