Gavin Howe
The gas laws are a group of laws that describe the behaviour of gases by outlining the relationships between volume, pressure, temperature, and the amount of gas. The basic gas laws were discovered by the end of the 18th century, with Boyle's Law, Charles' Law, and Avogadro's Law forming the three primary laws. These laws were formulated by Robert Boyle, Jacques Charles, and Amedeo Avogadro respectively.
| Characteristics | Values |
|---|---|
| Date of creation | Early 17th century |
| Number of primary laws | 3 |
| Names of primary laws | Charles' Law, Boyle's Law, Avogadro's Law |
| Names of scientists after whom the laws are named | Jacques Charles, Robert Boyle, Amedeo Avogadro |
| Combined form of the three primary laws | General Gas Equation, Ideal Gas Law |
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What You'll Learn
Boyle's Law
Robert Boyle was a 17th-century pioneer of modern chemistry, born in 1627 in Lismore Castle, Munster, Ireland. He was the 14th child of the Earl of Cork. As a young man, he was tutored at home and on the Continent. Later, he spent time at Oxford, where he read and experimented with colleagues and assistants, including Robert Hooke. Boyle was a founder of the Royal Society and was elected a Fellow of the Royal Society (FRS) in 1663.
Boyle's chief scientific interest was chemistry, and his first published scientific work, 'New Experiments Physico-Mechanicall, Touching the Spring of the Air, and Its Effects' (1660), concerned the physical nature of air. The second edition of this work, published in 1662, delineated the quantitative relationship that was later known as Boyle's Law: that the volume of a gas varies inversely with pressure.
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Charles' Law
Gas laws, created in the early 17th century, help scientists find volumes, amounts, pressures, and temperatures when dealing with matters of gas. Charles' Law, also known as the law of volumes, is an experimental gas law that describes how gases expand when heated. The law was named after scientist Jacques Charles, who formulated the original law in his unpublished work from the 1780s.
The French natural philosopher Joseph Louis Gay-Lussac confirmed the discovery in a presentation to the French National Institute on 31 January 1802, although he credited the discovery to Jacques Charles' unpublished work from the 1780s. Gay-Lussac worked with the vapours of volatile liquids in demonstrating Charles' Law and was aware that the law did not apply at low temperatures.
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Avogadro's Law
The gas laws were created in the early 17th century to help scientists determine the volume, amount, pressure, and temperature of gases. Avogadro's Law, one of the three fundamental gas laws, was formulated by Amedeo Avogadro, an Italian mathematical physicist and professor of higher physics at the University of Turin. Avogadro's Law, also known as Avogadro's hypothesis, states that under the same conditions of temperature and pressure, equal volumes of different gases contain an equal number of molecules. In other words, the volume of a gas is directly proportional to the number of moles of gas present when the temperature and pressure are held constant.
Avogadro first published his hypothesis in 1811, though some sources state it was in 1812. It reconciled Dalton's atomic theory with Joseph Louis Gay-Lussac's idea that some gases were composed of different fundamental substances (molecules) in integer proportions. Avogadro's Law is approximately valid for real gases at sufficiently low pressures and high temperatures. It is a specific case of the ideal gas law, which combines Boyle's Law, Charles's Law, and Avogadro's Law.
\ V = k \times n \: \: \: \text{and} \: \: \: \frac{V_1}{n_1} = \frac{V_2}{n_2}\nonumber \>
Where \(n\) is the number of moles of gas and \(k\) is a constant. This law is evident in everyday situations, such as blowing up a balloon. The volume of the balloon increases as you add more moles of gas by blowing into it. If the container holding the gas is rigid, pressure can be substituted for volume in Avogadro's Law.
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Gay-Lussac's Law
Mathematically, Gay-Lussac's Law can be expressed as:
> P ∝ T for gases of fixed mass kept at constant volume: P1/T1 = k (initial pressure/ initial temperature = constant) P2/T2 = k (final pressure/ final temperature = constant)
This law has important practical applications. For example, it explains why pressurised containers, such as aerosol cans, have warning labels instructing users to keep them away from fire and store them in a cool environment. When heated, the pressure exerted by the gases inside the container increases due to the rise in temperature, which can lead to an explosion. Similarly, in pressure cookers, heating increases the pressure exerted by the steam inside, causing the food to cook faster.
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Ideal Gas Law
The ideal gas law is a combination of several empirical gas laws, including Boyle's law, Charles's law, Avogadro's law, and Gay-Lussac's law. It was first stated by Benoît Paul Émile Clapeyron in 1834. The ideal gas law describes the behaviour of gases under different conditions of temperature, pressure, volume, and mass. Chemists use this law to explain and predict the behaviour of gases.
The ideal gas law is an equation of state that describes ideal gases and their behaviour. It is expressed as PV = nRT, where P is pressure, V is volume, T is temperature, n is the number of moles, and R is the universal gas constant. This equation assumes that the volume of gas particles is negligible compared to the volume of the container, that the gas particles have equal size and no intermolecular forces, and that the gas particles move randomly according to Newton's Laws of Motion.
The ideal gas law can also be written in terms of Avogadro's number as PV = NkT, where N is the total number of gas particles, and k is the Boltzmann constant. This version of the equation is useful when dealing with very small particles that cannot be counted individually.
The ideal gas law is a good approximation for most gases under moderate pressure and temperature. It is not a perfect representation of real gases, but it is a useful tool for understanding the relationships between pressure, volume, temperature, and the number of gas particles.
The development of the ideal gas law was made possible by the work of scientists such as Robert Boyle, Joseph Louis Gay-Lussac, and Amedeo Avogadro, who conducted experiments and made observations about the behaviour of gases. These scientists recognized the relationships between pressure, volume, temperature, and the number of gas molecules, which led to the development of the ideal gas law equation.
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