How does the partial pressure, exerted by a single component in a gaseous mixture, relate to the total pressure?
Answers
The pressure depends on only the total number of particles of gas present, the total pressure of the mixture will simply be twice the pressure of either component. More generally, the total pressure exerted by a mixture of gases at a given temperature and volume is the sum of the pressures exerted by each gas alone. Furthermore, if we know the volume, the temperature, and the number of moles of each gas in a mixture, then we can calculate the pressure exerted by each gas individually, which is its partial pressure, the pressure the gas would exert if it were the only one present (at the same temperature and volume).
The ideal gas law assumes that all gases behave identically and that their behavior is independent of attractive and repulsive forces. If volume and temperature are held constant, the ideal gas equation can be rearranged to show that the pressure of a sample of gas is directly proportional to the number of moles of gas present:
P=n(R/TV)=n×constant.
The total pressure exerted by a mixture of gases is the sum of the partial pressures of component gases. This law was first discovered by John Dalton, the father of the atomic theory of matter. It is now known as Dalton’s law of partial pressures. We can write it mathematically as:
P(tot)=P1+P2+P3+P4...
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Answer:
The total pressure exerted by a mixture of two or more non reactive gases in a definite volume is equal to the sum of individual pressure which each gas would exert if it occupies the same volume alone at a constant temperature.
P(total) = P₁ + P₂