Rashid calculated the partial pressures of the various major gases in the air we inhale.The following table gives the measured pressures of the major gases in both inhaled andexhaled air. Calculate the mole fractions of the gases in exhaled air.GasesInhaled Air (mmHg)Exhaled Air (mmHg)597568PN2Po21161580.328Pco2548PH20P Ar8.8.767767Pt

Mole fraction of a gas can be calculated using the formula mole fraction of gas =…

Answered: Rashid calculated the partial pressures…

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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Please help me solve part A&B. Thank you.
2. Sodium sulfide (0,1159 g) and excess hydrochloric acid were reacted together to form 35.75 mL of an unknown gas. The gas was collected over water when the atmospheric pressure was measured to be 767 mmHg. The temperature of the water was 23.0°C. Determine the molar mass, as well as identity, of the gas. Hint: You will need to reference your textbook for the vapor pressure of water.
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A sample of bromine gas occupies 2.65 L at 1.20 atm. What pressure (in kPa) would this sample of gas exert in a 1.50L container at the same temperature? Show your work. Click here for the Gas Laws Formula Sheet. Click here for the Periodic Table. I 0/10000 Word L 1 4 8 Support I Schoology Blog | PRIVACY POLICY | Te
c) Rashid calculated the partial pressures of the various major gases in the air we inhale. The following table gives the measured pressures of the major gases in both inhaled and exhaled air. Calculate the mole fractions of the gases in exhaled air. Gases Inhaled Air (mmHg) Exhaled Air (mmHg) 597 568 PN2 Po2 116 158 0.3 28 Pco2 48 PH20 8. 8 P Ar 767 767 Pt
3. A certain mass of magnesium is reacted with 6M HCl. The hydrogen gas liberated is collected by displacing 200 mL of water. The pressure of the gas and the atmospheric pressure are equalized. The atmospheric pressure is 762 mmHg. The temperature of the experiment is 27°C. How many moles of hydrogen have been liberated, and what is the mass of the magnesium that reacted?

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