The partial pressure of a gas in a mixture is calculated using which equation?

The correct equation for calculating the partial pressure of a gas in a mixture is given by ( p_J = x_J p ). In this equation, ( p_J ) represents the partial pressure of the gas J, ( x_J ) is the mole fraction of that gas in the mixture, and ( p ) is the total pressure of the gas mixture.

The mole fraction ( x_J ) is defined as the ratio of the number of moles of gas J to the total number of moles of all gases present in the mixture. Therefore, the partial pressure reflects the contribution of gas J to the total pressure, scaled by its proportion in the mixture.

This relationship is derived from Dalton's Law of Partial Pressures, which states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of each individual gas. The equation effectively allows you to determine how much of the total pressure is due to a specific gas, based on its mole fraction and the overall pressure of the system.

The other equations do not represent ways to calculate the partial pressure accurately. For instance, the equation involving the number of moles divided by total pressure does not yield a sensible result for pressure