Final answer:
The universal gas constant (R) is a value used in the ideal gas law and related equations to relate the volume, pressure, temperature, and moles of a gas. It has a value of 8.314 J/K mol or 0.0821 L·atm/mol·K. This constant is fundamental in understanding gas behavior and is derived from Avogadro's number and the Boltzmann constant.
Step-by-step explanation:
The universal gas constant, often denoted as R, is a constant that appears in the ideal gas law, which is an equation that relates the pressure, volume, temperature, and number of moles of an ideal gas. The value of R is calculated to be 8.314 J/K mol when the pressure is in kPa, but in chemistry, it is often used with the values of 0.0821 L·atm/mol·K or 8.314 J/mol·K. This constant is pivotal in equations like the combined gas law and the van der Waals equation of state, which serve as foundations for understanding the behaviour of gases under various conditions.
The value of R in units of L·atm/mol·K specifically relates to the conditions of molar volume of an ideal gas at 1 atm pressure and 0 °C temperature. The numerical value listed in Table 8.10.1 for R is indeed this same value, useful for solving problems that involve the ideal gas law.
Furthermore, R is derived from the fundamental constants NA (Avogadro's number) and kB (Boltzmann constant), as R = NAkB, reflecting the relationship between macroscopic and microscopic physical quantities. It is crucial when dealing with gas laws and related thermodynamic equations.