Advertisements
Advertisements
Question
Explain the following phenomena with the help of Henry’s law.
Painful condition known as bends.
Advertisements
Solution
To Henry's law pressure of a gas is directly proportional to solubility. Scuba divers when coming towards surface the air pressure gradually decreases. This reduced pressure releases the dissolved gases present in blood and leads to the formation of bubbles of nitrogen in the blood. These blocks capillaries and creates a medical condition known as bends, which is painful and dangerous to live.
APPEARS IN
RELATED QUESTIONS
What is the effect of temperature on solubility of a gas in a liquid?
Explain, why do aquatic animals prefer to stay at lower level of water during summer?
Gas (A) is more soluble in water than Gas (B) at the same temperature. Which one of the two gases will have the higher value of KH (Henry’s constant) and why
Why do gases always tend to be less soluble in liquids as the temperature is raised?
Henry’s law constant for CO2 in water is 1.67 × 108 Pa at 298 K. Calculate the quantity of CO2 in 500 mL of soda water when packed under 2.5 atm CO2 pressure at 298 K.
Give reasons for the following :
Aquatic animals are more comfortable in the cold water than in warm water.
The solubility product of PbCl2 at 298K is 1.7 × 10-5. Calculate the solubility of PbCl2 in g/lit. at 298K.
Atomic Weights: [Pb = 207 and Cl = 35.5]
Write the name of gas released when Cu is added to dilute HNO3
Write the name of gas released when Cu is added to the conc. HNO3
The statement “If 0.003 moles of a gas are dissolved in 900 g of water under a pressure of 1 atmosphere, 0.006 moles will be dissolved under a pressure of 2 atmospheres”, illustrates.
According to Henry’s law, the amount of gas that will dissolve in blood plasma or any other liquid is determined by which of these factors?
The value of Henry's constant KH is ______.
Solubility of gases in liquids decreases with rise in temperature because dissolution is an ______.
KH value for \[\ce{Ar(g)}\], \[\ce{CO2(g)}\], \[\ce{HCHO (g)}\] and \[\ce{CH4(g)}\] are 40.39, 1.67, 1.83 × 10–5 and 0.413 respectively. Arrange these gases in the order of their increasing solubility.
Match the items given in Column I with the type of solutions given in Column II.
| Column I | Column II |
| (i) Soda water | (a) A solution of gas in solid |
| (ii) Sugar solution | (b) A solution of gas in gas |
| (iii) German silver | (c) A solution of solid in liquid |
| (iv) Air | (d) A solution of solid in solid |
| (v) Hydrogen gas in palladium | (e) A solution of gas in liquid |
| (f) A solution of liquid in solid |
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:
In which of the following solvents, the \[\ce{C4H8NH3+X–}\] is soluble?
Write the two applications of Henry’s law.
