Advertisements
Advertisements
प्रश्न
State Henry's Law. What is the effect of temperature on the solubility of a gas in a liquid?
Advertisements
उत्तर
Henry's Law states that the solubility of a gas in a liquid is directly proportional to the pressure of the gas. If we use the mole fraction of a gas in the solution as a measure of its solubility, then it can be said that the mole fraction of gas in the solution is proportional to the partial pressure of the gas over the solution. The most commonly used form of Henry’s Law states that “the partial pressure of a gas in vapour phase (p) is directly proportional to the mole fraction of the gas (x) in the solution, i.e.
p ∝ x
p = KH x
where KH = Henry’s Law Constant
The solubility of gases is dependent on temperature. An increase in temperature results in a decrease in gas solubility in liquid, while a decrease in temperature results in an increase of gas solubility in liquid.
An increase in temperature causes an increase in kinetic energy, resulting in a more rapid motion of molecules, breaking intermolecular bonds which enable molecules to escape from the solution allowing the gases dissolved to evaporate more readily. Hence causing decrease in the solubility of gases in liquids.
APPEARS IN
संबंधित प्रश्न
Why do gases always tend to be less soluble in liquids as the temperature is raised?
The partial pressure of ethane over a solution containing 6.56 × 10−3 g of ethane is 1 bar. If the solution contains 5.00 × 10−2 g of ethane, then what shall be the partial pressure of the gas?
Write the name of gas released when Cu is added to the conc. HNO3
Henry’s law constant of oxygen is 1.4 × 10–3 mol lit–1 atm–1 at 298 K. How much of oxygen is dissolved in 100 ml at 298 K when the partial pressure of oxygen is 0.5 atm?
The value of Henry's constant KH is ______.
Which of the following factor(s) affect the solubility of a gaseous solute in the fixed volume of liquid solvent?
(a) nature of solute
(b) temperature
(c) pressure
(i) (a) and (c) at constant T
(ii) (a) and (b) at constant P
(iii) (b) and (c) only
(iv) (c) only
State Henry’s law and explain why are the tanks used by scuba divers filled with air diluted with helium (11.7% helium, 56.2% nitrogen and 32.1% oxygen)?
Assume that argon exerts a partial pressure of 6 bar. Calculate the solubility of argon gas in water. (Given Henry’s law constant for argon dissolved in water, KH = 40 k bar)
If O2 gas is bubbled through water at 303 K, the number of millimoles of O2 gas that dissolve in 1 litre of water is ______. (Nearest integer)
(Given: Henry's Law constant for O2 at 303 K is 46.82 k bar and partial pressure of O2 = 0.920 bar)
(Assume solubility of O2 in water is too small, nearly negligible)
Henry's constant (in k bar) for four gases α, β, γ and δ in water at 298 K is given below:
| α | β | γ | δ | |
| KH | 50 | 2 | 2 × 10-5 | 0.5 |
(density of water = 103 kg m-3 at 298 K)
This table implies that:
