A 10.0 L tank at 13.5 °C is filled with 15.4 g of dinitrogen difluoride gas and 4.72 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.| | | ||--------------------------------|-------------------------------|--------|| **dinitrogen difluoride** | **mole fraction:** | || | **partial pressure:** | ___ atm|| | | || **sulfur tetrafluoride** | **mole fraction:** | || | **partial pressure:** | ___ atm|| | | || **Total pressure in tank:** | | ___ atm|There is an interactive element represented by a reset button next to a checkbox labeled "×10" which allows for scaling or unit adjustment (specific function not detailed).

Given: Volume of tank = 10.0 L Mass of dinitrogen difluoride = 15.4 g Mass of sulfur tetrafluoride…

10.0 L tank at 13.5 °C is filled with 15.4 g of dinitrogen difluoride gas and 4.72 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal ases 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. mole fraction: dinitrogen difluoride partial pressure: ? atm mole fraction: sulfur tetrafluoride partial pressure: atm Total pressure in tank: atm O

10.0 L tank at 13.5 °C is filled with 15.4 g of dinitrogen difluoride gas and 4.72 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal ases 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. mole fraction: dinitrogen difluoride partial pressure: ? atm mole fraction: sulfur tetrafluoride partial pressure: atm Total pressure in tank: atm O

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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Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

A 10.0 L tank at 13.5 °C is filled with 15.4 g of dinitrogen difluoride gas and 4.72 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.

| | | |
|--------------------------------|-------------------------------|--------|
| **dinitrogen difluoride** | **mole fraction:** | |
| | **partial pressure:** | ___ atm|
| | | |
| **sulfur tetrafluoride** | **mole fraction:** | |
| | **partial pressure:** | ___ atm|
| | | |
| **Total pressure in tank:** | | ___ atm|

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