States of Matte...

1 mole of chlorine and 1 mole of hydrogen were taken in a 10 L evacuated flask along with a little charcoal. The flask was then irradiated with light until the reaction was complete. Subsequently, 5L of water was introduced into the flask and the flask was cooled to $$27^{o}C$$. The pressure exerted by the system is approximately equal to: 

According to the kinetic theory of gases, in an ideal gas, between two successive collisions, a gas molecule travels:

Calculate the volume of $$CO_{2}$$ evolved by the combustion of $$50$$ ml of a mixture containing $$40$$ per $$C_{2}H_{4}$$ and $$60$$ per $$CH_{4}$$ (by volume).

$$45.4$$ L of dinitrogen reacted with $$22.7$$ L of dioxygen and $$45.4$$ L of nitrous oxide was formed. The reaction is given below:
$$\displaystyle 2N_{2}\left ( g \right )+O_{2}\left ( g \right )\rightarrow 2N_{2}O\left ( g \right )$$
Which law is being obeyed in this experiment?

Two identical vessels are filled with 44 g of hydrogen and 44 g of carbon dioxide at the same temperature. If pressure of $$CO_2$$ is 2 atm. Find the pressure of hydrogen.

A 600 $$ml$$ vessel containing oxygen at 800 $$mm$$ and a 400 $$ml$$ vessel containing nitrogen at 600 $$mm$$ at the same temperature are joined to each other. The final pressure of the mixture is:

A balloon of diameter $$21\:meter$$ weight $$100 kg$$. Calculate its pay-load, if it is filled with $$He$$ at $$1.0\: atm$$ and $$27 ^\circ C$$. Density of air is $$1.2\: kg m^{-3}$$. (Given: $$R = 0.082\: L\: atm\: K^{-1} mol^{-1}$$)

Correct expression for density of an ideal gas mixture of two gases 1 and 2, where $$m_{1}$$ and $$m_{2}$$ are masses and $$n_{1}$$ and $$n_{2}$$ are moles and $$M_{1}$$ and $$M_{2}$$ are molar masses.

For any gas, the mean free path at a particular pressure :