   # Equal masses of gaseous N 2 and Ar are placed in separate flasks of equal volume at the same temperature. Tell whether each of the following statements is true or false. Briefly explain your answer in each case. (a) There are more molecules of N 2 present than atoms of Ar. (b) The pressure is greater in the Ar flask (c) The Ar atoms have a greater rms speed than the N 2 molecules. (d) The N 2 molecules collide more frequently with the walls of the flask than do the Ar atoms. ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 10, Problem 42PS
Textbook Problem
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## Equal masses of gaseous N2 and Ar are placed in separate flasks of equal volume at the same temperature. Tell whether each of the following statements is true or false. Briefly explain your answer in each case. (a) There are more molecules of N2 present than atoms of Ar. (b) The pressure is greater in the Ar flask (c) The Ar atoms have a greater rms speed than the N2 molecules. (d) The N2 molecules collide more frequently with the walls of the flask than do the Ar atoms.

(a)

Interpretation Introduction

Interpretation:

The rightness of the given statements should be checked and have to state whether the given statements are true or false.  Equal masses of N2andAr are placed in separate flasks of equal volume at same temperature.

There are more molecules of N2 present than atoms of Ar.

Concept Introduction:

• The temperature of the gas is proportional to the average kinetic energy of the gas.
• Average kinetic energy can be denoted by KE¯

KE¯=32RT32R-proportionalityconstantT-Temperature

• Equation which relates mass, average speed and temperature:

u2¯=3RTMu2¯-averagespeedM-Molecularmassu2¯-rootmeansquare(rms)

• No.ofmoles=massmolarmass

### Explanation of Solution

For correct statements

From the equation,No.ofmoles=massmolarmass, it could be understood that number of moles and molar mass are inversely proportional.

MolarmassofAr=39

(b)

Interpretation Introduction

Interpretation:

The rightness of the given statements should be checked and have to state whether the given statements are true or false. Equal masses of N2andAr are placed in separate flasks of equal volume at same temperature.

The pressure is greater in the Ar flask.

Concept Introduction:

• The temperature of the gas is proportional to the average kinetic energy of the gas.
• Average kinetic energy can be denoted by KE¯

KE¯=32RT32R-proportionalityconstantT-Temperature

• Equation which relates mass, average speed and temperature:

u2¯=3RTMu2¯-averagespeedM-Molecularmassu2¯-rootmeansquare(rms)

• No.ofmoles=massmolarmass

(c)

Interpretation Introduction

Interpretation:

The rightness of the given statements should be checked and have to state whether the given statements are true or false.  Equal masses of N2andAr are placed in separate flasks of equal volume at same temperature.

The argon atoms have a greater rms speed than the N2 molecules.

Concept Introduction:

• The temperature of the gas is proportional to the average kinetic energy of the gas.
• Average kinetic energy can be denoted by KE¯

KE¯=32RT32R-proportionalityconstantT-Temperature

• Equation which relates mass, average speed and temperature:

u2¯=3RTMu2¯-averagespeedM-Molecularmassu2¯-rootmeansquare(rms)

• No.ofmoles=massmolarmass

(d)

Interpretation Introduction

Interpretation:

The rightness of the given statements should be checked and have to state whether the given statements are true or false. Equal masses of N2andAr are placed in separate flasks of equal volume at same temperature.

There are more molecules of N2 present than atoms of Ar.

Concept Introduction:

• The temperature of the gas is proportional to the average kinetic energy of the gas.
• Average kinetic energy can be denoted by KE¯

KE¯=32RT32R-proportionalityconstantT-Temperature

• Equation which relates mass, average speed and temperature:

u2¯=3RTMu2¯-averagespeedM-Molecularmassu2¯-rootmeansquare(rms)

• No.ofmoles=massmolarmass

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