Who experimented the relationship between pressure and volume by trapping gas inside a j-tube?

Every general-chemistry student learns of Robert Boyle (1627–1691) as the person who discovered that the volume of a gas decreases with increasing pressure and vice versa—the famous Boyle’s law. A leading scientist and intellectual of his day, he was a great proponent of the experimental method.

Born at Lismore Castle, Munster, Ireland, Boyle was the 14th child of the Earl of Cork. As a young man of means, he was tutored at home and on the Continent. He spent the later years of the English Civil Wars at Oxford, reading and experimenting with his assistants and colleagues. This group was committed to the New Philosophy, which valued observation and experiment at least as much as logical thinking in formulating accurate scientific understanding. At the time of the restoration of the British monarchy in 1660, Boyle played a key role in founding the Royal Society to nurture this new view of science.
 

Boyle’s Law

Although Boyle’s chief scientific interest was chemistry, 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, as displayed in a brilliant series of experiments in which he used an air pump to create a vacuum. The second edition of this work, published in 1662, delineated the quantitative relationship that Boyle derived from experimental values, later known as Boyle’s law: that the volume of a gas varies inversely with pressure.
 

Corpuscularism and Elements

Boyle was an advocate of corpuscularism, a form of atomism that was slowly displacing Aristotelian and Paracelsian views of the world. Instead of defining physical reality and analyzing change in terms of Aristotelian substance and form and the classical four elements of earth, air, fire, and water—or the three Paracelsian elements of salt, sulfur, and mercury—corpuscularism discussed reality and change in terms of particles and their motion.

Boyle believed that chemical experiments could demonstrate the truth of the corpuscularian philosophy. In this context he defined elements in Sceptical Chymist (1661) as “certain primitive and simple, or perfectly unmingled bodies; which not being made of any other bodies, or of one another, are the ingredients of which all those called perfectly mixt bodies are immediately compounded, and into which they are ultimately resolved.”

He was probably referring to the uniform corpuscles—which were as yet unobserved—out of which corpuscular aggregates were formed, not using elements as Antoine-Laurent Lavoisier and others used the term in the 18th century to refer to different substances that could not be broken down further by chemical methods. In his experiments Boyle made many important observations, including that of the weight gain by metals when they are heated to become calxes. He interpreted this phenomenon as caused by fiery particles that were able to pass through the walls of glass vessels.
 

Alchemical Interests

Boyle’s theories of material change did nothing to eliminate the possibility of the transmutation of base metals to gold that was at the heart of alchemy. Indeed he practiced alchemy until the end of his life, believed that he had witnessed transmutation, and successfully lobbied Parliament to repeal England’s ban on transmutation.

Boyle also wrote extensively on natural theology, advocating the notion that God created the universe according to definite laws.

The information contained in this biography was last updated on December 1, 2017.

 Nader Makarious

Boyle's Law

In 1662, Robert Boyle (British chemist 1627 - 1691) studied the relationship between the pressure and the volume of a gas at a constant temperature.

 Boyle observed that the product of the pressure and volume are observed to be nearly constant. The product of pressure and volume is exactly a constant for an ideal gas.

P X V = constant

For 2 different gases Boyle’s law formula

P1 X V1 = P2 X V2

P1, V1 (pressure and volume for the first gas).

P2, V2 (pressure and volume for the second gas).

Boyle’s experiment:

Robert Boyle used a sealed end J-shaped piece of glass tubing, a gas (air) was trapped in the sealed end of the tube and varying amounts of mercury were added to the J-shaped tube to vary the pressure of the system. Boyle systematically varied the pressure and measured the volume of the gas. These measurements were performed using a fixed amount of gas at constant temperature. In this way Boyle was able to examine the pressure-volume relationship without complications from other factors such as changes in temperature or amount of gas.

Volume of a fixed mass of gas at a constant temperature is inversely proportional to the pressure of the gas.

When volume increases, pressure decreases, and vise versa

 Graph the given data at http://webserver.lemoyne.edu/faculty/giunta/

And use the equation      PXV= constant will give the results as below:

 Conclusion

 Graph type shows an inverse proportional between pressure and volume, also by using the given data and applying them using Boyle’s equation   P X V = constant

we always get a constant, even though it’s not the exact same number and this occurred because we didn’t use an ideal gas here (A gas consider ideal when its particles has a negligible volume, with no intermolecular forces and its atoms or molecules undergo perfectly elastic collisions).