What makes it true? We can briefly refer to ideas from kinetic-molecular theory (KMT), which Boyle did not have access to in the 1600s. KMT was developed into its modern form about 200 years after Boyle. The initial and final volumes and pressures of the fixed quantity of gas, to which the initial and final temperatures are equal (heating or cooling is necessary to satisfy this condition), are related by the equation: PV = k, by the way, is Boyle`s law, not the one above. The above is only an equation derived from Boyles` law. This law was the first physical law expressed in the form of an equation describing the dependence of two variable quantities.  The debate between proponents of energetics and atomism prompted Boltzmann to write a book in 1898, which was criticized until his suicide in 1906.  Albert Einstein showed in 1905 how kinetic theory can be applied to the Brownian motion of a fluid suspended particle, which was confirmed by Jean Perrin in 1908.  Boyle (and Mariotte) derived the law solely through experiments. The law can also be derived theoretically, based on the presumed existence of atoms and molecules and hypotheses about perfectly elastic motion and collisions (see kinetic theory of gases).
However, these hypotheses met with enormous resistance in the positivist scientific community of the time, as they were considered purely theoretical constructs for which there was not the slightest observational evidence. Note that mmHg units are cancelled. X is a symbol of unknown and technically carries no unit. So don`t write x L for x liters. Just keep checking that you are using the correct equation and that you have all the correct values and units. Don`t put unity on the unknown. And do the left side on the calculator, then divide by V4 (this is the value 382.0) This relationship between pressure and volume was first established by Richard Towneley and Henry Power in the 17th century.   Robert Boyle confirmed their discovery through experiments and published the results.  According to Robert Gunther and other authorities, it was Boyle`s assistant, Robert Hooke, who built the experimental apparatus. Boyle`s law is based on experiments with air, which he considered to be a liquid of particles resting between small, invisible sources. At the time, tune was still considered one of the four elements, but Boyle disagreed.
Boyle`s interest was probably to understand air as an essential element of life;  He has published work on the growth of airless plants.  Boyle used a closed J-shaped tube, and after pouring mercury on one side, he forced the air on the other side to contract under the pressure of mercury. After repeating the experiment several times and using varying amounts of mercury, he found that under controlled conditions, the pressure of a gas is inversely proportional to the volume it occupies.  The French physicist Edme Mariotte (1620-1684) discovered the same law independently of Boyle in 1679, but Boyle had already published it in 1662.  However, Mariotte discovered that the volume of air changes with temperature.  Therefore, this law is sometimes referred to as the Mariotte law or the Boyle-Mariotte law. Later, in 1687, in the Philosophiæ Naturalis Principia Mathematica, Newton showed mathematically that in an elastic fluid composed of stationary particles between which the repulsive forces are inversely proportional to their distance, the density would be directly proportional to the pressure, but this mathematical treatise is not the physical explanation of the observed relationship. Instead of a static theory, a kinetic theory is needed, provided two centuries later by Maxwell and Boltzmann.
This equation shows that as the volume increases, the gas pressure decreases proportionately. Similarly, as the volume decreases, the gas pressure increases. The law was named after chemist and physicist Robert Boyle, who published the original law in 1662.  Boyle`s Law is often used to explain how the respiratory system works in the human body. This often involves explaining how lung volume can be increased or decreased, causing relatively lower or higher air pressure (in accordance with Boyle`s Law). This forms a pressure difference between the air in the lungs and the ambient air pressure, which in turn triggers inhalation or exhalation as the air changes from high to low pressure.  3) Multiply the left side and divide (by 760.0 mmHg) to solve for x. Here, P1 and V1 represent the original print and volume, respectively, and P2 and V2 represent the second print and volume, respectively. Boyle`s law, also known as Boyle–Mariotte`s law or Mariotte`s law (especially in France), is an experimental gas law that describes how the pressure of a gas decreases with increasing container volume. A modern statement of Boyles` law is: Daniel Bernoulli (1737-1738) derived Boyle`s law by applying Newton`s laws of motion at the molecular level.
It remained ignored until about 1845, when John Waterston published a paper constructing the great principles of kinetic theory; this was rejected by the Royal Society of England. Later work by James Prescott Joule, Rudolf Clausius and especially Ludwig Boltzmann established the kinetic theory of gases and drew attention to the two theories of Bernoulli and Waterston.  The absolute pressure exerted by a given mass of an ideal gas is inversely proportional to the volume it occupies if the temperature and the quantity of gas remain unchanged in a closed system.   Now, when the volume is changed to a new value called V2, the pressure spontaneously changes to P2. This happens because the PV product must always be the same k. The PV product cannot simply be changed to an old value, it MUST go to k. (If the temperature and quantity remain the same.) Discovered by Robert Boyle in 1662. On the European continent, this law is attributed to Edme Mariotte, so these countries tend to call this law by its name. However, Mariotte did not publish his work until 1676. Personally, I think this attempt to confuse the problems is due to the fact that more or less all the problems of Boyle`s law are the same.
So people found a little more spices to spice up the sauce, so to speak. Most gases behave like ideal gases at moderate pressures and temperatures. The technology of the 17th century could not produce very high pressures or very low temperatures. Therefore, it was unlikely that there were any discrepancies in the legislation at the time of publication. As technological improvements have allowed for higher pressures and lower temperatures, deviations from the ideal behavior of the gas have become noticeable, and the relationship between pressure and volume can only be accurately described using the theory of real gas.  The difference is expressed as a compressibility factor.