A piece of solid carbon dioxide, with a mass of 22.0 g, is placed in an otherwise empty 4.00-L container at 278C. What is the pressure in the container after all the carbon dioxide vaporizes? If 22.0 g of solid carbon dioxide was placed in a similar container already containing air at 740. torr, what would be the partial pressure of carbon dioxide and the total pressure in the container after the carbon dioxide had vaporized?
Answer to relevant QuestionsDerive Dalton’s law of partial pressures from the ki-netic molecular theory of gases. What assumptions are necessary? Methane (CH4) gas flows into a combustion chamber at a rate of 200. L/ min at 1.50 atm and ambient temperature. Air is added to the chamber at 1.00 atm and the same temperature, and the gases are ignited. a. To ensure ...You are given an unknown gaseous binary compound (that is, a compound consisting of two different elements). When 10.0 g of the compound is burned in excess oxygen, 16.3 g of water is produced. The compound has a density ...A diagram for an open- tube manometer is shown below. If the flask is open to the atmosphere, the mercury levels are equal. For each of the following situations in which a gas is contained in the flask, calculate the ...At 0oC a 1.0 L flask contains 5.0 × 10-2 mole of N2, 1.5 × 102 mg O2, and 5.0 × 10-1 molecules of NH3. What is the partial pressure of each gas, and what is the total pressure in the flask?
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