   Chapter 13, Problem 58QAP ### 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

# At what temperature would 4 . 25 g of oxygen gas O 2 , exert a pressure of 784 mm Hg in a 2 . 51 − L container?

Interpretation Introduction

Interpretation:

The temperature of oxygen gas in the sample should be calculated.

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:

The mass of oxygen gas is 4.25 g, pressure of gas is 784 mm Hg and volume of container is 2.51 L.

To calculate the temperature, first calculate the number of moles of gas using the following equation:

n=mM

Molar mass of oxygen is 32 g/mol and putting the values,

n=4.25 g32 g/mol=0.133 mol

Now, calculate temperature using the ideal gas equation as follows:

PV=nRT

On rearranging,

T=PVnR

Covert the given pressure from torr to atm as follows:

1 atm=760 mm Hg

Thus, following conversion factor will be used:

(1 atm760 mm Hg)

Putting the values,

T=(784 mm Hg)(1 atm760 mm Hg)(2

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