Assertion: Andrews worked on a temporary gas (so called at that time) and derived the condition to liquefy the permanent gases (so called at that time).
Reason: Andrews studied isotherms of `CO_(2)` and obtained the required conditions of liquefaction of gas as `T gas lt Tc` (critical temperature).

A gas which obeys all the assumptions of kinetic theory of gases at all conditions of temperatures and pressures is called

The pressure of a gas is increased 2 times. What should be the change in its volume so that the temperature and number of moles remain constant?

The pressure of a gas is increased 2 times. What should be the change in its volume so that the temperature and number of moles remain constant?

Assertion : Different gases at the same conditions of temperature and pressure have same root mean square speed Reason : Average K.E. of a gas is directly proportional to temperature in kelvin

The pressure of gas is increased 2 times. What should be the change in its volume so that the temperature and number of moles remains constant ?

The pressure of gas is increased 2 times. What should be the change in its volume so that the temperature and number of moles remains constant ?

The essential conditions for liquefaction of gases were discovered by Andrews in 1869 as a result of his study of pressure-volume-temperature relationship for CO_(2) . It was found that above a certain temperature, it was impossible to liquefy a gas whatever the pressure was applied. The temperature below which the gas can be liquefied by the application of pressure alone is called critical temperature (Tc). The pressure required to liquefy a gas at this temperature is called the critical pressure (Pc). The volume occupied by one mole of the substance at the critical temperature and pressure is called critical volume. Critical constants are related with van der waals' constant as follows: V_( c) = 3b, P_( c) =a/(27b^(2)), T_( c) =(8a)/(27 Rb) The values of critical volumes of four gases A, B, C and D are 0.025L, 0.312L, 0.245L and 0.432L respectively. The gas with larger molecular diameter will be :

The essential conditions for liquefaction of gases were discovered by Andrews in 1869 as a result of his study of pressure-volume-temperature relationship for CO_(2) . It was found that above a certain temperature, it was impossible to liquefy a gas whatever the pressure was applied. The temperature below which the gas can be liquefied by the application of pressure alone is called critical temperature (Tc). The pressure required to liquefy a gas at this temperature is called the critical pressure (Pc). The volume occupied by one mole of the substance at the critical temperature and pressure is called critical volume. Critical constants are related with van der waals' constant as follows: V_( c) = 3b, P_( c) =a/(27b^(2)), T_( c) =(8a)/(27 Rb) The values of critical volumes of four gases A, B, C and D are 0.025L, 0.312L, 0.245L and 0.432L respectively. The gas with larger molecular diameter will be :