CHEM 111 Chapter Notes - Chapter 11: Gas Laws, Jmol, Stoichiometry

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kurtzkm

13 Aug 2019

School

College of Charleston

Department

Chemistry and Biochemistry

Course

CHEM 111

Professor

Deavor

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Document Summary

Pressure is the force exerted on an object divided by the area over which the force is exerted. An apparatus used to measure atmospheric pressure. A common unit of pressure, defined as the pressure that can support a. A unit of pressure equivalent to 1 mm of mercury. 1 pa = 1 n / m 2. Boyle"s law states that the pressure and volume of a gas sample are inversely related when the amount of gas and temperature are held constant. Charles"s law states that the temperature and volume of a gas sample are directly related when the pressure and the amount of gas are held constant. V 1 / t 1 = v 2 / t 2. Avogadro"s hypothesis states that equal volumes of gases have the same number of particles when they are at the same temperature and pressure.

Related Questions

To understand several methods of measuring gas pressure. Gases exert a measurable pressure (P) on the walls of their container. The SI unit for pressure is the pascal (Pa). Other pressure units frequently used in chemistry are millimeters of mercury (mmHg) and atmospheres (atm). You can convert between units of pressure using conversion factors such as those indicated below. 1 atm=760 mmHg=101,325 Pa

Part A

On a rainy day, a barometer reads 737 mmHg . Convert this value to atmospheres.

Express your answer numerically in atmospheres

Part B

A closed container is filled with oxygen. The pressure in the container is 445 kPa . What is the pressure in millimeters of mercury?

Express the pressure numerically in millimeters of mercury.

Part C

What is the pressure (in atmospheres) of the gas inside the container connected to an open-end, mercury-filled manometer as shown in the picture? (Figure 1) The atmospheric pressure is 0.95 atm.

Express your answer numerically in atmospheres.

Converting between Units of Pressure Gases are different from solids and liquids. In a sample of gas, the molecules are far apart. The gas molecules also move around and collide with each other as well as with the walls of the container. These collisions generate pressure. The pressure of a gas can be measured in different units. One convenient unit of measure is called the atmosphere (atm) because it is based on atmospheric pressure. At sea level, the average pressure is 1 atm. As you get higher in altitude, the pressure steadily drops until you leave the atmosphere, where the pressure is very close to 0 atm. The table below shows the different commonly used units of measuring gas pressure. Use this table in the pressure unit conversions. Unit Abbreviation 1 atm equivalent atmosphere atm 1.00 atm (exact) millimeters of mercury mmHg 760 mmHg torr torr 760 torr inches of mercury in.Hg 29.9 in.Hg pounds per square inch (psi) lb/in.2 14.7 lb/in.2 pascal Pa 101,325 Pa.

Part C

High-pressure liquid chromatography (HPLC) is a method used in chemistry and biochemistry to purify chemical substances. The pressures used in this procedure range from around 500 kilopascals (500,000 Pa) to about 60,000 kPa (60,000,000 Pa). It is often convenient to know the pressure in torr. If an HPLC procedure is running at a pressure of 5.81Ã10⁸ Pa , what is its running pressure in torr?

Express the pressure numerically in torr.

CHEM 111 Chapter Notes - Chapter 11: Gas Laws, Jmol, Stoichiometry

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