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प्रश्न
Write the two applications of Henry’s law.
Mention some important applications of Henry’s law.
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उत्तर
- To increase the solubility of CO2 in soft drinks and soda water, the bottle is sealed under high pressure.
- Aquatic species feel uncomfortable in hot water.
- Scuba divers must cope with high concentrations of dissolved gases while breathing high-pressure air underwater. Increased pressure increases the solubility of atmospheric gases in blood. When the divers come towards the surface, the pressure gradually decreases. This releases dissolved gases, leading to the formation of nitrogen bubbles in the blood. This blocks capillaries and causes a medical condition known as the bends, which is painful and life-threatening. To avoid bends and the toxic effects of high concentrations of nitrogen in the blood, the tanks used by scuba divers are filled with air diluted with helium (11.7% helium, 56.2% nitrogen, and 32.1% oxygen).
- At high altitudes, the partial pressure of oxygen is less than that at the ground level. This leads to low oxygen concentrations in the blood and tissues of people living at high altitudes or of climbers. Low blood oxygen causes climbers to become weak and unable to think clearly, symptoms of a condition known as anoxia.
- The way that oxygen reaches tissues is explained by Henry’s law. Because of the high partial pressure of oxygen in the lungs, when air is inhaled, it combines with the blood’s haemoglobin to generate oxyhaemoglobin. In tissues, the partial pressure of oxygen is low. As a result, oxyhaemoglobin releases oxygen, which the cells use.
Notes
Students should refer to the answer according to their questions.
संबंधित प्रश्न
Explain, why do aquatic animals prefer to stay at lower level of water during summer?
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?
Henry’s law constant for the molality of methane in benzene at 298 K is 4.27 × 105 mm Hg. Calculate the solubility of methane in benzene at 298 K under 760 mm Hg.
The air is a mixture of a number of gases. The major components are oxygen and nitrogen with approximate proportion of 20% is to 79% by volume at 298 K. The water is in equilibrium with air at a pressure of 10 atm. At 298 K if the Henry’s law constants for oxygen and nitrogen are 3.30 × 107 mm and 6.51 × 107 mm respectively, calculate the composition of these gases in water.
Which mixture is used for respiration by deep sea divers?
(A) He + O2
(B) Ne + O2
(C) Ar + O2
(D) Kr + O2
Give reasons for the following :
Aquatic animals are more comfortable in the cold water than in warm water.
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
State Henry’s law.
Which law shows relation between pressure and solubility of a gas in solvent?
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?
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
Solubility of gases in liquids decreases with rise in temperature because dissolution is an ______.
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 |
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)
In which of the following solvents, the \[\ce{C4H8NH3+X–}\] is soluble?
Assertion (A): Helium is used to dilute oxygen in diving apparatus.
Reason (R): Helium has high solubility in O.
In the light of the above statements, choose the correct answer from the options given below:
