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Dalton's Law of Partial Pressure Collecting Gases Over Water Partial Pressure Gases > Partial Pressure Free to share, print, make copies and changes. Get yours at

The total pressure of a mixture of gases can be defined as the sum of the pressures of each individual gas: [Equation 1]. Dalton's Law of Partial Pressure Gases > Partial Pressure Free to share, print, make copies and changes. Get yours at /gases-10/partial-pressure-80/dalton-s-law-of-partial-pressure Equation 1 View on Boundless.com Dalton View on Boundless.com

The partial pressure of an individual gas is equal to the total pressure multiplied by the mole fraction of that gas. Boyle's Law and the Ideal Gas Law tell us the total pressure of a mixture depends solely on the number of moles of gas, and not the kinds of molecules; Dalton's Law allows us to calculate the total pressure in a system from each gas' individual contribution. Dalton's Law of Partial Pressure Free to share, print, make copies and changes. Get yours at /gases-10/partial-pressure-80/dalton-s-law-of-partial-pressure Dalton View on Boundless.com Gases > Partial Pressure

The total pressure in an inverted tube can be determined by the height of the water displaced in the tube. When calculating the amount of gas collected, Dalton's Law must be used to account for the presence of water vapor in the collecting bottle. Collecting Gases Over Water Free to share, print, make copies and changes. Get yours at /gases-10/partial-pressure-80/collecting-gases-over-water Collecting gas over water View on Boundless.com Gases > Partial Pressure

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Key terms Dalton's Law of Partial Pressures the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of each individual gas; also known as Dalton's Law of Partial Pressures mole fraction number of moles of one particular gas divided by the total moles of gas in the mixture pneumatic trough device used to collect a gas over water; the height of water displaced in the tube can be used to determine the total pressure inside the tube Free to share, print, make copies and changes. Get yours at Gases

Collecting a Gas Over Water How to calculate the pressure of a gas sample if it has been collected over water. Free to share, print, make copies and changes. Get yours at View on Boundless.com Gases

Collecting gas over water When collecting oxygen gas and calculating its partial pressure by displacing water from an inverted bottle, the presence of water vapor in the collecting bottle must be accounted for; this is easily accomplished using Dalton's Law of Partial Pressures. Free to share, print, make copies and changes. Get yours at Wikibooks. "Chemical Principles/Gas Laws and the Kinetic Theory." CC BY-SA View on Boundless.comCC BY-SA on Boundless.com Gases

Dalton Dr.McCord describes Dalton's Law of Partial Pressures. Free to share, print, make copies and changes. Get yours at View on Boundless.com Gases

Free to share, print, make copies and changes. Get yours at Gases On the top of Mt. Everest, the atmospheric pressure is approximately 34 kPa. If the gas ratios are the same as at sea level (i.e., 1/5 O2 and 4/5 N2), what is the partial pressure of O2 at the peak? A) 17.0 kPa B) 6.8 kPa C) 27.2 kPa D) 11.3 kPa

Free to share, print, make copies and changes. Get yours at Boundless - LO. "Boundless." CC BY-SA BY-SA 3.0http:// Gases On the top of Mt. Everest, the atmospheric pressure is approximately 34 kPa. If the gas ratios are the same as at sea level (i.e., 1/5 O2 and 4/5 N2), what is the partial pressure of O2 at the peak? A) 17.0 kPa B) 6.8 kPa C) 27.2 kPa D) 11.3 kPa

Free to share, print, make copies and changes. Get yours at Gases Gas from a lighter was collected over water. The loss of mass of the lighter was 128 mg and the volume of the collected gas was L. If the temperature and pressure in the room were at 35oC and 1 atm, what is the molar mass of the gas? (Note: Partial pressure of water vapor at 35oC is 42.2 mm Hg.) A) 52.1 g/mol B) 55.2 g/mol C) 53.6 g/mol D) 49.4 g/mol

Free to share, print, make copies and changes. Get yours at Boundless - LO. "Boundless." CC BY-SA BY-SA 3.0http:// Gases Gas from a lighter was collected over water. The loss of mass of the lighter was 128 mg and the volume of the collected gas was L. If the temperature and pressure in the room were at 35oC and 1 atm, what is the molar mass of the gas? (Note: Partial pressure of water vapor at 35oC is 42.2 mm Hg.) A) 52.1 g/mol B) 55.2 g/mol C) 53.6 g/mol D) 49.4 g/mol

Attribution Steve Lower's Website. "gas mixtures and Dalton's law." CC BY-SA BY-SAhttp:// Wikibooks. "Chemical Principles/Gas Laws and the Kinetic Theory." CC BY-SA BY-SA Wiktionary. "ideal gas law." CC BY-SA BY-SA 3.0http://en.wiktionary.org/wiki/ideal+gas+law Wikipedia. "Ideal Gas Equation." CC BY-SA BY-SA 3.0http://en.wikipedia.org/wiki/Ideal%20Gas%20Equation Wikipedia. "Dalton's law of partial pressures." CC BY-SA BY-SA Connexions. "The Ideal Gas Law." CC BY BY 3.0http://cnx.org/content/m12598/latest/?collection=col10264/latest Wikipedia. "Dalton's Law of Partial Pressure." CC BY-SA BY-SA Steve Lower's Website. "gas mixtures and Dalton's law." CC BY-SA BY-SA Wiktionary. "Boyle's law." CC BY-SA BY-SA 3.0http://en.wiktionary.org/wiki/Boyle's+law Free to share, print, make copies and changes. Get yours at Gases