   Chapter 13, Problem 57QAP ### 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
8 views

# At what temperature will a 1 .0 − g sample of neon gas exert a pressure of 5 00 torr in a 5 .0 − L container?

Interpretation Introduction

Interpretation:

The temperature of neon 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 sample is 1.0 g, pressure of gas is 500 torr and volume of container is 5.0 L.

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

n=mM

Molar mass of neon is 20.18 g/mol and putting the values,

n=1.0 g20.18 g/mol=0.05 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 torr

Thus, following conversion factor will be used:

(1 atm760 torr)

Putting the values,

T=(500 torr)(1 atm760 torr)(5

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