Homework Help is Here – Start Your Trial Now!
Science
Chemistry
A 9.00 L tank at 28.8 °C is filled with 3.33 g of sulfur tetrafluoride gas and 14.3 g of sulfur hexafluorid under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Rounde sulfur tetrafluoride sulfur hexafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0.239 0.0085 0.761 atm 0.270 atm 0.355 atm X 5

A 9.00 L tank at 28.8 °C is filled with 3.33 g of sulfur tetrafluoride gas and 14.3 g of sulfur hexafluorid under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Rounde sulfur tetrafluoride sulfur hexafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0.239 0.0085 0.761 atm 0.270 atm 0.355 atm X 5

Chemistry
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...
See similar textbooks
icon
Related questions
Question
100%
i need help i got the partial pressures wrong and need help please
The task involves calculating the mole fraction and partial pressure of sulfur tetrafluoride and sulfur hexafluoride gases in a 9.00 L tank at 28.8 °C. **Initial Problem Statement:** - A 9.00 L tank is filled with 3.33 g of sulfur tetrafluoride gas and 14.3 g of sulfur hexafluoride gas. - The task is to calculate the mole fraction and partial pressure of each gas and the total pressure in the tank. **Results from the Table:** 1. **Sulfur Tetrafluoride:** - **Mole fraction:** 0.239 - **Partial pressure:** 0.085 atm 2. **Sulfur Hexafluoride:** - **Mole fraction:** 0.761 - **Partial pressure:** 0.270 atm 3. **Total pressure in tank:** - 0.355 atm **Feedback Area:** - Incorrect answers are noted for both gases' partial pressures. **Instructions:** - A prompt to "Try one last time" is displayed, along with a "Recheck" button to submit revised answers. This exercise is an example of applying gas laws to real-world problems, specifically focusing on computing mole fractions and partial pressures of gas mixtures under specific conditions.
Transcribed Image Text:The task involves calculating the mole fraction and partial pressure of sulfur tetrafluoride and sulfur hexafluoride gases in a 9.00 L tank at 28.8 °C. **Initial Problem Statement:** - A 9.00 L tank is filled with 3.33 g of sulfur tetrafluoride gas and 14.3 g of sulfur hexafluoride gas. - The task is to calculate the mole fraction and partial pressure of each gas and the total pressure in the tank. **Results from the Table:** 1. **Sulfur Tetrafluoride:** - **Mole fraction:** 0.239 - **Partial pressure:** 0.085 atm 2. **Sulfur Hexafluoride:** - **Mole fraction:** 0.761 - **Partial pressure:** 0.270 atm 3. **Total pressure in tank:** - 0.355 atm **Feedback Area:** - Incorrect answers are noted for both gases' partial pressures. **Instructions:** - A prompt to "Try one last time" is displayed, along with a "Recheck" button to submit revised answers. This exercise is an example of applying gas laws to real-world problems, specifically focusing on computing mole fractions and partial pressures of gas mixtures under specific conditions.
Expert Solution
steps

Step by step

Solved in 4 steps with 10 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Mole Concept
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS