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Chapter 11: Problem 6

Which of the following statement(s) describes the pressure of a gas? a. the temperature of the gas b. the volume of the container c. \(3.00 \mathrm{~atm}\) d. \(0.25 \mathrm{~mol}\) of \(\mathrm{O}_{2}\) e. \(101 \mathrm{kPa}\)

Short Answer

Expert verified
Options c (3.00 atm) and e (101 kPa) describe the pressure of a gas.

Step by step solution

01

Understand the Definition of Pressure

Pressure of a gas is defined as the force that the gas exerts on the walls of its container per unit area. It is usually measured in units like atmospheres (atm), Pascals (Pa), or kilopascals (kPa).
02

Analyze Each Statement

Go through each option to determine if it directly describes the pressure of the gas.
03

Evaluate Statement a

Option a states 'the temperature of the gas'. This describes the thermal state of the gas, not its pressure. Therefore, option a does not describe pressure.
04

Evaluate Statement b

Option b states 'the volume of the container'. This describes the space in which the gas is contained, not its pressure. Therefore, option b does not describe pressure.
05

Evaluate Statement c

Option c states '3.00 atm'. This directly describes a pressure value. Therefore, option c does describe pressure.
06

Evaluate Statement d

Option d states '0.25 mol of O鈧�'. This describes the amount of substance, not its pressure. Therefore, option d does not describe pressure.
07

Evaluate Statement e

Option e states '101 kPa'. This directly describes a pressure value. Therefore, option e does describe pressure.
08

Conclusion

Summarize the options that describe the pressure of a gas.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Pressure Units
Pressure is a measurement of the force exerted by a gas per unit area. It helps understand how much push or pull the gas molecules create when they hit the container walls. Units used to measure pressure come in different forms:
  • Atmospheres (atm): One atmosphere is the pressure exerted by the air at sea level.
  • Pascals (Pa): This is a metric unit of pressure. One Pascal equals one Newton per square meter. KiloPascals (kPa) are more common because Pascal is a small unit.
  • Millimeters of mercury (mmHg): Used in medical and scientific fields, commonly used in blood pressure readings.
For example, in our exercise: '3.00 atm' and '101 kPa' both represent units of pressure. They tell us how much force the gas is exerting in different units.
Gas Laws
Gas laws describe how gases behave under various conditions. They relate temperature, volume, pressure, and the number of gas particles together using mathematical relationships:
  • Boyle's Law: It states that the pressure of a gas is inversely proportional to its volume when temperature is constant. It means if you compress the gas, the pressure increases.
  • Charles' Law: This law says the volume of a gas is directly proportional to its temperature, provided the pressure is constant. If you heat the gas, it expands.
  • Avogadro's Law: It states that the volume of a gas is directly proportional to the number of gas particles (moles) when temperature and pressure are constant. More gas molecules mean a larger volume.
Understanding these laws helps us see why neither the temperature (option a) nor the volume (option b) alone can describe the pressure of a gas. Instead, these factors can influence pressure.
Measurement of Pressure
To measure gas pressure, various instruments exist, ensuring accurate readings:
  • Manometer: Measures the pressure of gas in a closed system. It usually has a U-shaped tube with mercury. Reading the level difference between the two sides gives the pressure.
  • Barometer: Measures atmospheric pressure. Like a manometer, it uses mercury and a glass tube but is used for open air environments.
  • Digital sensors: Modern tools can provide precise pressure readings in various units and are common in labs and industrial applications.
In our exercise, 'c. 3.00 atm' and 'e. 101 kPa' are specific readings that you could get using such instruments. They accurately describe the gas pressure directly.

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Most popular questions from this chapter

Calculate the final pressure, in atmospheres, for each of the following, with \(n\) and \(V\) constant: a. A gas with an initial pressure of \(1.20\) atm at \(75^{\circ} \mathrm{C}\) is cooled to \(-22{ }^{\circ} \mathrm{C}\). b. A sample of \(\mathrm{N}_{2}\) with an initial pressure of \(780 . \mathrm{mmHg}\) at \(-75^{\circ} \mathrm{C}\) is heated to \(28^{\circ} \mathrm{C}\).

A scuba diver \(60 \mathrm{ft}\) below the ocean surface inhales \(50.0 \mathrm{~mL}\) of compressed air from a scuba tank at a pressure of \(3.00\) atm and a temperature of \(8{ }^{\circ} \mathrm{C}\). What is the final pressure of air, in atmospheres, in the lungs when the gas expands to \(150.0 \mathrm{~mL}\) at a body temperature of \(37^{\circ} \mathrm{C}\), and the amount of gas remains constant?

Glucose, \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\), is metabolized in living systems. How many grams of water can be produced from the reaction of \(18.0 \mathrm{~g}\) of glucose and \(7.50 \mathrm{~L}\) of \(\mathrm{O}_{2}\) at \(1.00 \mathrm{~atm}\) and \(37^{\circ} \mathrm{C}\) ? \((9.2,9.3,11.8,11.9)\) $$ \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(s)+6 \mathrm{O}_{2}(g) \longrightarrow 6 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) $$

In the formation of \(\mathrm{smog}\), nitrogen and oxygen gas react to form nitrogen dioxide. How many grams of \(\mathrm{NO}_{2}\) will be produced when \(2.0 \mathrm{~L}\) of nitrogen at \(840 \mathrm{mmHg}\) and \(24^{\circ} \mathrm{C}\) are completely reacted? \((11.8,11.9)\) \(\mathrm{N}_{2}(g)+2 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)\)

Your spaceship has docked at a space station above Mars. The temperature inside the space station is a carefully controlled \(24{ }^{\circ} \mathrm{C}\) at a pressure of \(745 \mathrm{mmHg}\). A balloon with a volume of \(425 \mathrm{~mL}\) drifts into the airlock where the temperature is \(-95^{\circ} \mathrm{C}\) and the pressure is \(0.115\) atm. What is the final volume, in milliliters, of the balloon if \(n\) remains constant and the balloon is very elastic? \((11.6)\)
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