   # You have two flasks of equal volume. Flask A contains H 2 at 0 °C and 1 atm pressure. Flask B contains CO 2 gas at 25 °C and 2 atm pressure. Compare these two gases with respect to each of the following: (a) average kinetic energy per molecule (b) root mean square speed (c) number of molecules (d) mass of gas ### 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 41PS
Textbook Problem
2517 views

## You have two flasks of equal volume. Flask A contains H2 at 0 °C and 1 atm pressure. Flask B contains CO2 gas at 25 °C and 2 atm pressure. Compare these two gases with respect to each of the following: (a) average kinetic energy per molecule (b) root mean square speed (c) number of molecules (d) mass of gas

(a)

Interpretation Introduction

Interpretation:

The average kinetic energy of two gases given should be compared.

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)

### Explanation of Solution

The average kinetic energy of H2andCO2 at different temperatures

H2-Temperature=0°C=273KPressure=1atmCO2 -Temperature=25°C=25+273=298Pressure=2atm

Average kinetic energy can be calculated using the equation:

KE¯=32RT32R-proportionalityconstantT-Temperature

(b)

Interpretation Introduction

The average rms has be compared.

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)

(c)

Interpretation Introduction

The average number of molecules of two gases given should be compared.

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)

(d)

Interpretation Introduction

The average masses of two gases given should be compared.

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)

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