Ch.5 - Gases

Tro - Chemistry: A Molecular Approach 4th Edition

Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook

Tro 4th Edition

Ch.5 - Gases

Problem 46

Chapter 5, Problem 46

A 1.0-L container of liquid nitrogen is kept in a closet measuring 1.0 m by 1.0 m by 2.0 m. Assuming that the container is completely full, that the temperature is 25.0 °C, and that the atmospheric pressure is 1.0 atm, calculate the percent (by volume) of air that is displaced if all of the liquid nitrogen evaporates. (Liquid nitrogen has a density of 0.807 g/mL.)

Verified step by step guidance

Calculate the mass of liquid nitrogen using its density and the volume of the container: \( \text{mass} = \text{density} \times \text{volume} \).

Convert the mass of liquid nitrogen to moles using the molar mass of nitrogen (N2), which is approximately 28.02 g/mol.

Use the ideal gas law \( PV = nRT \) to find the volume of nitrogen gas at 25.0 °C and 1.0 atm. Remember to convert the temperature to Kelvin by adding 273.15.

Calculate the volume of the closet in liters: \( \text{volume} = \text{length} \times \text{width} \times \text{height} \).

Determine the percent of air displaced by dividing the volume of nitrogen gas by the volume of the closet and multiplying by 100 to get the percentage.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ideal Gas Law

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is essential for understanding how gases behave under varying conditions and is crucial for calculating the volume of nitrogen gas produced when liquid nitrogen evaporates.

Density and Volume Conversion

Density is defined as mass per unit volume (density = mass/volume). In this problem, knowing the density of liquid nitrogen allows us to convert its mass into volume, which is necessary to determine how much nitrogen gas will occupy the space when it evaporates.

Displacement of Air

When a substance is placed in a container, it displaces an equivalent volume of the fluid (or gas) that was previously in that space. In this scenario, calculating the volume of nitrogen gas produced will help determine the volume of air displaced in the closet, which is essential for finding the percent of air displaced.

Related Practice

Textbook Question

A piece of dry ice (solid carbon dioxide) with a mass of 28.8 g sublimes (converts from solid to gas) into a large balloon. Assuming that all of the carbon dioxide ends up in the balloon, what is the volume of the balloon at 22 °C and a pressure of 742 mmHg?

An automobile tire has a maximum rating of 38.0 psi (gauge pressure). The tire is inflated (while cold) to a volume of 11.8 L and a gauge pressure of 36.0 psi at a temperature of 12.0 °C. On a hot day, the tire warms to 65.0 °C, and its volume expands to 12.2 L. Does the pressure in the tire exceed its maximum rating? (Note: The gauge pressure is the difference between the total pressure and atmospheric pressure. In this case, assume that atmospheric pressure is 14.7 psi.)

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Textbook Question

This picture represents a sample of gas at a pressure of 1 atm, a volume of 1 L, and a temperature of 25 °C. Draw a similar picture showing what would happen to the sample if the volume were reduced to 0.5 L and the temperature were increased to 250 °C. What would happen to the pressure?

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Textbook Question

A weather balloon is inflated to a volume of 28.5 L at a pressure of 748 mmHg and a temperature of 28.0 °C. The balloon rises in the atmosphere to an altitude of approximately 25,000 ft, where the pressure is 385 mmHg and the temperature is -15.0 °C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.

Which gas sample has the greatest pressure? Assume that all the samples are at the same temperature. Explain.

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