Advertisements
Advertisements
Question
State Henry's Law. What is the effect of temperature on the solubility of a gas in a liquid?
Advertisements
Solution
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
RELATED QUESTIONS
H2S, a toxic gas with rotten egg like smell, is used for the qualitative analysis. If the solubility of H2S in water at STP is 0.195 m, calculate Henry’s law constant.
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?
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.
A solution is prepared by dissolving 9.25 g of non-volatile solute in 450 mL of water. It has an osmotic pressure of 350 mm of Hg at 27°C. Assuming the solute is non-electrolyte, determine its molecular mass. (R = 0.0821 Lit-atm K−1 mol−1)
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.
The value of Henry's constant KH is ______.
Explain the solubility rule “like dissolves like” in terms of intermolecular forces that exist in solutions.
The solubility of a gas in water depends on ______
Explain the following phenomena with the help of Henry’s law.
Feeling of weakness and discomfort in breathing at high altitude.
Write the two applications of Henry’s law.
