According to Dalton's Law, what does the total pressure of a mixture of gases equal?

The total pressure of a mixture of gases is correctly described by Dalton's Law, which states that the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of each individual gas present in the mixture. This means that each gas in the mixture contributes to the overall pressure based on its concentration and behavior, and these contributions are additive.

For instance, in a container with oxygen, nitrogen, and carbon dioxide, each of these gases exerts its own pressure independent of the others. By summing the pressure contributions from each gas, you determine the total pressure within that system. Dalton's Law is fundamental in understanding gas behavior, especially in respiratory physiology and various applications in chemistry and physics.

The other options do not accurately represent the relationship of partial pressures in a gas mixture and therefore do not align with the established principles outlined in Dalton's Law.