An ideal monatomic gas is adiabatically compressed so that itsfinal temperature is twice its initial temperature. What is the ratio of the final pressure to itsinitial pressure?

When an ideal gas is compressed adiabatically and reversible, the final temperature is

5.6 liter of helium gas at STP is adiabatically compressed to 0.7 liter. Taking the initial temperature to be T_1, the work done in the process 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

If , at 50^@C and 75 cm of mercury prssure , a definite mass of a gas is compressed slowly, then what will be the final pressure and temperature of the gas in each case if the final volume is one - fourth of the initial volume ? (y = 1.5)

One mole of a gas at pressure 2 Pa and temperature 27 °C is heated till both pressure and volume are tripled. What is the temperature of the gas?

If 5 moles of oxygen at STP is adiabatically compressed so that temperature increases to 400^@C , then find the work done on the gas. R=8.3J/mole−K

At same temperature and pressure of an ideal gas

If , at 50^@C and 75 cm of mercury prssure , a definite mass of a gas is compressed suddenly, then what will be the final pressure and temperature of the gas in each case if the final volume is one - fourth of the initial volume ? (y = 1.5)

An ideal gas of volume 1.0L is adiabatically compressed to frac(1)15)th of its initial volume. Its initial pressure and temperature is 1.01xx10^5 Pa and 275^@C respectively. Given Cv for ideal gas = 20.8J/mol.K and gamma = 1.4. Calculate final temperature