   Chapter 13, Problem 51QAP ### 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
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# What mass of neon gas is required to fill a 5 .00 − L container to a pressure of 1 .0 2 atm at 25  ° C ?

Interpretation Introduction

Interpretation:

The mass of neon gas required to fill the container 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 volume of container is 5.00 L, pressure of gas is 1.02 atm and temperature is 25 C.

To calculate the mass, first calculate the number of moles of gas using the ideal gas equation as follows:

n=PVRT

Convert the temperature from C to K as follows:

0 C=273.15 K

Thus,

25 C=(25+273.15) K=298.15 K

Putting the values,

n=(1

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