The volume of an ideal diatomic gas with `gamma` = 1.5 is changed adiabatically from 16 litre to 12 litre. Find the ratio of the final and initial pressures and temperatures.

The volume of an ideal gas (gamma = 1.5 ) is changed adiabatically from 4.00 liters to 3.00 liters . Find the ratio of (a) the final pressure to the initial pressure and (b) the final temperature to the initial temperature.

The volume of an ideal gas (gamma = 1.5 ) is changed adiabatically from 4.00 liters to 3.00 liters . Find the ratio of (a) the final pressure to the initial pressure and (b) the final temperature to the initial temperature.

The volume of an ideal gas (gamma 1.5 ) is changed adiabatically from 4.00 liters to 3.00 liters . Find the ratio of (a) the final pressure to the initial pressure and (b) the final temperature to the initial temperature.

A gas for which gamma=1.5 is suddenly compressed to 1//4 th of the initial volume. Then the ratio of the final to initial pressure is

A gas for which gamma=1.5 is suddenly compressed to 1//4 th of the initial volume. Then the ratio of the final to initial pressure is

A gas for which gamma=1.5 is suddenly compressed to 1//4 th of the initial volume. Then the ratio of the final to initial pressure is

A gas for which gamma = 1.5 is suddenly compressed to 1/4 th of the initial volume. Then the ratio of the final to the initial pressure is

One mole of an ideal monoatomic gas expands reversibly and adiabatically from a volume of x litre to 14 litre at 27^(@) C. Then value of x will be [Given, final temperature 189 K and C_(V) = 3/2 R].

One mole of an ideal monoatomic gas expands reversibly and adiabatically from a volume of x litre to 14 litre at 27^(@) C. Then value of x will be [Given, final temperature 189 K and C_(V) = 3/2 R].