The partial pressure of nitrogen in the atmosphere is 593. mmHg. Calculate the partial pressure in atm and torr. Round each of your answers to 3 significantdigits.atatmDtorrx10X

The objective of this question is to convert the given partial pressure of nitrogen from millimeters…

Answered: The partial pressure of nitrogen in the…

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter6: The States Of Matter

Section: Chapter Questions

Problem 6.21E

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A collapsed balloon is filled with He to a volume of 12.5 L at a pressure of 1.00 atm. Oxygen, O2, is then added so that the final volume of the balloon is 26 L with a total pressure of 1.00 atm. The temperature, which remains constant throughout, is 21.5 C. (a) What mass of He does the balloon contain? (b) What is the final partial pressure of He in the balloon? (c) What is the partial pressure of O2 in the balloon? (d) What is the mole fraction of each gas?
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The partial pressure of nitrogen in the atmosphere is 593. mmHg. Calculate the partial pressure in atm and torr. Round each of your answers to 3 significant digits. at atm D torr x10 X