Hydrogen gas is produced by the reaction between metallic aluminum and aqueous hydrochloric acid. 2 Al(s) + 6 HCl(aq) →→→ 2 AlCl3 (aq) + 3 H₂(g) The hydrogen gas produced by this reaction is typically collected via water displacement. During this process, the hydrogen gas becomes saturated with water vapor. If 280.5 mL of gas with a total pressure of 1.14 atm is collected via water displacement at 29.4 °C, what is the partial pressure of the hydrogen gas in the sample? The vapor pressure of water at 29.4 °C is 30.75 torr. atm PH₂ = How many grams of aluminum must have reacted to produce this quantity of hydrogen gas? mass of aluminum:

Hydrogen gas is produced by the reaction between metallic aluminum and aqueous hydrochloric acid. 2 Al(s) + 6 HCl(aq) →→→ 2 AlCl3 (aq) + 3 H₂(g) The hydrogen gas produced by this reaction is typically collected via water displacement. During this process, the hydrogen gas becomes saturated with water vapor. If 280.5 mL of gas with a total pressure of 1.14 atm is collected via water displacement at 29.4 °C, what is the partial pressure of the hydrogen gas in the sample? The vapor pressure of water at 29.4 °C is 30.75 torr. atm PH₂ = How many grams of aluminum must have reacted to produce this quantity of hydrogen gas? mass of aluminum:

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter10: Gases And Their Properties

Section: Chapter Questions

Problem 95IL: You have a 550.-mL tank of gas with a pressure of 1.56 atm at 24 C. You thought the gas was pure...

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93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
You have a 550.-mL tank of gas with a pressure of 1.56 atm at 24 C. You thought the gas was pure carbon monoxide gas, CO, but you later found it was contaminated by small quantities of gaseous CO2 and O2. Analysis shows that the tank pressure is 1.34 atm (at 24 C) if the CO2 is removed. Another experiment shows that 0.0870 g of O2 can be removed chemically. What are the masses of CO and CO2 in the tank, and what is the partial pressure of each of the three gases at 25 C?
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