Anaya Nolan
Boyle's Law, discovered by Robert Boyle in 1662, describes the behaviour of an ideal gas and the relationship between its pressure and volume. The law states that the pressure exerted by a gas is inversely proportional to its volume, provided the temperature and mass of the gas remain constant. This law can be applied to various scenarios, such as changes in pressure and volume when a balloon is inflated or squeezed, or when a scuba diver rapidly ascends from a deep zone towards the water surface. In calculations involving Boyle's Law, it is essential to ensure that consistent units are used for pressure and volume, such as mm Hg (millimetres of mercury) or atm (atmospheres). For example, if a sample of gas has an initial volume of 12.0 litres at a pressure of 1.00 atm, and the pressure is increased to 1000 mm Hg, we can use Boyle's Law to calculate the new volume of the gas.
| Characteristics | Values |
|---|---|
| Other Names | Mariotte's law, Boyle-Mariotte law |
| Year of Discovery | 1662 |
| Discovered By | Robert Boyle, Edme Mariotte |
| Equation | PV = k |
| Formula | V2 = p1 × V1 / p2 |
| Units | mmHg, atm |
| Process | Isobaric, isochoric, isothermal |
| Curve | Hyperbola |
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What You'll Learn
Boyle's Law, also known as Boyle-Mariotte Law
Boyle's Law, also known as the Boyle-Mariotte Law, was discovered by Robert Boyle in 1662. On the continent of Europe, this law is sometimes attributed to Edme Mariotte, who discovered it independently in 1679, after Boyle had published his work. Mariotte did not publish his findings until 1676.
Boyle's Law is an empirical gas law that describes the relationship between the pressure and volume of a confined gas at a constant temperature and mass of gas. It is based on experiments with air, which Boyle considered to be a fluid of particles at rest between small invisible springs.
The law states that the pressure and volume of a gas are inversely proportional. This means that as the volume of a gas increases, the pressure it exerts decreases, and vice versa. This relationship can be expressed mathematically as an equation, which was the first of its kind to describe the dependence of two variable quantities.
Boyle's Law can be applied to calculations involving different pressure units, such as atm and mmHg. However, it is important to ensure that the units are converted to the same unit before performing the calculation. For example, if a problem provides the pressure in mmHg, but the answer is required in atm, the mmHg value must first be converted to atm.
Boyle's Law is a fundamental concept in gas laws and has been further developed and supported by other scientists, such as Daniel Bernoulli, Rudolf Clausius, Maxwell, and Boltzmann.
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Pressure and volume are inversely proportional
Boyle's Law is a basic law in chemistry that describes the behaviour of a gas held at a constant temperature. It states that when the temperature is fixed, the volume of a gas is inversely proportional to the pressure exerted by the gas. In other words, when a gas is pumped into an enclosed space, it will adjust to fit the volume of that space, and the pressure it exerts on the container will increase.
Mathematically, Boyle's Law can be written as pV=k, where p is the pressure of the gas, V is the volume of the gas, and k is a constant. An example of Boyle's Law in action is inflating a balloon. When air is blown into a balloon, the pressure of that air pushes on the rubber, causing the balloon to expand. If one end of the balloon is squeezed, the volume decreases, and the pressure inside increases, causing the other end of the balloon to expand outwards.
Boyle's Law problems often involve different units of pressure, such as atm and mmHg. In such cases, it is necessary to convert one unit to the other before performing the calculation.
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Converting units: atm and mmHg
Boyle's Law, also known as the Boyle-Mariotte Law, describes the relationship between the pressure and volume of a confined gas. It was discovered by Robert Boyle in 1662, although it was also discovered independently by French physicist Edme Mariotte in 1679. The law is based on experiments with air, which Boyle considered to be a fluid of particles at rest between small invisible springs.
When applying Boyle's Law, it is important to ensure that the pressure and volume units are consistent. If you are given a problem where the pressure is provided in mmHg but you need to answer in atm, you must first convert the pressure to a single unit.
To convert from mmHg to atm, you can use the following formula: 1 mmHg = 0.00131579 atm. This means that there are 0.00131579 atmospheres in one mmHg.
For example, let's say you want to convert 8 atm to mmHg. You would use the formula: atm x 760 = mmHg. So, 8 atm x 760 = 6,080 mmHg. Therefore, 8 atm is equal to 6,080 mmHg.
You can also use online conversion calculators to convert between atm and mmHg. These calculators provide a quick and easy way to convert between pressure units.
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Real gases and ideal behaviour
Ideal gases are theoretical constructs that do not exist in reality. This is because the postulates of the kinetic molecular theory of gases ignore the volume occupied by the molecules of a gas and all interactions between molecules, whether attractive or repulsive. However, in reality, all gases have nonzero molecular volumes and the molecules of real gases interact with one another in ways that depend on the structure of the molecules. Therefore, real gases do not behave according to the assumptions of the kinetic-molecular theory and deviate from ideal behaviour.
Boyle's Law, discovered by Robert Boyle in 1662, is an empirical gas law that describes the relationship between the pressure and volume of a confined gas. It states that, for a fixed mass of an ideal gas kept at a fixed temperature, pressure and volume are inversely proportional. The law can be applied to gases with different units of pressure, such as mm Hg and atm, by converting one unit to the other before performing calculations.
Real gases behave ideally when subjected to either very low pressures or high temperatures. At low pressures, real gases exhibit PV/nRT values close to those predicted by the ideal gas law, whereas at high pressures, they exhibit larger PV/nRT values. At high temperatures, the molecules of real gases have sufficient kinetic energy to overcome intermolecular attractive forces, causing the effects of nonzero molecular volume to predominate. Conversely, as the temperature is lowered, the kinetic energy of the gas molecules decreases, and they can no longer overcome the intermolecular attractive forces, leading to liquefaction.
The deviations from ideal gas behaviour can be described by the van der Waals equation, which includes empirical constants to correct for the actual volume of the gaseous molecules and quantify the reduction in pressure due to intermolecular attractive forces. The ideal gas law can be useful for calculation purposes in either low-pressure or high-temperature systems, where real gases can be considered ideal.
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Calculating final volume
Boyle's Law, also known as the Boyle-Mariotte Law, is an empirical gas law that describes the relationship between the pressure exerted by a gas and its volume at a constant temperature and mass of gas. In other words, the pressure and volume of a gas are inversely proportional to each other as long as the temperature and the quantity of gas are kept constant.
Boyle's Law can be expressed as:
P1 * V1 = p2 * V2
Where:
- P1 and V1 are initial pressure and volume, respectively
- P2 and V2 are the final values of these gas parameters
To calculate the final volume (V2) using Boyle's Law, follow these steps:
- Identify the given information: Start by identifying the initial pressure (p1) and volume (V1) values provided in the problem. These values represent the initial state of the gas.
- Determine the unknown: Recognize that the final volume (V2) is what you need to find in this calculation.
- Apply Boyle's Law equation: Plug the given initial pressure and volume values into the equation: p1 * V1 = p2 * V2.
- Rearrange the equation: To solve for V2, divide both sides of the equation by p2. This gives you: V2 = (p1 * V1) / p2.
- Calculate: Substitute the known values into the equation and perform the multiplication and division to obtain the final volume (V2).
For example, let's consider a gas with an initial pressure of 2.5 atm and an initial volume of 6 liters. If the gas is decompressed isothermally to a pressure of 0.2 atm, we can calculate its final volume using Boyle's Law:
V2 = p1 * V1 / p2
V2 = (2.5 atm * 6 L) / 0.2 atm
V2 = 75 L
Therefore, the final volume of the gas is 75 liters.
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Frequently asked questions
Boyle's Law, also known as the Boyle-Mariotte Law, describes the relationship between the pressure and volume of a gas when its temperature and mass are held constant. It states that the pressure and volume of a gas are inversely proportional to each other.
When using Boyle's Law with mm Hg, it is important to note that the units of mm Hg will cancel out. For example, if you have a gas at a pressure of 740.0 mm Hg and a volume of 2.00 L, you can use Boyle's Law to calculate its volume at standard pressure.
One example of Boyle's Law in action is the expansion of a balloon. When a filled balloon is squeezed, the volume occupied by the air inside decreases, leading to an increase in pressure. This increase in pressure can eventually cause the balloon to pop. Another example is the behaviour of a gas when the atmospheric pressure changes, such as during an approaching storm.
