Calculate the final pressure when 2 molesof He at N..T.P. is compressed to 10 lit. Given `gamma=1.61`

The initial volume of a gas is 2m^(3) . When the gas is compressed adiabatically at a pressure of 4 xx 10^(5) N cdot m^(-2) , its volume become 0.5 m^(3) . What will be the final pressure of the gas? If it is compressed isothermally, what will be the final pressure? Calculate the work done on the gas in both cases (gamma = 1.4) .

Calculate the pressure exerted by 5 moles of CO_2 in one litre vessel at 47^@ C using Vanderwaal's equation. Also report the pressure of gas if it behaves ideally in nature. Given that a=3.592 atm lit^2 mol^(-2) . b = 0.0427 lit mol^(-1)

Calculate the mass of 2.24 liter C0_2 at N.T.P

Calculate the osmotic pressure of a 10%. Solution of glucose at 18^@C . R = 0.082 lit atm K^-1 mol^-1 .

Calculate the partial pressures of O_2 and H_2 in a mixture of 3 moles of O_2 and 1 mole of H_2 at S.T.P.

Calculate the pressure required to compress a gas adiabatically at atmospheric pressure to one third of its volume. Given gamma = 1.47 .

Find the. final temperature when under same pressure a gas expands from 750 cc to 1 lit. Initial temperature is -30^@C

The initial volume of a gas is 1 L and the pressure is 16 atm. Due to adiabatic expansion, the final pressure of the gas becomes 2 atm. Find out the final volume of the gas [gamma = 3/2] .

Calculate the work done when 56 gm N_2 gas (ideal) at 28^@C expands from 10 atm pressure to 2 atm pressure.