Using the kinetic theory derive an expression for the pressure exerted by an ideal gas, stating clearly the assumption which you make.

Derive an expression for pressure exterted by an ideal gas?

Obtain Graham's law of diffusion from the expression for the pressure exerted by a gas.

Name the device by which the pressure exerted by a gas can be measured.

Which of the following expressions is true for an ideal gas ?

The kinetic theory of gases gives the formula PV=1/3Nmv^(2) for the pressure P exerted by a gas enclosed in a volume V. The term Nm represents

Starting from the pressure exerted by a gas derive (i) Boyle's law (ii) Charle's law.

On the basis of the kinetic theory explain why the pressure of a gas at constant volume increases with rise in temperature?

A gas is filled in a cylinder fitted with piston at a constant temperature and pressure. Explain on the basis of kinetic theory : (i) The pressure of the gas increases by raising its temperature. (ii) On pulling the piston out, the pressure of the gas decreases. The pressure of an ideal gas filled in the bulb of a constant - volume gas thermomrter at 7^(@)C is 60 cm of mercury. What will be the pressure of the same volume of gas at 147^(@)C ?

van der Waal's equation for calculating the pressure of a non ideal gas is (P+(an^(2))/(V^(2)))(V-nb)=nRT van der Waal's suggested that the pressure exerted by an ideal gas , P_("ideal") , is related to the experiventally measured pressure, P_("ideal") by the equation P_("ideal")=underset("observed pressure")(underset(uarr)(P_("real")))+underset("currection term")(underset(uarr)((an^(2))/(V^(2)))) Constant 'a' is measure of intermolecular interaction between gaseous molecules that gives rise to nonideal behavior. It depends upon how frequently any two molecules approach each other closely. Another correction concerns the volume occupied by the gas molecules. In the ideal gas equation, V represents the volume of the container. However, each molecule does occupy a finite, although small, intrinsic volume, so the effective volume of the gas vecomes (V-nb), where n is the number of moles of the gas and b is a constant. The term nb represents the volume occupied by gas particles present in n moles of the gas . Having taken into account the corrections for pressure and volume, we can rewrite the ideal gas equation as follows : underset("corrected pressure")((P+(an^(2))/(V^(2))))underset("corrected volume")((V-nb))=nRT AT relatively high pressures, the van der Waals' equation of state reduces to

The molecular theory states that the pressure exerted by a gas in closed vessel results from the gas molecules striking against the walls of the vessel. How will the pressure change if : the volume is made half of its original value keeping the temperature constant?