Textbook Question
A sample of gas has an initial volume of 5.6 L at a pressure of 735 mmHg. If the volume of the gas is increased to 9.4 L, what is its pressure?
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Ch.5 - Gases
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving107
- Ch.2 - Atoms & Elements100
- Ch.3 - Molecules, Compounds & Chemical Equations127
- Ch.4 - Chemical Quantities & Aqueous Reactions114
- Ch.5 - Gases103
- Ch.6 - Thermochemistry92
- Ch.7 - Quantum-Mechanical Model of the Atom50
- Ch.8 - Periodic Properties of the Elements89
- Ch.9 - Chemical Bonding I: The Lewis Model84
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory74
- Ch.11 - Liquids, Solids & Intermolecular Forces60
- Ch.12 - Solids and Modern Material50
- Ch.13 - Solutions90
- Ch.14 - Chemical Kinetics111
- Ch.15 - Chemical Equilibrium65
- Ch.16 - Acids and Bases135
- Ch.17 - Aqueous Ionic Equilibrium145
- Ch.18 - Free Energy and Thermodynamics92
- Ch.19 - Electrochemistry100
- Ch.20 - Radioactivity and Nuclear Chemistry68
- Ch.21 - Organic Chemistry121
Chapter 5, Problem 30b
Given a barometric pressure of 751.5 mmHg, calculate the pressure of each gas sample as indicated by the manometer.
(b)
Verified step by step guidance1
Identify the type of manometer used (open or closed) to determine how to relate the barometric pressure to the gas pressure.
If it's an open manometer, note the height difference (h) between the mercury levels in the two arms of the manometer.
For an open manometer, if the mercury level is higher on the side open to the atmosphere, the gas pressure is less than the atmospheric pressure. Use the formula: P_gas = P_atm - h.
If the mercury level is higher on the side connected to the gas, the gas pressure is greater than the atmospheric pressure. Use the formula: P_gas = P_atm + h.
Substitute the given barometric pressure (751.5 mmHg) and the height difference (h) into the appropriate formula to find the pressure of the gas sample.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Barometric Pressure
Barometric pressure is the pressure exerted by the weight of the atmosphere at a given point. It is commonly measured in units such as mmHg or atm. Understanding barometric pressure is essential for calculating the pressure of gases in various conditions, as it serves as a reference point for other pressure measurements.
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Pressure Units
Manometer
A manometer is a device used to measure the pressure of gases. It typically consists of a U-shaped tube filled with liquid, where the difference in liquid height between the two arms indicates the pressure of the gas relative to atmospheric pressure. Knowing how to read a manometer is crucial for determining the pressure of gas samples accurately.
Gas Laws
Gas laws describe the relationships between pressure, volume, temperature, and the number of moles of a gas. Key laws include Boyle's Law, which states that pressure and volume are inversely related at constant temperature, and Dalton's Law, which states that the total pressure of a mixture of gases is the sum of the partial pressures of each gas. These laws are fundamental for calculating the pressures of gas samples in various scenarios.
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Related Practice
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A syringe containing 1.55 mL of oxygen gas is cooled from 95.3 °C to 0.0 °C. What is the final volume of oxygen gas?
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Textbook Question
Given a barometric pressure of 751.5 mmHg, calculate the pressure of each gas sample as indicated by the manometer.
(a)
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Textbook Question
A 48.3-mL sample of gas in a cylinder is warmed from 22 °C to 87 °C. What is its volume at the final temperature?
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Textbook Question
The world record for lowest pressure (at sea level) was 652.5 mmHg recorded inside Typhoon Tip on October 12, 1979, in the western Pacific Ocean. Convert this pressure to each indicated unit. a. torr c. in Hg