Chemistry Question Bank

The compressibility factor (Z) is defined as (a) real ideal V V (b) P Z nRT (c) ideal real V V (d) nRT Z PV

In Van der Waal’s equation of state for a non-ideal gas, the term that accounts for intermolecular forces is

The value of Van der Waal’s constant ‘a’ for the gases O2, N2, NH3 and CH4 are 1.360, 1.390, 4.170 and 2.253L2 atm mol–2 respectively. The gas which can most easily be liquified is

The term that corrects for the attractive forces present in a real gas in the van der Waals’ equation is

For one mole of a vander Waals’ gas when b = 0 and T = 300 K, the PV vs. 1/V plot is shown below. The value of the van der Waals’ constant a (atm L mol–2)

In van der Waals equation of state of the gas law, the constant ‘b’ is a measure of

The units of the van der Waal’s constant ‘b’ are

The units of the van der Waal’s constant ‘a’ are

Van der Waals constants ‘a’ and ‘b’ are related with..... respectively.

a and b are van der Waals constants for gases. Chlorine is more easily liquefied than ethane because

A gas will approach ideal behaviour at

In case of hydrogen and helium, the van der Waal’s forces are

Two separate bulbs contain ideal gases A and B. The density of gas A is twice that of gas B. The molecular mass of A is half that of gas B. The two gases are at the same temperature. The ratio of the pressure of A to …

Any gas shows maximum deviation from ideal gas at

For a gas deviation from ideal behaviour is maximum at :

The pressure of real gases is less than that of ideal gas because of

A gas is said to behave like an ideal gas when the relation PV/T = constant. When do you expect a real gas to behave like an ideal gas ?

The ratio of root mean square velocity to average velocity of a gas molecule at a particular temperature is

The average velocity of an ideal gas molecule at 27ºC is 0.3 m/s. The average velocity at 927º C will be

At constant volume, for a fixed number of moles of a gas the pressure of the gas increases with rise of temperature due to

The ratio between the root mean square speed of H2 at 50K and that of O2 at 800 K is

The r.m.s. velocity of hydrogen is 7 time the r.m.s. velocity of nitrogen. If T is the temperature of the gas,

The root mean square velocity of an ideal gas at constant pressure varies with density (d) as

For a monatomic gas kinetic energy = E. The relation with rms velocity is (a) 1/ 2 2E u m (b) 1 / 2 3E u 2m (c) 1 / 2 E u 2m (d) 1/ 2 E u 3m

Which one of the following statements is not true about the effect of an increase in temperature on the distribution of molecular speeds in a gas?