Partial pressure **Partial Pressures I**A sample of a gas mixture contains the following quantities of three gases:| Compound | Mass ||----------|-------|| CO | 2.16 g|| CO₂ | 2.69 g|| SF₆ | 3.50 g|The sample has:- Volume = 2.50 L- Temperature = 16.6 °C**Questions:**1. What is the partial pressure for each gas, in mmHg?2. What is the total pressure in the flask?- CO: [______] mmHg- CO₂: [______] mmHg- SF₆: [______] mmHg- Total: [______] mmHg**Instructions:**- Use the ideal gas law and the molecular weights of the gases to calculate the moles.- Calculate the partial pressures using the mole fraction and the total pressure.

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TUTOR Partial Pressures I A sample of a gas mixture contains the following quantities of three gases. compound mass CO 2.16 g CO2 2.69 g SF6 3.50 g The sample has: volume = 2.50L %3D temperature = 16.6 °C What is the partial pressure for each gas, in mmHg? What is the total pressure in the flask? CO mmHg CO2 mmHg SF6 mmHg total mmHg

TUTOR Partial Pressures I A sample of a gas mixture contains the following quantities of three gases. compound mass CO 2.16 g CO2 2.69 g SF6 3.50 g The sample has: volume = 2.50L %3D temperature = 16.6 °C What is the partial pressure for each gas, in mmHg? What is the total pressure in the flask? CO mmHg CO2 mmHg SF6 mmHg total mmHg

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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