Question

Using Charle's Law and Boyle's Law how can you derive the ideal gas equation ​

Answer 1

Answer:

As the pressure on a gas increases, the volume of the gas decreases because the gas particles are forced closer together. Conversely, as the pressure on a gas decreases, the gas volume increases because the gas particles can now move farther apart. Weather balloons get larger as they rise through the atmosphere to regions of lower pressure because the volume of the gas has increased; that is, the atmospheric gas exerts less pressure on the surface of the balloon, so the interior gas expands until the internal and external pressures are equal.

Explanation:

Charles's law, a statement that the volume occupied by a fixed amount of gas is directly proportional to its absolute temperature, if the pressure remains constant. It is a special case of the general gas law and can be derived from the kinetic theory of gases under the assumption of a perfect (ideal) gas.

Answer 2

Answer:

We can solve Boyle’s law and Charles’ law for the volume. Equating the two, we have

nα(T)P=nβ(P)T(2.6.1)(2.6.1)nα(T)P=nβ(P)T

The number of moles, nn, cancels. Rearranging gives

α(T)T=Pβ(P)(2.6.2)(2.6.2)α(T)T=Pβ(P)

In this equation, the left side is a function only of temperature, the right side only of pressure. Since pressure and temperature are independent

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