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Ch. 10 Physical Characteristics of Gases

Ch. 10 Physical Characteristics of Gases. 10.4 Dalton’s Law of Partial Pressure. Dalton’s Law of Partial Pressure. John Dalton responsible for atomic theory also studied gas mixtures the P of gas mixture is the sum of the individual pressures of each gas alone

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Ch. 10 Physical Characteristics of Gases

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  1. Ch. 10 Physical Characteristics of Gases 10.4 Dalton’s Law of Partial Pressure

  2. Dalton’s Law of Partial Pressure • John Dalton • responsible for atomic theory • also studied gas mixtures • the P of gas mixture is the sum of the individual pressures of each gas alone • the P that each gas exerts in the mixture is independent of the P that are exerted by other gases

  3. Dalton’s Law of Partial Pressure • the total P of a mixture of gases is equal to the sum of partial P of component gases, no matter how many different gases • PT = P1 + P2 + P3 + … • Partial Pressure- P of each gas in mixture

  4. Why? • the particles of each gas in a mixture have an equal chance to hit the walls • so each gas exerts P independent of that exerted by other gases • total P is result of the total # of collisions per unit of wall area

  5. set for a certain T equal to atmospheric pressure Water Displacement • gas produced is less dense than water so it replaces the water in the bottle • gas collected is not pure because it contains vapor from the water PT = Pgas + Pwater

  6. Example • Oxygen gas from decomposition of KClO3 was collected by water displacement. The barometric pressure and the temperature during the experiment were 731.0 torr and 20.0°C respectively. If the partial pressure of water vapor is 17.5 torr at 20.0°C, what was the partial pressure of oxygen collected? • PT = PO2 + PH2O • 731.0 torr = PO2 + 17.5 • PO2 = 713.5 torr

  7. Example • Find the partial pressure by 2 gases (A and B) mixed if the overall pressure is 790 mmHg. The percent by volume is A: 20% and B: 80%. • PT = PA + PB = 790 mmHg • A: 0.20 x 790 = 158 mmHg • B: 0.80 x 790 = 632 mmHg

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