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The combustion of octane, C, H. proceeds according to the reaction shown. 2C,H) + 250,(2) – 16CO,(g) + 18 H,o) If 514 mol of octane combusts, what volume of carbon dioxide is produced at 20.0 C and 0.995 atm?

The combustion of octane, C, H. proceeds according to the reaction shown. 2C,H) + 250,(2) – 16CO,(g) + 18 H,o) If 514 mol of octane combusts, what volume of carbon dioxide is produced at 20.0 C and 0.995 atm?

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter5: Gases
Section: Chapter Questions
Problem 78QAP
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Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table. Total volume of H-(g) collected 93.88 ml Temperature Barometric pressure 24.0 °C 742 mmHg 22.5 mmHg Vapor pressure of water at 24.0 °C Calculate the moles of hydrogen gas produced by the reaction. moles: 3.21 x10 mol H2 The combustion of octane, C, H,. proceeds according to the reaction shown. 2C,H,0) + 250,(g) – 16 CO,(g) + 18 H,O(1) If 514 mol of octane combusts, what volume of carbon dioxide is produced at 20.0 °C and 0.995 atm? A container of N,0,() has a pressure of 0.320 atm. When the absolute temperature of the N,0,() is tripled, the gas completely decomposes, producing NO, (g) and NO(g). Calculate the final pressure of the gas mixture, assuming that the container volume does not change. atm final pressure: 0.96 Incorect
Transcribed Image Text:Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table. Total volume of H-(g) collected 93.88 ml Temperature Barometric pressure 24.0 °C 742 mmHg 22.5 mmHg Vapor pressure of water at 24.0 °C Calculate the moles of hydrogen gas produced by the reaction. moles: 3.21 x10 mol H2 The combustion of octane, C, H,. proceeds according to the reaction shown. 2C,H,0) + 250,(g) – 16 CO,(g) + 18 H,O(1) If 514 mol of octane combusts, what volume of carbon dioxide is produced at 20.0 °C and 0.995 atm? A container of N,0,() has a pressure of 0.320 atm. When the absolute temperature of the N,0,() is tripled, the gas completely decomposes, producing NO, (g) and NO(g). Calculate the final pressure of the gas mixture, assuming that the container volume does not change. atm final pressure: 0.96 Incorect
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