Full Answer
What is the formula of Henry’s law?
The mathematical formula of Henry’s law is given by: P ∝ C (or) P = kH.C. Where, ‘P’ denotes the partial pressure of the gas in the atmosphere above the liquid. ‘C’ denotes the concentration of the dissolved gas. ‘k H ’ is the Henry’s law constant of the gas. This law was formulated in the early 19 th century by the English chemist William Henry.
What is Henry's Law of partial pressure?
In other words, the amount of dissolved gas is directly proportional to the partial pressure of its gas phase. The law contains a proportionality factor that is called Henry's law constant.
What is Henry's Law of solubility?
This law was proposed by William Henry in 103 and it is used for determining the quantity of gases dissolved in water and a second way to define is that the gas solubility in a liquid is proportional to the partial pressure of the gas above that liquid. Formula: The both ways to define this law can be expressed by the equation:
What are the factors that affect the value of Henry's Law constant?
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 write its formula?
Henry's law states that the solubility of a gas in a liquid is directly proportional to the pressure of the gas. And mole fraction (X) of the gas in a solution is proportional to the partial pressure (P) of the gas. P=KHX. Solve any question of Solutions with:- Patterns of problems.
What is Henry's law statement?
Henry's law, statement that the weight of a gas dissolved by a liquid is proportional to the pressure of the gas upon the liquid. The law, which was first formulated in 1803 by the English physician and chemist William Henry, holds only for dilute solutions and low gas pressures.
What is Henry's law example?
EXAMPLES. An everyday example of Henry's law is given by carbonated soft drinks. Before the bottle or can is opened, the gas above the drink is almost pure carbon dioxide at a pressure slightly higher than atmospheric pressure. The drink itself contains dissolved carbon dioxide.
What is unit of Henry's law?
What is the unit for Henry's law constant? Henry's law constant is expressed in mol L–1 bar–1.
What is Henry's law class 11th?
Henry's law states that at a constant temperature, the amount of gas particles dissolved in the liquid solution is directly proportional to the gas partial pressure which is above the liquid.
What is Henry's law in chemistry class 12?
Henry's law is one of the gas laws formulated by William Henry in 1803 and it states that at constant temperature the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid.
What is Henry's law and its application?
Henry law explains the solubility of a gas in a liquid solution by partial pressure and mole fraction of the gas in the liquid. Henry's Law states that “the partial pressure applied by any gas on a liquid surface is directly proportional to its mole fraction present in a liquid solvent.”
What is Henry's law of solubility?
The relationship of gas solubility to pressure is described by Henry's law, named after English chemist William Henry (1774-1836). Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.
What is Henry's law?
This article deals with Henry’s law formula. Henry’s law is a law that describes the behavior of a gas. This law states that the dissolved gas’s amount in a liquid is proportional to its partial pressure above the liquid. Furthermore, this proportionality factor is known as Henry’s law constant. English chemist William Henry was behind the formulation of this law. He came up with this law in the year 1803. Experts make use of this law for determining the quantity of gases dissolved in water.
What are some examples of Henry's law?
A good example where Henry’s law is at action is in the dissolution of oxygen and nitrogen that is depth-dependent in the blood of divers underwater. So when underwater, this dissolution changes during decompression, resulting in decompression sickness. Another good example can be the experience with carbonated soft drinks ...
What is the symbol for Henry's law constant?
Furthermore, the units are M or gas/L. The symbol k is a constant and is called as Henry’s law constant. Moreover, refers to the partial pressure of the gas.
Who came up with the law of dissolved gases?
English chemist William Henry was behind the formulation of this law. He came up with this law in the year 1803. Experts make use of this law for determining the quantity of gases dissolved in water.
Is Henry's law an approximation?
Henry’s law is only an approximation and is applicable for dilute solutions. Furthermore, the further the divergence of a system takes place from the ideal solutions, the lesser the accurateness of the calculation will be. Moreover, this law works best when the solvent and the solute are chemically similar. There is a lot of usage of Henry’s law in ...
What is Henry's law constant?
The Henry's law constants mentioned so far do not consider any chemical equilibria in the aqueous phase. This type is called the intrinsic, or physical, Henry's law constant. For example, the intrinsic Henry's law solubility constant of formaldehyde can be defined as
What is the effect of Henry's law constant on aqueous solutions?
Values of Henry's law constants for aqueous solutions depend on the composition of the solution, i.e., on its ionic strength and on dissolved organics. In general, the solubility of a gas decreases with increasing salinity (" salting out "). However, a " salting in " effect has also been observed, for example for the effective Henry's law constant of glyoxal. The effect can be described with the Sechenov equation, named after the Russian physiologist Ivan Sechenov (sometimes the German transliteration "Setschenow" of the Cyrillic name Се́ченов is used). There are many alternative ways to define the Sechenov equation, depending on how the aqueous-phase composition is described (based on concentration, molality, or molar fraction) and which variant of the Henry's law constant is used. Describing the solution in terms of molality is preferred because molality is invariant to temperature and to the addition of dry salt to the solution. Thus, the Sechenov equation can be written as
What is the relationship between equilibrium solubility and partial pressure?
Relation of equilibrium solubility of a gas in a liquid to its partial pressure in the contacting gas phase. In physical chemistry, Henry's law is a gas law that states that the amount of dissolved gas in a liquid is proportional to its partial pressure above the liquid. The proportionality factor is called Henry's law constant.
What is the concentration of a dilute solution?
For a dilute solution, the concentration of the solute is approximately proportional to its mole fraction x, and Henry's law can be written as
Which law states that the separation of gas particles one from another in the vapor phase bears the ratio of a?
Charles Coulston Gillispie states that John Dalton "supposed that the separation of gas particles one from another in the vapor phase bears the ratio of a small whole number to their interatomic distance in solution. Henry's law follows as a consequence if this ratio is a constant for each gas at a given temperature."
Does Henry's law apply to sucrose?
Henry's law has been shown to apply to a wide range of solutes in the limit of infinite dilution ( x → 0), including non-volatile substances such as sucrose. In these cases, it is necessary to state the law in terms of chemical potentials. For a solute in an ideal dilute solution, the chemical potential depends only on the concentration. For non-ideal solutions, the activity coefficients of the components must be taken into account:
What is Henry's law?
The law states that "At a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid." This law was proposed by William Henry in 103 and it is used for determining the quantity of gases dissolved in water and a second way to define is that the gas solubility in a liquid is proportional to the partial pressure of the gas above that liquid.
Who proposed the law of solubility?
This law was proposed by William Henry in 103 and it is used for determining the quantity of gases dissolved in water and a second way to define is that the gas solubility in a liquid is proportional to the partial pressure of the gas above that liquid.
Do gases at high pressure follow Henry's law?
Also, gases at a high pressure do not follow the Henry's law or if the solvent and solute reacts. Related Links: <a href="https://www.softschools.com/formulas/chemistry/henrys_law_equation_formula/562/">Henry's law equation (Henry's law) Formula </a>.
Problem 1
The Henry’s law constant for CO 2 is 3.34 × 10 –2 M atm –1 at 25 °C. What pressure (in atm) of CO 2 is needed to maintain a CO 2 concentration of 0.100 M in a can of lemon-lime soda? 1
Problem 2
What is the maximum concentration (in M) of CO 2 that can be dissolved in a can of lemon-lime soda if the maximum pressure that the can is able to withstand is 4.6 atm (at 25 °C)? k (CO 2) = 3.34 × 10 –2 M atm –1
Problem 4
At 20 °C, the concentration of O 2 in water with a partial pressure of 1 atm is 1.38 × 10 –3 M. What is the solubility (in M) of O 2 when the partial pressure is 0.204 atm? k (O 2) = 1.32 × 10 –3 M atm –1
How is Henry's law used?
For example, it is used to determine the amount of dissolved oxygen and nitrogen in the blood of divers to help determine the risk of decompression sickness (the bends).
What degree did William Henry have?
He holds bachelor's degrees in both physics and mathematics. our editorial process. Todd Helmenstine. Updated February 27, 2020. Henry's law is a gas law formulated by the British chemist William Henry in 1803.
What is the law of dissolved gas?
The law states that at a constant temperature, the amount of dissolved gas in a volume of a specified liquid is directly proportional to the partial pressure of the gas in equilibrium with the liquid. In other words, the amount of dissolved gas is directly proportional to the partial pressure of its gas phase. ...
Is Henry's law accurate?
Henry's law is only an approximation that is applicable for dilute solutions. The further a system diverges from ideal solutions ( as with any gas law ), the less accurate the calculation will be. In general, Henry's law works best when the solute and solvent are chemically similar to each other.
Is the amount of dissolved gas directly proportional to the partial pressure of its gas phase?
In other words, the amount of dissolved gas is directly proportional to the partial pressure of its gas phase. The law contains a proportionality factor that is called Henry's law constant. This example problem demonstrates how to use Henry's law to calculate the concentration of a gas in solution under pressure.
What is Henry Law?
Henry law explains the solubility of a gas in liquid solution by partial pressure and mole fraction of the gas in liquid.
When is Henry's law applicable?
Gas shouldn’t cause any chemical change in the solution. Henry’s law is appropriate only when pressure is not high, temperature is not too low and gas is extremely soluble.
What happens to solubility of gas in liquids if pressure is constant?
According to henry’s law, we have explained above that if pressure is constant, as the value of henry’s law constant increases, solubility of gas in liquid decreases. It can also be expressed as follow –
What happens to the solute in a solution when Henry's law constant decreases?
Mole fraction of the gas in liquid can be taken as solubility. Thus, as henry’s law constant decreases, solubility of the solute in solution increases.
Which law states that the partial pressure applied by any gas on a liquid surface is directly proportional to its mole?
Henry’s Law states that “the partial pressure applied by any gas on a liquid surface is directly proportional to its mole fraction present in liquid solvent.”.
When pressure remains constant, what is Henry's law?
When pressure remains constant, according to henry’s law henry constant will be inversely proportional to mole fraction of the gas. It can be represented as follows –
Why do different gases have different Henry's law constants in the solvent?
Nature of the gas. This is the reason different gases have different henry’s law constants in the solvent.
Table of Contents
Introduction
- This law was formulated in the early 19th century by the English chemist William Henry. It can be noted that the Henry’s law constant can be expressed in two different ways. If the constant is defined in terms of solubility/pressure, it is referred to as the Henry’s law solubility constant (denoted by ‘H’). On the other hand, if the proportionality constant is defined in terms of pressure…
Examples of Henry’s Law
- Pepsi and other Carbonated Drinks
Henry’s law comes into play every time a bottle of Pepsi (or any other carbonated drink) is opened. The gas above the unopened carbonated drink is usually pure carbon dioxide, kept at a pressure which is slightly above the standard atmospheric pressure. As a consequence of Henry… - Respiration and the Oxygenation of Blood
In the process of respiration, inhalation is accompanied by an increase in the partial pressure of oxygen in the alveoli. When deoxygenated blood interacts with the oxygen-rich air in the alveoli, the following gas-exchanges take place as a consequence of Henry’s law: 1. Since the partial pre…
Factors Affecting The Henry’s Law Constant
- 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 Therefore, different gases have different Henry’s laws constant in different solvents, as illustrated graphically below.
Limitations of Henry’s Law
- This law is only applicable when the molecules of the system are in a state of equilibrium.
- Henry’s law does not hold true when gases are placed under extremely high pressure.
- The law is not applicable when the gas and the solution participate in chemical reactions with each other.
Solved Examples
- Example 1
Calculate the solubility of gaseous oxygen in water at a temperature of 293 K when the partial pressure exerted by O2 is 1 bar. (Given: kH for O2 34840 bar.L.mol-1) As per Henry’s law, P = kH*C Substituting, kH = 34840 bar.L.mol-1and P = 1 bar, the equation becomes C = 1/34840 mol.L-1 = … - Example 2
The value of kH for carbon dioxide at a temperature of 293 K is 1.6*103 atm.L.mol-1. At what partial pressure would the gas have a solubility (in water) of 2*10-5M? Substituting the given values kH = 1.6*103 atm.L.mol-1 and C = 2*10-5M into the Henry’s law formula: P = kH*C = (1.6*…
Overview
In physical chemistry, Henry's law is a gas law that states that the amount of dissolved gas in a liquid is proportional to its partial pressure above the liquid. The proportionality factor is called Henry's law constant. It was formulated by the English chemist William Henry, who studied the topic in the early 19th century.
An example where Henry's law is at play is in the depth-dependent dissolution of oxygen and nitr…
Non-ideal solutions
Henry's law has been shown to apply to a wide range of solutes in the limit of infinite dilution (x → 0), including non-volatile substances such as sucrose. In these cases, it is necessary to state the law in terms of chemical potentials. For a solute in an ideal dilute solution, the chemical potential depends only on the concentration. For non-ideal solutions, the activity coefficients of the components must be taken into account:
History
In his 1803 publication about the quantity of gases absorbed by water, William Henry described the results of his experiments:
… water takes up, of gas condensed by one, two, or more additional atmospheres, a quantity which, ordinarily compressed, would be equal to twice, thrice, &c. the volume absorbed under the common pressure of the atmosphere.
Applications of Henry's law
In production of carbonated beverages Under high pressure, solubility of CO 2 increases. On opening the bottle to atmospheric pressure, solubility decreases and the gas bubbles are released from the liquid. For climbers or people living at high altitude Concentration of O 2 in the blood and tissues is so low that they feel weak and are unable to think properly, a condition called hypoxia. In underwater diving Gas is breathed at the ambient pressure which increases with depth due to …
Fundamental types and variants of Henry's law constants
There are many ways to define the proportionality constant of Henry's law, which can be subdivided into two fundamental types: One possibility is to put the aqueous phase into the numerator and the gaseous phase into the denominator ("aq/gas"). This results in the Henry's law solubility constant . Its value increases with increased solubility. Alternatively, numerator and denominator can be switched ("gas/aq"), which results in the Henry's law volatility constant . The …
Temperature dependence
When the temperature of a system changes, the Henry constant also changes. The temperature dependence of equilibrium constants can generally be described with the van 't Hoff equation, which also applies to Henry's law constants:
where is the enthalpy of dissolution. Note that the letter in the symbol refers to enthalpy and is not related to the letter for Henry's law constants. Integrating the above equation and creating an exp…
Effective Henry's law constants Heff
The Henry's law constants mentioned so far do not consider any chemical equilibria in the aqueous phase. This type is called the intrinsic, or physical, Henry's law constant. For example, the intrinsic Henry's law solubility constant of formaldehyde can be defined as
In aqueous solution, formaldehyde is almost completely hydrated:
The total concentration of dissolved formaldehyde is
Dependence on ionic strength (Sechenov equation)
Values of Henry's law constants for aqueous solutions depend on the composition of the solution, i.e., on its ionic strength and on dissolved organics. In general, the solubility of a gas decreases with increasing salinity ("salting out"). However, a "salting in" effect has also been observed, for example for the effective Henry's law constant of glyoxal. The effect can be described with the Sechenov equation, named after the Russian physiologist Ivan Sechenov (sometimes the Germa…