   # A piece of solid carbon dioxide, with a mass of 7.8 g, is placed in a 4.0-L otherwise empty container at 27°C. What is the pressure in the container after all the carbon dioxide vaporizes? If 7.8 g solid carbon dioxide were placed in the same container but it already contained air at 740 torr, what would be the partial pressure of carbon dioxide and the total pressure in the container after the carbon dioxide vaporizes? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 8, Problem 83E
Textbook Problem
1517 views

## A piece of solid carbon dioxide, with a mass of 7.8 g, is placed in a 4.0-L otherwise empty container at 27°C. What is the pressure in the container after all the carbon dioxide vaporizes? If 7.8 g solid carbon dioxide were placed in the same container but it already contained air at 740 torr, what would be the partial pressure of carbon dioxide and the total pressure in the container after the carbon dioxide vaporizes?

Interpretation Introduction

Interpretation: The total pressure of container and the partial pressure of the 7.8g carbon dioxide (vaporized) placed in the container should be determined at 27oC when the container is empty situation and the container having air of 740torr .

Concept introduction:

Partial pressure of a gas in a mixture of gases is the pressure of that gas when it alone.

• Partial pressure of a gas, according to ideal gas equation,

Pressure=Numberofmoles×R×TemperatureVolume

• Number of moles of a substance from its given mass is,

Number of moles=GivenmassMolecularmass

Total pressure of a mixture of gases is the sum of individual partial pressures of constituted gases.

### Explanation of Solution

Explanation

The given mass of carbon dioxide is 7.8g. So the number of moles of this carbon dioxide is,

Equation for finding number of moles is,

Number of moles=GivenmassMolecularmass

Therefore, the number of moles of this carbon dioxide is,

Number of moles of given carbon dioxide=7.8g44g*1mol =0.1772mol

The number of moles of carbon dioxide is calculated.

nco2=0.1772mol

Equation for finding partial pressure of a gas,

Partial pressure of a gas, according to ideal gas equation,

Pressure=Numberofmoles×R×TemperatureVolume

• Partial pressure of carbon dioxide in empty container is,

Pressure of carbon dioxide=0

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