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A 9.00 L tank at -3.2 °C is filled with 17.1 g of chlorine pentafluoride gas and 11.6 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Be sure each of your answer entries has the correct number of significant digits. gas chlorine pentafluoride sulfur tetrafluoride mole fraction 0 0 X

A 9.00 L tank at -3.2 °C is filled with 17.1 g of chlorine pentafluoride gas and 11.6 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Be sure each of your answer entries has the correct number of significant digits. gas chlorine pentafluoride sulfur tetrafluoride mole fraction 0 0 X

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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### Description A 9.00 L tank at −3.2 °C is filled with 17.1 g of chlorine pentafluoride gas and 11.6 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Be sure each of your answer entries has the correct number of significant digits. ### Table | Gas | Mole Fraction | |-------------------------|---------------| | Chlorine Pentafluoride | [Input Field] | | Sulfur Tetrafluoride | [Input Field] | ### Interactive Elements - There are interactive input fields next to each gas entry for calculating the mole fractions. - Two buttons are present: - A reset button to clear fields. - A check button to submit answers. ### Instructions Use the given masses to find the molar amounts of each gas and then determine the mole fraction by dividing the moles of each gas by the total moles present. Remember to consider significant figures based on provided data.
Transcribed Image Text:### Description A 9.00 L tank at −3.2 °C is filled with 17.1 g of chlorine pentafluoride gas and 11.6 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Be sure each of your answer entries has the correct number of significant digits. ### Table | Gas | Mole Fraction | |-------------------------|---------------| | Chlorine Pentafluoride | [Input Field] | | Sulfur Tetrafluoride | [Input Field] | ### Interactive Elements - There are interactive input fields next to each gas entry for calculating the mole fractions. - Two buttons are present: - A reset button to clear fields. - A check button to submit answers. ### Instructions Use the given masses to find the molar amounts of each gas and then determine the mole fraction by dividing the moles of each gas by the total moles present. Remember to consider significant figures based on provided data.
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The mole fraction of a component in the mixture is defined by the ratio of moles of that substance and the total moles of all components in the mixture.

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