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Ch.10 - Gases
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.10 - GasesProblem 43b
Chapter 10, Problem 43b

Chlorine is widely used to purify municipal water supplies and to treat swimming pool waters. Suppose that the volume of a particular sample of Cl2 gas is 8.70 L at 119.3 kPa and 24 °C. (b) What volume will the Cl2 occupy at STP?

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1
Identify the initial conditions: Volume (V1) = 8.70 L, Pressure (P1) = 119.3 kPa, Temperature (T1) = 24 °C.
Convert the initial temperature from Celsius to Kelvin using the formula: T(K) = T(°C) + 273.15.
Identify the conditions at STP: Pressure (P2) = 101.3 kPa, Temperature (T2) = 273.15 K.
Use the combined gas law to relate the initial and final states: \( \frac{P_1 \times V_1}{T_1} = \frac{P_2 \times V_2}{T_2} \).
Rearrange the equation to solve for the final volume \( V_2 \): \( V_2 = \frac{P_1 \times V_1 \times T_2}{T_1 \times P_2} \).

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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 different conditions and allows for the calculation of one variable when the others are known.
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Ideal Gas Law Formula

Standard Temperature and Pressure (STP)

STP is defined as a temperature of 0 °C (273.15 K) and a pressure of 1 atm (101.3 kPa). At STP, one mole of an ideal gas occupies 22.4 L. Understanding STP is crucial for converting gas volumes from one set of conditions to another.
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Standard Temperature and Pressure

Gas Volume Conversion

Gas volume conversion involves using the Ideal Gas Law and the conditions of STP to determine how the volume of a gas changes with variations in temperature and pressure. This concept is key for solving problems that require finding the volume of a gas under different environmental conditions.
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Common Conversion Factors
Related Practice
Textbook Question

Many gases are shipped in high-pressure containers. Consider a steel tank whose volume is 210.0 L that contains O2 gas at a pressure of 16,500 kPa at 23 °C. (a) What mass of O2 does the tank contain?

Textbook Question

Chlorine is widely used to purify municipal water supplies and to treat swimming pool waters. Suppose that the volume of a particular sample of Cl2 gas is 8.70 L at 119.3 kPa and 24 °C. (d) At what pressure will the volume equal 5.00 L if the temperature is 58 °C?

Textbook Question
A 50.0 g sample of solid CO2 (dry ice) is added at -100 °C toan evacuated (all of the gas removed) container with a volumeof 5.0 L. If the container is sealed and then allowed to warmto room temperature 125 °C2 so that the entire solid CO2 isconverted to a gas, what is the pressure inside the container?
Textbook Question

Chlorine is widely used to purify municipal water supplies and to treat swimming pool waters. Suppose that the volume of a particular sample of Cl2 gas is 8.70 L at 119.3 kPa and 24 °C. (c) At what temperature will the volume be 15.00 L if the pressure is 116.8 kPa

Textbook Question
A 334-mL cylinder for use in chemistry lectures contains5.225 g of helium at 23 °C. How many grams of helium mustbe released to reduce the pressure to 7.60 MPa assuming idealgas behavior?
Textbook Question

An aerosol spray can with a volume of 125 mL contains 1.30 g of propane gas (C3H8) as a propellant. (c) The can's label says that exposure to temperatures above 50 °C may cause the can to burst. What is the pressure in the can at this temperature?