Show that the volume of 1 gram-molecule of any gas at 273K temperature and 1 atm pressure is 22.4 L.

Calculate the volume of 3.6g of water vapour at 273K temperature and 1 atm pressure.

What are the molar volumes of nitrogen and argon gases at 273.15 K temperature and 1 atm pressure? [consider both the gases behave ideally].

The number of molecules 67.2 L of a gas at 0^@C and 1 atm pressure is:

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 -

At 273 K and 76 cm pressure, the volume of 0.64 g of any gas is 224 mL. At what temperature 1 g of that gas at 1 atm pressure will occupy a volume of 1 litre?

At a given temperature and pressure, 1 mol of an ideal gas occupies a volum eof 20.8 L for 1 mol of a real gas at the same temperature and pressure- (i) Z will be equal to 1 if the volume of the real gas is (ii) Z will be greater than 1 if the volume of the real gas is (iii) Z will be less than 1 if the volume of the real gas is.

What will be the signs of DeltaG for melting of ice at 267 K and 276K temperature and 1 atm pressure?

Prove that at STP the molar volume of any gas is 22.4 lit.

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) .

The molar specific heat of an ideal gas at constant pressure is C_(p) = 5/2 R . Some amount of this gas in a closed container has a volume 0.0083 m^(3) , a temperature 300 K and a pressure 1.6 xx 10^(6) N cdot m^(-2) . If 2.49 xx 10^(4) J 1 of heat is supplied at a constant volume of the gas, find out the final temperature and pressure. Given, R = 8.3 J cdot mol^(-1) cdot K^(-1) .