WednesdayWednesdayFebruary 3, 2010February 3, 2010(Review for Test 7)(Review for Test 7)

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Notes: The Kinetic-Molecular Theory of Gases/Nature of Gases

1 1/20 1/27 2/3

WS: Introduction to Gases

7 1/21 1/28 2/4

Notes: Gases and Pressure

9 1/22 1/29 2/5

WS: Pressure 13 1/25 2/1 2/8

Notes: The Gas Laws

15 1/26 2/2 2/9

WS: Calculations Involving Gases

19 1/28 2/4 2/11

Review for Test 7

The Kinetic Molecular Theory of Gases

The Nature of Gases

Gases and Pressure

The Gas Laws

1The Kinetic-Molecular

Theory of Matter is based upon the idea that

particles of matter are always in motion.

What are the five basic assumptions of the Kinetic-Molecular Theory of Gases?

2

Gases consist of large numbers of tiny particles that are far apart relative to their size.

Collisions between gas particles and between particles and container walls are elastic collisions.Gas particles are in continuous, rapid, random

motion.There are no forces of attraction or repulsion

between gas particles.The average kinetic energy of gas particles

depends on the temperature of the gas.

3

The average kinetic energy of

gas particles depends upon the ________ of the gas.temperature

4Gas molecules are _______________ and ______________ than the molecules in

liquids and solids.moving faster

farther apart

5

Gas molecules will spread out and occupy their entire container

because of the property of ________.

expansion

6List four materials that are fluids and four that are not.

Fluids Not Fluids

Any liquid or any gas.

any solid

7What is the general trend in density of a substance as it passes through its three common phases?

The solid phase usually has the highest density, then the liquid phase, and the gas phase has the lowest

density.

8Which phase of matter

is the most compressible, and why?The gas phase is the most

compressible, because there is empty space between gas

particles that can be squeezed out.

9Which phase of matter

is the least compressible, and why?The solid phase is the least

compressible, because there is very little empty space between

solid particles that can be squeezed out.

10Give a good

example of the diffusion of a gas.Examples would be gas

particles that are bounced from one place to another by molecular motion of air molecules.

11 The force of the collisions

of gas particles against the inside walls of their

container is called _______.

pressure

12What are the standard

conditions for gas measurements?

1 atmosphere of pressure at a

temperature of 0oC

13450 torrs of pressure is

how many atmospheres?

0.59 atm

145.75 atmospheres of pressure is how many kilopascals?

583 kPa

1523.34 kilopascals of

pressure is how many atmospheres?

0.2303 atm

162.65 × 103 atm of

pressure is how many kPa?

2.69 × 105 kPa?

17 What is the value of

atmospheric pressure at sea level when the temperature is

0oC and the weather is neutral? Give your answer in five

different units. 760 mm Hg = 760 torr = 1 atm = 101325 Pa =

101.325 kPa

18 The pressure exerted on a 650. mL sample of oxygen gas at constant

temperature is increased from 0.325 atm to 0.675 atm. What will the final

volume of the sample be?Law? Formula

Boyle’s P1V1 = P2V2

V2 = 313 mL

19 A sample of oxygen gas has a volume of 660. mL at 35°C. At what temperature will its

volume be 750. mL?Law?

Formula Charles’ V1/T1 = V2/T2

T2 = 350 K

20 A sample of nitrogen gas at 46°C

exerts a pressure of 0.645 atm. The gas is heated to 76°C at constant

volume. What will its new pressure be?

Law? Formula

Gay-Lussac P1/T1 = P2/T2

P2 = 0.706 atm

21 A sample of fluorine gas at

17°C and 1.16 atm occupies a volume of 3.86 L. What

volume would this gas occupy at 66°C and 0.950 atm?

Law? Formula Combined P1V1/T1 = P2V2/T2

V2 = 5.50 L

22 What pressure, in

atmospheres, is exerted by 0.440 mol of hydrogen gas in a

4.00 L container at 45°C?

Law? Formula Ideal PV = nRT

P = 2.87 atm

23 How many moles of oxygen gas are there if the gas has a volume

of 5.60 L, a pressure of 1.75 atm, and a temperature of 35°C?

Law? Formula

Ideal PV = nRT n = 0.387 mol