CHEM 142 Study Guide - Midterm Guide: Van Der Waals Equation, Kinetic Theory Of Gases, Ideal Gas Law

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2 Feb 2017

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Document Summary

Pressure: the force exerted per unit area by gas particles as they strike the surfaces around them; the result of the constant collisions between the atoms or molecules in a gas and the surfaces around them. Force: the pressure that a gas sample exerts that results form the collisions of gas particles. Millimeter of mercury (mmhg): a common unit of pressure; originates from how pressure is measured with a barometer. Barometer: an evacuated glass tube, the tip of which is submerged in a pool of mercury. Torr: the unit millimeter of mercury; named after the inventor of the barometer. Atmosphere (atm): unit of pressure; the average pressure at sea level; is about 760 mmhg. Pascal (pa): si unit of pressure; defined as 1 newton (n) per square meter. Boyle"s law: a law stating that the pressure of a given mass of an ideal gas is inversely proportional to its volume at a constant temperature; v 1/p; p1v1 = p2v2.

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 142 Study Guide - Midterm Guide: Van Der Waals Equation, Kinetic Theory Of Gases, Ideal Gas Law

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