# What is henry’s law constant

## What is Henry’s law constant k?

Henry’s law states that the concentration of a dissolved gas is directly proportional to the partial pressure of that gas above the solution: (18.12) where, KH is the Henry’s law constant, pa is the partial pressure of the gas, and [c] is the molar concentration of the gas or, (18.13)

## How do you find the Henry’s law constant?

L. mol-1 and C = 2*10-5 M into the Henry’s law formula: P = kH*C = (1.6*103 atm.

The value of the Henry’s law constant of a gas is dependent on the following factors:

1. The nature of the gas.
2. The nature of the solvent.
3. Temperature & pressure.

## What is Henry’s law and its application?

Mention some of its important applications. Answer: Henry’s law states that the solubility of a gas in a liquid is directly proportional to the pressure of the gas. … (iii) To avoid bends (painful effects during the decompression of scuba divers), oxygen diluted with less soluble helium gas is used by the sea divers.

## What is the difference between Henry’s law and Raoult’s Law?

As you can see for the example shown in the picture posted by the OP, Henry’s law describes the partial pressure of a component at very low concentration. On the other hand, Raoult’s law describes the pressure of a component at a concentration close to pure liquid.

## What is modification over Henry’s Law?

The concentration of a chemical species in a liquid solution is proportional to its gas- phase partial pressure. For molecules that form ions in solution, Henry’s law is modified to take account of the increased solubility as a function of pH. …

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## Why is Henry’s law important?

The main application of Henry’s law in respiratory physiology is to predict how gasses will dissolve in the alveoli and bloodstream during gas exchange. The amount of oxygen that dissolves into the bloodstream is directly proportional to the partial pressure of oxygen in alveolar air.

## What are the limitations of Henry’s Law?

Limitations of Henry’s law – definition

• The pressure should be low and the temperature should be high i.e the gas should behave like an ideal gas.
• The gas should not undergo compound formation with the solvent or association or dissociation in the solvent.

## Does Henry constant increase with temperature?

1, demonstrate that Henry’s constant at constant solvent volume increases monotonically with temperature, while the experimental Henry’s constant at the solvent saturation pressure goes through a maximum. The difference between the two plotted curves is the integral term of Eq.

## When can you use Henry’s Law?

Henry’s law works best at low concentration of the solute (close to 5% or less). Raoult’s law works best at non-low concentration of the solute ( 10−50% or so).