Does the magnitude of C in Boyle's Law depend on the quantity of gas enclosed?

In summary, Boyle's law states that at constant temperature, the product of pressure and volume is a constant (PV = C). This constant, represented by C, is dependent on the quantity of gas enclosed, as seen in the ideal gas law equation where C is directly proportional to the number of molecules (PV = NkT). This also explains why Boyle's Law holds true when temperature is constant.
  • #1
Amith2006
427
2
1) According to Boyle’s law,
PV = C (At constant temperature)

Where C is the constant of proportionality. Is it true that the magnitude of C depends upon the quantity of gas enclosed?
 
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  • #2
Yes.

If you look at the ideal gas law, PV=NkT where T is temperature in Kelvin, k is the Boltzmann constant, and N is the number of molecules you will see that C in your example is directly proportional to the number of molecules. From that relationship you can also see why Boyle's Law works when temperature is constant.

(Alternatively you can write the ideal gas law as PV=nRT where n is the number of moles and R is the ideal gas law constant.)
 
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What is the Kinetic Theory of gases?

The Kinetic Theory of gases is a scientific theory that explains the behavior of gases based on the motion of their molecules. It states that gas molecules are constantly moving in random directions and at different speeds, and that the pressure, volume, and temperature of a gas are all related to the average kinetic energy of its molecules.

What are the assumptions of the Kinetic Theory of gases?

The Kinetic Theory of gases is based on three main assumptions: 1) Gas molecules are in constant, random motion; 2) The size of gas molecules is negligible compared to the distance between them; and 3) Collisions between gas molecules are perfectly elastic, meaning no energy is lost during collisions.

How does the Kinetic Theory of gases explain the properties of gases?

The Kinetic Theory of gases explains the properties of gases by relating them to the motion of gas molecules. For example, the pressure of a gas is caused by the constant collisions of gas molecules with the walls of its container, and the temperature of a gas is directly proportional to the average kinetic energy of its molecules.

What is the relationship between temperature and kinetic energy in the Kinetic Theory of gases?

According to the Kinetic Theory of gases, the temperature of a gas is directly proportional to the average kinetic energy of its molecules. This means that as the temperature of a gas increases, the average kinetic energy of its molecules also increases, resulting in faster and more frequent collisions and a higher pressure.

What are some real-world applications of the Kinetic Theory of gases?

The Kinetic Theory of gases is used in various fields such as chemistry, physics, and engineering to understand and predict the behavior of gases. It is also the basis for many practical applications, including gas laws, refrigeration and air conditioning systems, and the production of industrial gases. Additionally, the Kinetic Theory of gases is used to explain phenomena such as diffusion, effusion, and thermal conductivity.

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