In gas laws, various constants are used for precise measurements and predictions. The universal gas constant \(R\) is a key part of these laws. It is a physical constant expressed as \(8.314\ J/(mol·K)\) and ties together multiple gas law equations, like the Ideal Gas Law and the Van der Waals Equation.Additionally, in the Van der Waals equation, two unique constants \(a\) and \(b\) are tailored for each gas:
- \(a\): Measures intermolecular attraction. Higher values indicate stronger forces, as seen in gases like \(NH_3\).
- \(b\): Accounts for the volume occupied by the gas particles themselves.
Understanding these constants helps in predicting the behavior of real gases under various conditions. Comparing these constants across different gases reveals their unique properties, such as why \(NH_3\) has more intermolecular forces compared to \(H_2\) or \(He\).