When multiplied by three-halves T it is equivalent to the (*) average translational energy of an ideal gas, and when multiplied by the number of micro-states available to a system, this quantity gives entropy.
The van't Hoff relation states that this quantity is equal to the equilibrium pressure of a system divided by the product of concentration and temperature. In the Arrhenius equation, when activation energy is given in molecular units, this quantity, instead of the gas constant, is used. When multiplied by three-halves T it is equivalent to the (*) average translational energy of an ideal gas, and when multiplied by the number of micro-states available to a system, this quantity gives entropy. Name this quantity, a constant equal to the gas constant divided by Avogadro's constant, often represented by K sub B.
The van't Hoff relation states that this quantity is equal to the equilibrium pressure of a system divided by the product of concentration and temperature.
{Boltzmann}’s Constant [accept {K-sub-B} early]