How is the partial pressure of a gas in a mixture related to the total pressure of the gaseous mixture?
Answers
Answer:
Because it is dependent solely the number of particles and not the identity of the gas, the Ideal Gas Equation applies just as well to mixtures of gases is does to pure gases. In fact, it was with a gas mixture—ordinary air—that Boyle, Gay-Lussac, and Charles performed their early experiments. The only new concept we need to deal with gas mixtures is partial pressure, a concept invented by the famous English chemist John Dalton (1766-1844). Dalton correctly reasoned that the low density and high compressibility of gases were indicative of the fact that they consisted mostly of empty space; from this, it Dalton concluded that when two or more different gases occupy the same volume, they behave entirely independently of one another.
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Answer:
The partial pressure of a gas mixture is related to the total pressure of the gaseous mixture by Dalton's Law.
Explanation:
According to Dalton’s law of partial pressure, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures exerted by each individual gas present in the mixture. For example, the total pressure exerted by a mixture of three gases A, B, and C is equal to the sum of the individual partial pressures exerted by gas A, gas B, and gas C.
Total pressure, P = Pa + Pb + Pc
where, Pa, Pb, and Pc are the individual partial pressures exerted by gas A, gas B, and gas C.
So, the partial pressure of a gas is related to the total pressure of the gas mixture by Dalton's Law of partial pressure.
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