Answered: Suppose a gas mixture used for…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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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