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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Transcribed Image Text:<Chapter 08
Problem 7
<
7 of 27
Review I Constants I Periodic Table
Learning Goal:
To use partial pressure in gas law calculations.
A volume of 18.0 L contains a mixture of 0.250 mole N2 , 0.250 mole O2 , and an unknown
quantity of He. The temperature of the mixture is 0 °C, and the total pressure is 1.00 atm
How many grams of helium are present in the
In a mixture of gases, the total pressure of the gas
mixture is equal to the sum of the partial pressures of the
individual gases. For example, if you have a mixture of
helium at 2 atm and argon at 4 atm, then the total
pressure of the gas inside the cylinder is 6 atm. (Figure
mixture?
gas
Express your answer to three significant figures and include the appropriate units.
View Available Hint(s)
Figure
Hint 1. Find the total number of moles
1 of 1
The following values are given:
. P 1.00 atm
V 18.0 L
T 0 °C
R 0.0821 L atm/(mole K)
3
nRT, determine the total number of moles of gas,
Using the ideal gas law, PV
ntotal
in the container. Be sure to convert the temperature to kelvins.
Express your answer to three significant figures and include the appropriate
units.
View Available Hint(s)
?
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