The volume of a gas is reduced adiabatically to `(1)/(4)` of its volume at `27^(@)C`, if the value of `gamma=1.4`, then the new temperature will be

An ideal gas at 27^(@)C is compressed adiabatically to 8//27 of its original volume. If gamma = 5//3 , then the rise in temperature is

The volume of a given mass of gas at NTP is compressed adiabatically to 1/5th of its original volume. What is the new pressure ? gamma =1.4.

A monoatomic gas is compressed adiabatically to 8/27 of its initial volume, if initial temperature is 27^° C, then increase in temperature

A monoatomic gas is compressed adiabatically to (1)/(4)^(th) of its original volume , the final pressure of gas in terms of initial pressure P is

A diatomic ideal gas is compressed adiabatically to 1/32 of its initial volume. If the initial temperature of the gas is T_i (in Kelvin) and the final temperature is a T_i , the value of a is

A diatomic ideal gas is compressed adiabatically to 1/32 of its initial volume. If the initial temperature of the gas is T_i (in Kelvin) and the final temperature is a T_i , the value of a is

A diatomic ideal gas is compressed adiabatically to 1/32 of its initial volume. If the initial temperature of the gas is T_i (in Kelvin) and the final temperature is aT_i , the value of a is

The volume of gas is reduced to half from its original volume. The specific heat will be

The volume of gas is reduced to half from its original volume. The specific heat will be

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].