Suppose a gas mixture used for anesthesia contains 4.00 mol oxygen (O₂) and 6.00 mol nitrous oxide (N₂O). The total pressure of the mixture is 2.00 atm. a. A mole fraction is defined as the moles of a specific component divided by the total number of moles present. What is the mole fraction of N₂O in this mixture? b. What is the partial pressure in atm of O₂ in this mixture? c. What is the partial pressure in atm of N₂O in this mixture?
Suppose a gas mixture used for anesthesia contains 4.00 mol oxygen (O₂) and 6.00 mol nitrous oxide (N₂O). The total pressure of the mixture is 2.00 atm. a. A mole fraction is defined as the moles of a specific component divided by the total number of moles present. What is the mole fraction of N₂O in this mixture? b. What is the partial pressure in atm of O₂ in this mixture? c. What is the partial pressure in atm of N₂O in this mixture?
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter19: The Representative Elements
Section: Chapter Questions
Problem 104CP
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4. Suppose a gas mixture used for anesthesia contains 4.00 mol oxygen (O₂) and 6.00 mol nitrous oxide (N₂O). The total pressure of the mixture is 2.00 atm.
a. A mole fraction is defined as the moles of a specific component divided by the total number of moles present. What is the mole fraction of N₂O in this mixture?
b. What is the partial pressure in atm of O₂ in this mixture?
c. What is the partial pressure in atm of N₂O in this mixture?
5. A gas is formed in the reaction shown below. The gas laws can help determine the volume of gas produced. Zn(s) + 2 HCl(aq) → ZnCl₂ + H₂(g)
a. In the last part, you determined that you started with 2.001 moles of Zn. How many moles of H₂ gas will be formed in this reaction?
b. At STP, what volume in L of H₂ will be produced?
Remember the gas constant, R, is 0.08206 L・atm/mol・K.
6. When the ideas from Boyle’s Law, Charles’ Law and Gay-Lussac’s Law are combined, you get the combined gas law. This law combines the effects of pressure, temperature and volume changes on a gas. Remember the combined gas law is P₁V₁/T₁ = P₂V₂/T₂ Imagine an ideal gas in a cylinder with a piston, starting at a pressure of 1.00 atm and a volume of 10.0 L at 298.15 K. This system is cooled to 273.15 K and compressed to 5.00 L. What is the final pressure in the cylinder, in atm?
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