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Chapter 31: Problem 3

Consider a mixture that has partial pressures of 525 torr of He and 363 torr of Ar. What is the total pressure of this mixture in torr and in atm?

Short Answer

Expert verified
The total pressure in torr is \( P = 888 torr\). The total pressure in atm is \( P = 1.17 atm\).

Step by step solution

01

Calculate Total Pressure in Torr

Add the given partial pressures to calculate the total pressure in torr. Thus, the total pressure in torr is \( P = P_{He} + P_{Ar} = 525 torr + 363 torr\)
02

Calculate the Total Pressure in Atm

Use the conversion factor as \(1 atm = 760 torr\) to convert the total pressure from torr to atm. So, the total pressure in atm is \( P_{atm} = \frac{P_{torr}}{760}\)

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Most popular questions from this chapter

Rearrange the ideal gas law to isolate \(V\) on the left side to complete the equation: \(V=\)

Based on your answer to CTQ 4: a) How does the volume of a gas (at constant \(n\) and \(P\) ) change as the temperature is raised? b) How does the volume of a gas (at constant \(n\) and \(T\) ) change as the pressure is increased? c) How does the volume of a gas (at constant \(T\) and \(P\) ) change as the number of molecules is increased?

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