= O STATES OF MATTER Calculating partial pressure in a gas mixture A 6.00 L tank at 11.1 °C is filled with 13.3 g of chlorine pentafluoride gas and 6.71 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. chlorine pentafluoride sulfur tetrafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 atm 0 0 atm atm X 1/5 S

= O STATES OF MATTER Calculating partial pressure in a gas mixture A 6.00 L tank at 11.1 °C is filled with 13.3 g of chlorine pentafluoride gas and 6.71 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. chlorine pentafluoride sulfur tetrafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 atm 0 0 atm atm X 1/5 S

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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