Explain the universal gas law?

Answer 1

The universal gas law, or “Ideal Gas Law” shows the interaction of pressure, volume and temperature on a gaseous substance.

The “Ideal Gas Law” developed over time from the experiments and formulas derived by several separate chemists. It was first stated by Émile Clapeyron in 1834 as a combination of the empirical Boyle's law, Charles' law and Avogadro's Law. The simplest complete form is the combined law form, or Ideal Gas Law. #((PV)/T)_1 = ((PV)/T)_2# is applicable in all situations.

In real life, different molecular compositions show different amounts of intermolecular attraction or repulsion that will affect the final state of a gas. This factor is called the fugacity, and it can affect the conditions of some gases markedly (e.g. carbon dioxide). However, it is "Ideal," meaning that no intermolecular interactions are 'allowed'.

Therefore, anytime "non-ideal" gases are used beyond fairly dilute concentrations, caution (and corrections) must be made when calculating values with this equation.

The related Dalton's Law (1766-1844) describes partial pressures, and it was derived by combining the relationships of each of the other general laws (Boyles Law (1627-1691), Charles' Law (1746-1823), and Guy-Lussacs Law (1778-1850).

The other important one to keep in mind is the relationship to moles, which is PV = nRT (Avogadro's Law, 1776–1856). In this case, you must be cautious to use the appropriate "gas constant,” R, as different dimensions have different values for R.

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Answer 2

The universal gas law, also known as the ideal gas law, describes the behavior of ideal gases. It states that the pressure (P) of a gas is directly proportional to its temperature (T) and the amount of gas (n), and inversely proportional to its volume (V). Mathematically, it can be expressed as:

[PV = nRT]

Where:

  • P is the pressure of the gas (in Pascals or atmospheres)
  • V is the volume of the gas (in liters)
  • n is the number of moles of gas
  • R is the ideal gas constant ((8.314 , \text{J/mol} \cdot \text{K}))
  • T is the temperature of the gas (in Kelvin)

The universal gas law helps to predict the behavior of gases under different conditions, such as changes in pressure, volume, temperature, or the amount of gas.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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