CHMA10H3 Chapter Notes - Chapter 5: Ideal Gas Law, Molar Volume, Mole Fraction

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CHMA10H3 Full Course Notes

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Topic 5. 2: pressure- the result of molecular collisions. The result of the constant collisions between the atoms or molecules in a gas and the surface around them is due to pressure. Thanks to pressure, it allows us to drink from straws, inflate basketballs, move air into and out of our lungs. Depends on factors such as the # of gas particles in a given volume (fewer gas particles, lower the pressure) Low density= low pressure, high density= high pressure. Common unit of pressure: mmhg (often called a torr) and measured with a barometer. Sl unit of pressure is the pascal (pa) 101 325 pa=101. 325 kpa=760 torr= 1 atm. U-shaped tube containing a dense liquid (use to measure the pressure of a gas) Always measured pressure of a gas relative to atmospheric pressure. Height difference indicates pressure of gas relative to atmospheric pressure. Hypertension may include obesity, high sodium intake, high alcohol intake, lack of exercise, stress, etc.

Related Questions

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.

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.

CHMA10H3 Chapter Notes - Chapter 5: Ideal Gas Law, Molar Volume, Mole Fraction

CHMA10H3 Full Course Notes

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