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Ch.5 - Gases
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook
All textbooksTro 4th EditionCh.5 - GasesProblem 30a
Chapter 5, Problem 30a

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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1
Identify the type of manometer used (open or closed) to determine how to relate the manometer reading to the barometric pressure.
If it's an open manometer, determine whether the gas pressure is greater or less than the atmospheric pressure by observing the height difference in the manometer.
For an open manometer, if the gas pressure is greater than atmospheric pressure, add the height difference to the barometric pressure. If less, subtract the height difference from the barometric pressure.
If it's a closed manometer, the gas pressure is equal to the height difference since there is no atmospheric pressure to consider.
Use the appropriate formula based on the type of manometer to calculate the gas pressure. For open: \( P_{gas} = P_{atm} \pm h \), and for closed: \( P_{gas} = h \).

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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 millimeters of mercury (mmHg) and is crucial for understanding how gases behave under different atmospheric conditions. In this context, the barometric pressure of 751.5 mmHg serves as a reference point for calculating the pressure of gas samples in a manometer.
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Manometer

A manometer is a device used to measure the pressure of gases. It typically consists of a U-shaped tube filled with liquid, often mercury, where the difference in liquid height between the two arms indicates the pressure of the gas relative to atmospheric pressure. Understanding how to read a manometer is essential 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 of Partial Pressures, which states that the total pressure of a gas mixture is the sum of the partial pressures of its individual gases. These principles are vital for calculating the pressures of gas samples in relation to the given barometric pressure.
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Related Practice
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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Textbook Question

Given a barometric pressure of 751.5 mmHg, calculate the pressure of each gas sample as indicated by the manometer.

(b)

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Textbook Question

The North American record for highest recorded barometric pressure is 31.85 in Hg, set in 1989 in Northway, Alaska. Convert this pressure to each indicated unit. a. mmHg

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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