   Chapter 13, Problem 60QAP ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
3 views

# Which flask will have the higher pressure a 5 .00 − L flask cantaining 4 . 15 g of helium at 298 K , or a l 00 − L flask containing 56 . 2 g of argon at 3 0 3 K ?

Interpretation Introduction

Interpretation:

The flask with higher pressure should be determined.

Concept Introduction:

According to ideal gas equation:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

The value of Universal gas constant can be taken as 0.082 L atm K1 mol1.

Mass of gas can be calculated from number of moles and molar mass as follows:

m=n×M

Here, n is number of moles, m is mass and M is molar mass.

Explanation

Given Information:

Volume of flask containing 4.15 g of helium gas is 5.00 L at 298 K and volume of flask containing 56.2 g of argon is 10.0 L at 303 K.

Calculation:

Calculate the pressure of flask 1 containing helium as follows:

To calculate the pressure, first calculate number of moles of helium as follows:

n=mM

Molar mass of helium gas is 4.0 g/mol putting the values,

n=4.15 g4 g/mol=1.0375 mol

Now, calculate pressure of flask as follows:

P=nRTV

Putting the values,

P=(1.0375 mol)(0.082 L atm/ K mol)(298 K)(5.00 L)=5

### Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

#### The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started 