Advertisements
Advertisements
प्रश्न
What are ideal gases?
Advertisements
उत्तर
The kinetic theory of gases which is the basis for the gas equation (PV = nRT), assumes that the individual gas molecules occupy negligible volume when compared to the total volume of the gas and there is no attractive force between the gas molecules. Gases whose behaviour is consistent with these assumptions under all conditions are called ideal gases.
APPEARS IN
संबंधित प्रश्न
Solve the following.
A neon-dioxygen mixture contains 70.6 g dioxygen and 167.5g neon. If the pressure of the mixture of the gases in the cylinder is 25 bar. What is the partial pressure of dioxygen and neon in the mixture?
Solve the following.
Calculate the volume of 1 mole of a gas at exactly 20°C at a pressure of 101.35 kPa.
A bottle of ammonia and a bottle of HCl connected through a long tube are opened simultaneously at both ends. The white ammonium chloride ring first formed will be
At identical temperature and pressure, the rate of diffusion of hydrogen gas is `3sqrt3` times that of a hydrocarbon having molecular formula CnH2n–2. What is the value of n?
A tank contains a mixture of 52.5 g of oxygen and 65.1 g of CO2 at 300 K the total pressure in the tanks is 9.21 atm. Calculate the partial pressure (in atm.) of each gas in the mixture.
What mass of an oxygen gas will occupy 8.21 L of volume at 1 atm pressure and 400 K temperature?
Which of the following graphs is not correct for ideal gas?
If 10−4 dm3 of water is introduced into a 1 dm3 flask at 300 K, how many moles of water are in the vapour phase when equilibrium is established?
(Given: Vapour pressure of H2O at 300 K is 3170 Pa; R = 8.314 JK−1 mol−1)
According to Boyle's Law, at constant temperature, the pressure of a gas is ______.
An oxygen cylinder of volume 30 litres has 18.20 moles of oxygen. After some oxygen is withdrawn from the cylinder, its gauge pressure drops to 11 atmospheric pressure at temperature 27°C. The mass of the oxygen withdrawn from the cylinder is nearly equal to:
[Given: R = `100/12`Jmol−1 K−1,and molecular mass of 12 O2 = 32, 1 atm pressure = 1.01 × 105 N/m]
