A certain mass of gas is expanded from (1L,10 atm) to (4L,5 atm) against a constant external pressure of 1 atm. If the initial temperature of the gas is 300 K and the heat capacity of the process is 50 J/∘C. Then the enthalpy change during the process is: (1L atm≃100 J).

The equation of state for a gas is P(V−nb)=nRT, where b and R are constants. If the pressure and temperature are such that V m​ =10b, what is the compressibility factor of gas in this condition?

A 10 liter container consist of 1 mole of gas at 300 K. It is connected to another container having volume 40 liter and is initially at 300 K. The nozzle connecting two containers is opened for a long time and once the movement of gas stopped, the larger container was heated to a temperature of 600 K. Calculate

(A) Moles and pressure of gas in both the containers before heating. (B) Moles and pressure in two containers after heating. Assume that initially the larger container is completely evacuated.

1 ml of gaseous aliphatic compound CnH3nOm is completely burnt in an excess of O2 and cooled to room temperature. The contraction in volume is

A mixture of ethane (C2H6) and ethene (C2H4) occupies 40 litre at 1.00 atm and 400 K , the mixture reacts completely with 130 gm of O2 to produce CO2 and H2O . Assuming ideal gas behaviour , calculate the mole fraction of ethane (C2H6) and ethene (C2H4) in mixture. (R= 0.0821 atm L par mole par kelvin) (IIT 1915)