Kara Sears
Henry's law, formulated in the 19th century by English chemist William Henry, describes the direct relationship between the solubility of a gas and the partial pressure of that gas above a liquid. The law is only applicable when the molecules of the system are in a state of equilibrium and does not apply to gases under extremely high pressure or when the gas and solution undergo a chemical reaction. While the law is useful for understanding the behaviour of gases, it does not apply to solids or liquids, as changes in pressure do not affect their solubility.
| Characteristics | Values |
|---|---|
| Applicability | Only applicable when the molecules are in a state of equilibrium |
| Applicability in relation to pressure | Does not hold true when gases are placed under extremely high pressure |
| Applicability in relation to chemical reactions | Does not apply when the gas and the solution participate in chemical reactions with each other |
| Applicability in relation to temperature | Does not apply to solids and liquids |
| Temperature dependency | Henry's law constants are highly dependent on temperature |
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What You'll Learn
- Henry's Law is specific to gases and does not apply to solids or liquids
- The law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid
- Henry's Law does not apply to gases at high pressures
- The law is only valid when the molecules in the system are in equilibrium
- The Henry's Law constant is highly temperature-dependent
Henry's Law is specific to gases and does not apply to solids or liquids
Henry's Law is a scientific principle that specifically applies to gases and the relationship between their solubility and the pressure exerted on them. It does not apply to solids or liquids. This law is expressed as the direct proportionality between the solubility of a gas and the pressure of that gas above a liquid. In other words, as the pressure exerted on a gas above a liquid increases, the gas is forced into the liquid, increasing its solubility.
It is important to note that Henry's Law is temperature-dependent, as vapour pressure and solubility are both influenced by temperature. The law is also only valid when the molecules in the system are in a state of equilibrium. When gases are under extremely high pressure, Henry's Law becomes inapplicable. This is because, at high pressures, certain gases can become very soluble and dangerous when introduced into the bloodstream.
Henry's Law has been demonstrated to apply to a wide range of solutes in the limit of infinite dilution, including non-volatile substances. In these cases, the law must be stated in terms of chemical potentials. For a solute in an ideal dilute solution, the chemical potential depends solely on the concentration. Additionally, Henry's Law is related to the concept of vapour pressure, which is the change of a liquid or solid into a vapour phase. This means that if a substance vapourises, it can enter the atmosphere.
While Henry's Law specifically pertains to gases, there are other laws that address similar concepts for solids and liquids. For instance, Raoult's Law, which is considered a special case of Henry's Law, applies to pairs of closely related substances, such as benzene and toluene, and holds true over the entire composition range. Furthermore, the Henry adsorption constant is relevant to solids, as it represents the ratio of the concentration of an adsorbate onto a solid concerning its partial pressure in the gas phase.
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The law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid
Henry's Law is a scientific principle that explains the relationship between the solubility of a gas and the pressure of that gas above a liquid. It states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above it. In other words, as the pressure of a gas above a liquid increases, the gas is forced into the liquid, increasing its solubility.
It's important to note that Henry's Law only applies to gases and not to solids or liquids. This is because the law is specifically concerned with the behaviour of gas molecules and how they interact with liquids under pressure. When the pressure above a liquid increases, more gas molecules are pushed into the liquid, where they become dissolved. This relationship between pressure and solubility is unique to gases and is not observed with solids or liquids, where changes in pressure do not affect solubility.
The law is expressed mathematically as: P = the partial pressure of the gas. The Henry's Law constant is highly temperature-dependent, as both vapour pressure and solubility vary with temperature. The Van 't Hoff equation is used to describe the temperature dependence of the Henry's Law constant. Additionally, Henry's Law only holds true when the molecules in the system are in a state of equilibrium. At extremely high pressures, the law becomes invalid, as the behaviour of gases under such conditions can be very different and dangerous.
Henry's Law has practical applications in various fields. For example, in diving, if the supersaturation is too great, bubbles may form and cause blockages in capillaries or distortion in solid tissues, resulting in decompression sickness. To avoid this, divers must ascend slowly to allow excess dissolved gas to be carried away by the blood and released into the lung. In environmental science, Henry's Law can be used to model the release of substances into the atmosphere, helping to understand the behaviour of contaminants and their impact on air and water quality.
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Henry's Law does not apply to gases at high pressures
Henry's Law, formulated by English chemist William Henry in 1803, is a gas law that states that the amount of dissolved gas in a liquid is directly proportional to its partial pressure above the liquid when the molecules of the system are in a state of equilibrium. The law is expressed as:
> 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.
The law is only valid when the molecules in the system are in equilibrium. Henry's Law constants are highly temperature-dependent because vapour pressure and solubility are both temperature-dependent. The law has been shown to apply to a wide range of solutes in the limit of infinite dilution. However, it is important to note that Henry's Law does not apply to gases at high pressures.
When gases are under extremely high pressure, Henry's Law is no longer applicable. For example, N2(g) at high pressure becomes very soluble and dangerous if introduced into the blood supply. This is because the solubility of gases increases with greater depth (and therefore greater pressure) according to Henry's Law. This can lead to a condition called hypoxia, where the concentration of O2 in the blood and tissues is so low that individuals feel weak and unable to think properly.
In summary, while Henry's Law provides valuable insights into the behaviour of gases at equilibrium, it has limitations and does not account for the behaviour of gases under high-pressure conditions.
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The law is only valid when the molecules in the system are in equilibrium
Henry's law, formulated by English chemist William Henry in 1803, is a gas law that states that the amount of dissolved gas in a liquid is directly proportional to its partial pressure above the liquid when the temperature is kept constant. In other words, the partial pressure of a gas in the vapour phase is directly proportional to the mole fraction of a gas in solution. The proportionality factor is called Henry's law constant.
Henry's law is only applicable when the molecules of the system are in a state of equilibrium. The law does not hold true when gases are placed under extremely high pressure. For instance, N2(g) at high pressure becomes very soluble and dangerous when introduced into the blood supply. This law also does not apply when the solution and gas are involved in a chemical reaction with each other.
The temperature dependence of equilibrium constants can be described with the Van 't Hoff equation, which also applies to Henry's law constants. Henry's law constant is highly temperature-dependent because vapour pressure and solubility are both temperature-dependent. The solubility of gases increases with greater depth (greater pressure) according to Henry's law, so the body tissues of a diver take on more gas over time in deeper waters.
An everyday example of Henry's law is carbonated soft drinks, which contain dissolved carbon dioxide. Before opening, the gas above the drink in its container is almost pure carbon dioxide, at a pressure higher than atmospheric pressure. When the bottle is opened, the pressurised CO2 escapes into the atmosphere. As the partial pressure of CO2 in the atmosphere above the drink rapidly decreases, the solubility of the carbon dioxide in the drink also decreases. If the drink is left open long enough, the concentration of carbon dioxide in the drink will reach an equilibrium with the concentration of carbon dioxide in the atmosphere, causing it to go flat.
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The Henry's Law constant is highly temperature-dependent
Henry's Law is a gas law formulated in the early 19th century by English chemist William Henry. It states that the amount of dissolved gas in a liquid is directly proportional to the partial pressure of that gas above the liquid when the temperature is kept constant. The constant of proportionality for this relationship is called the Henry's Law constant, often denoted by 'kH'.
The law is only valid when the molecules in the system are in a state of equilibrium. It does not apply when gases are under extremely high pressure or when the gas and solution undergo chemical reactions with each other.
An example of Henry's Law in action is the release of carbon dioxide from a carbonated drink when the bottle is opened. The gas above the unopened drink is usually pure carbon dioxide, kept at a pressure slightly above atmospheric pressure. As a result of Henry's Law, the solubility of carbon dioxide in the unopened drink is high. When the bottle is opened, the pressurised CO2 escapes, and as the partial pressure of CO2 decreases, the solubility of the carbon dioxide in the drink also decreases, causing the formation of bubbles.
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Frequently asked questions
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.
No, Henry's Law is specific to gases and does not apply to solids or liquids.
Henry's Law describes the relationship between the solubility of gases and the partial pressure of those gases above a liquid. Changes in pressure do not affect the solubility of solids.
Temperature affects the solubility of solids. As temperature increases, the solubility of solids also increases.
Henry's Law constants are highly dependent on temperature as both vapor pressure and solubility are temperature-dependent.
