 Dalton’s law defines the effect gas composition has on the pressures the gas exerts on its atmosphere. Dalton’s law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of the presence exerted by the individual gases. The gas in the mixture exerts a pressure equal to that of the gas in the mixture.

Dalton’s law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of the pressure exerted by the individual gases. Each gas in the mixture exerts a pressure equal to the fractional concentration of that gas in the mixture. Dalton’s law states that the pressure exerted by a mixture of gases or gases and vapours, enclosed in a given space, is equal to the sum of the pressures in which the gas or vapor would exert if it occupied the same space in its own right.

Rate Law

A rate law expresses how the rate depends on concentration, but it is often simply called rate law or differential rate law. Thus, when we use the term rate law in the text, the expression that gives the rate as a function of concentration. The expression describing the relation between the rate and these concentrations is called the rate law of the reaction.The rate of chemical reaction is either the speed at which the reaction substances or the velocity at which the products are produced, are used up.

A second kind of rate law is the integrated rate law, which will also be important in our study of kinetics. The integrated law of rate explains how time depends on the concentration. A given differential rate law is often related to some form of integrated rate legislation and vice versa. Therefore, the rate of a chemical reaction describes how fast the reactants are used up and the products are formed, usually expressed as the change in concentration of one of the reactants or products per unit time.

Dalton’s Law of Partial Pressure

Dalton’s law of partial pressures is applied frequently in respiratory physiology. It states that the partial pressure of a gas in a mixture of gases is the pressure that gas would exert if it occupied the total volume of the mixture. Thus, partial pressure is the total pressure multiplied by the fractional concentration of dry gas.

Px = PB x F

The relationship for humidified gas is determined by correcting the barometric pressure for the water vapor pressure.

Thus,

Px = (PB – PH2O) x F

So the total vapour pressure can be drawn from the equation. The total vapour pressure over the solution can be related to the mole fraction of any one component. The overall vapor pressure over the solution decreases or rises with the rise of the mole fraction of component A, depending on the vapor pressures of the individual components.