The temperature of a hypothetical gas increases to `sqrt(2)` times when compressed adiabatically to half the volume. Its equation can be written as

A gas is compressed adiabatically to half its volume. By what factor does the pressure of the gas increase?

A diatomic gas at pressure P, compressed adiabatically to half of its volume, what is the final pressure-

At normal temperature, one mole of diatomic gas is compressed adiabatically to half of its volume. Where, gamma = 1.41. The final temperature of the gas will be

A gas at 10^(@)C temperature and 1.013xx 10^(5) Pa pressure is compressed adiabatically to half of its volume. If the ratio of specific heats of the gas is 1.4, what is its final temperature?

When a gas is compressed adiabatically and reversibly, the final temperature is -

A volume of gas at atmospheric pressure is compressed adiabatically to half its original volume. Calculate the resulting pressure (gamma = 1.4)

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

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