The ideal gas equation, PV = nRT, can be rearranged to solve for any of the three variables. To solve for pressure, divide both sides by volume (P = nRT/V). To solve for volume, divide both sides by pressure (V = nRT/P). To solve for temperature, divide both sides by the product of moles and gas constant (T = PV/nR).
According to the ideal gas equation, pressure and volume are inversely proportional. This means that as pressure increases, volume decreases, and vice versa, as long as all other variables (moles, temperature, and gas constant) remain constant. This relationship is known as Boyle's Law.
Temperature has a direct relationship with the ideal gas equation. As temperature increases, so does the volume of the gas, assuming all other variables are constant. This relationship is known as Charles's Law.
The gas constant (R) is a proportionality constant that relates the properties of an ideal gas to its temperature, pressure, and volume. Its value depends on the units used for pressure, volume, and temperature. The most commonly used value is 0.0821 L⋅atm/mol⋅K.
The ideal gas equation is an approximation that is most accurate for gases at low pressure and high temperature. This means that it can be used for most gases under normal conditions. However, at high pressures and low temperatures, the ideal gas law breaks down and more complex equations, such as the van der Waals equation, must be used.