In a vessel, whose volume is `1l`, there is a gas, which is a compound of oxygen and nitrogen. Mass of gas is 1g, gas's temperature is `17_(0)C` and pressure of the gas is `31.7 k P.a`. Determine the chemical formula of compound of `(R=8.31 J//mol -K)`:-

The kinetic energy of one gram molecule of a gas at normal temperature and pressure is (R=8.31J//mol-K)

Three moles of an ideal gas kept at a constant temperature of 300 K are compressed from a volume of 4 litre to 1 litre. Calculate the work done in the process. (R = 8.31 J mol^-1 K^-1 )

At a given temperature and pressure, the volume of 1 mol of an ideal gas is 10 L. at the same temperature and pressure, the volume of 1 mol of a real gas is VL. At this temperature and pressure, if the compressibility factor of the real gas is greater than 1, then -

It temperature of 5 moles of a gas is raised through 100^(@)C at constant pressure, then external work done by the gas will be (R=8.32 J/mol K)

The K.E. of one mole of a gas at normal temperature and perssure is (R=8.31 J mol^(-1)K^(-1)) ........... .

10 mol of an ideal gas is taken through an isothermal process in which the volume is compressed from 40 L to 30 L. If the temperature and the pressure of the gas are 0^(@)C and 1 atm respectively. Find the work done in the process. Given: R = 8.31 J cdot mol^(-1) cdot K^(-1) .

What mass of an oxygen gas will occupy 8.21 L of volume at 1 atm pressure and 200 K temperature ?

What mass of an oxygen gas will occupy 8.21 L of volume at 1 atm pressure and 200 K temperature ?