The Ideal Gas Law is a mathematical equation that describes the behavior of an ideal gas under different conditions. It states that the pressure (P), volume (V), temperature (T), and number of moles (n) of an ideal gas are directly proportional to each other.
To solve for T2 in the Ideal Gas Law, you will use the rearranged equation: T2 = (P2 x V1 x T1) / (P1 x V2). This equation allows you to calculate the temperature (T2) of an ideal gas when given the initial pressure (P1), volume (V1), and temperature (T1), as well as the final pressure (P2) and volume (V2).
The units of measurement for the Ideal Gas Law depend on the values used for each variable. The pressure (P) can be measured in atmospheres (atm), kilopascals (kPa), or other units of pressure. The volume (V) can be measured in liters (L) or cubic meters (m³). The temperature (T) can be measured in Kelvin (K) or degrees Celsius (°C). The number of moles (n) is measured in moles (mol).
An ideal gas is a hypothetical gas that follows the Ideal Gas Law under all conditions. This means that an ideal gas has no intermolecular forces, occupies no volume, and experiences no collisions. In reality, no gas is truly ideal, but some gases such as hydrogen and helium behave closely to the predictions of the Ideal Gas Law.
The Ideal Gas Law is a simplified version of the gas laws that applies to ideal gases. Real gases do not always follow the predictions of the Ideal Gas Law due to factors such as intermolecular forces and volume occupied by the gas particles. However, at high temperatures and low pressures, real gases can behave similarly to ideal gases and the Ideal Gas Law can still provide accurate approximations.