Henry's law constant for CO2​ in water is 1.67×10^8 Pa at 298K. Calculate the quantity of CO2​ in 500 ml of soda water when packed under 2.5 atm CO2​ pressure at 298K.

If N2 gas is bubbled through water at 293 K, how many millimoles of N2 gas would dissolve in 1 litre of water. Assume that N­2 exerts a partial pressure of 0.987 bar. Given that Henry’s law constant for N2 at 293 K is 76.84 kbar.

The solubility of gas is related to its mole fraction in the aqueous solution. The mole fraction of the gas in the solution is calculated by applying Henry’s law. Thus,

As 1litre water contains 55.5 mol of it, therefore, if n represents number of moles of N₂ in solution,

Related Questions:

(1) The vapour pressure of ethanol and methanol are 44.5 mm and 88.7 mm Hg respectively. An ideal solution is formed at the same temperature by mixing 60 g of ethanol with 40g of methanol. Calculate total vapour pressure of the solution.

(2) What is the composition of the vapour which is in equilibrium at 30°C with a benzene-toluene solution with a mole fraction of benzene of 0.400?

The States of matter : Numerical Questions : Part-(2):

(1) The rms speed of an ideal gas at 27°C is 0.3 ms–1 . Its rms speed at 927°C (in ms–1) is

(2) The compressibility factor for 1 mole of a van der Waals gas at 0oC and 100 atm pressure is found to be 0.5. Assuming that the volume of a gas molecule is negligible, calculate the van der Waals constant, a.

(3) Two moles of ammonia gas are enclosed in a vessel of 5 litre capacity at 27oC. Calculate the pressure exerted by the gas, assuming that (i) the gas behaves like an ideal gas (using ideal gas equation). (ii) the gas behaves like a real gas (using van der Waal’s equation). Given that for ammonia, a = 4.17 atm litre2 mol–2 and b = 0.037 litre mol–1

(4) 1 mole of CCl4 vapours at 77oC occupies a volume of 35.0 L. If vander waal’s constants are a = 20.39 L 2 atm mol–2 and b = 0.1383 L mol–1, calculate compressibility factor Z under (a) low pressure region. (b) high pressure region.

(5) What is Vander waals equation of state of a real gas ?

(6) Calculate the mass of mercuryin a uniform column, 760 mm high and 1.00 cm2 in cross-sectional area. Is there any change in (a) mass and (b) pressure of column of same height but with 2.00 cm2 cross sectional area is taken ? (density of Hg = 13.6 g/cm3 )

(7) A sample of a given mass of a gas at a constant temperature occupies 95cm3 under a pressure of 9.962 × 104N/m2 .At the same temperature, it volume at a pressure of 10.13 × 104 N/m2 is :

(8) A gas occupied a volume of 250 ml at 700 mm Hg pressure and 25°C. What additional pressure is required to reduce the gas volume to its 4/5th value at the same temperature

(9) Volume of a cylinder containing 10 marbles and gas is 1 litre at 2 atm pressure. Now pressure on the cylinder is increased to 4 atm, at which volume becomes 725 ml. Calculate volume of each marble.the

(10) Why liquid have a definite volume but no definite shape?

The States of matter : Numerical Questions : Part-(1):

(1) What is Boyle's temperature ? and what is relation of Boyle's temperature with Vander waal's constant?

(2) A 10 cm column of air is trapped by a column of Hg, 8 cm long, in a capillary tube horizontally fixed as shown below, at 1 atm pressure. Calculate the length of air column when the tube is fixed at the same temperature 

(a) vertically with open end up

(b) vertically with open end down (c) At 45° from vertical, with open end up.

(3) What is payload of Balloon ?

(4) Calculate payload of a balloon having volume 100 litre. It is filled with helium gas at 0.2486 atm pressureand 300K. Density of air is 1.3 gm/litre and mass of material of balloon is 20 gm.

(5) A balloon of diameter 20 m weighs 100 kg. Calculate its paylod if it is filled with helium at 1.0 atm and 27 ∘ C. Density of air is 1.2 kg m −3 .(R=0.082 dm 3 atm K −^1 mol ^−1 ).

(6) What is Aqueous tension ?

(7) The diameters of a buble at the surface of a lake is 4 mm and at the bottom of the lake is 1 mm. If atmospheric pressure is 1 atm, what is the depth of the lake ? The density of lake-water and Hg are 1.0 gm/ml and 13.6 gm/ml, respectively. Assume that temperature of lake water is equal to that of atmosphere.Also neglect the contribution of pressure due to surface tension.

(8) Volume of a cylinder containing 10 marbles and gas is 1 litre at 2 atm pressure. Now pressure on the cylinder is increased to 4 atm, at which volume becomes 725 ml. Calculate volume of each marble.

(9) In a barometeric tube Hg is replaced by H2O then find the height of H2O column to measure the atmospheric pressure.Assume that vapour pressure of H2O in negligible.

(10) An open vessel at 27℃ is heated at constant pressure until 3/5th of the air in it has been expelled. Find 

(a) the temperature at which vessel was heated ? 

(b) the moles of air eascaped out, if vessel were heated to 900 K ?

(c) temperature at which half of the air escapes out ?

(11) When 3.2 g of sulphur is vapourised at 450°C and 723 mm pressure, the vapours occupy a volume of 780 ml. What is the molecular formula of sulphur vapours under these conditions?

(12) A spherical balloon of 21 cm diameter is to be filled up with hydrogen at 0℃ and 1 atm from a cylinder containing the gas at 20 atmosphere at 27℃. If the cylinder can hold 2.82 litre of water at 0℃ and 1 atm, calculate the number of balloon that can be filled up.

(13) The density of methane at 2.0 atmosphere pressure and 27°C is

(14) A mixture of CO and CO2 is found to have a density of 1.50 g/litre at 30℃ and 730 mm. The mole percent of CO in the mixture is

(15) A vessel of 2 lit. capacity contains hydrogen at 380 mm pressure at 27°C. 16 gm of O2 is added to the container at constant temperature, then find the final total pressure and final partial pressure of H2 . Sol. As partial pressure of a gas is independent from the pressure of other gas, initial as well as final partial pressue of H2 gas,

(16) 1 mole of N2 and 3 moles of H2 are mixed in 8.21 lit. container at 300 K to form NH3 . If at equilibrium, average molecular mass was found to be 34/3, then find partial pressure of each component.

(17) One litre flask contains air, water vapour and a small amount of liquid water at a pressure of 200 mmHg. If this is connected to another one-litre evacuated flask, what will be the final pressure of the gas mixture at equilibrium?Assume the temperature to be 50°C.Aqueous tension at 50°C = 93 mm Hg.

(18) A sample of butane gas C4H10 of unknown mass is contained in a vessel of unknown volume V at 25oC and a pressure of 760 mmHg. To this vessel 8.6787 g of neon gas is added in such a waythat no butane is lost from the vessel. The final pressure in the vessel is 1920 mm Hg at the same temperature. Calculate the volume of the vessel and the mass of butane.

(19) What are the difference between Diffusion and Effusion ?

(20) The rms speed of CO2 at a temperature T (in kelvin) is x cm s–^1.At what temperature (in kelvin) the rms speed of nitrous oxide would be 4x cm s^–1 ?

Gram Molecular Mass:

The molecular mass of a substance (Molecule) express in gram is called gram molecular mass of the substance.

OR

Mass of 6.022×10^23 molecules of a substance is define as gram molecular mass or GMM.

OR

Mass of one mole  of a molecule is called GMM.

For example for O2 molecule:

Molecular mass of O2 molecule = mass of one  OF molecule = 2 × mass of one "O" atom = 2× 16 amu = 32 amu

GMM= mass of 6.022×10^23 "O2" molecules =

32 amu × 6.022×10^23 "O2"  molecules.

GMM= 32  × 6.022×10^23 × 1.67 ×10 ^-24 gram

GMM = 32 amu

Note : (6.022×10^23 × 1.67 ×10 ^-24  =1)