Chapter 14 Test

Question 1

Liquid

Answer 1

• Shape: Takes shape of container
• Volume: Fixed
• Moderate space between particles

Question 2

Gas

Answer 2

• Shape: Takes shape of space
• Volume: Not fixed
• Great deal of space between particles

Question 3

Characteristics of Gases

Answer 3

• Expand to fill its container
• Volume of gas= to volume of its container
• Highly compressible (pressure applied, gas volume decreases)
• Form homogeneous mixtures (composition constant throughout)
• The motion of the particles in a gas are rapid, constant, and random
• Don’t travel in straight lines for long
• Take part in elastic collisions (little speed is lost)

Question 4

Kinetic Energy

Answer 4

-Energy an object has because of its motion

Question 5

Potential Energy

Answer 5

-Energy stored by a body by virtue of its position relative to others, stresses within itself, electric charge and other factors

Question 6

Assumptions for Kinetic Theory

Answer 6

• 1). Gas Particles have no volume (gas has volume)
• 2. Gas Particles relatively far apart (False because collide)
• 3. Between particles empty space (False, other particles of dif gases can be between them)
• 4.No attractive or repulsive forces exist between particles (Atoms have charges, can repel or attract)

Question 7

Factors which effect gases

Answer 7

• Temperature (K)
• Pressure (kPa)
• Volume (L)
• Amount of gas in moles (n)

Question 8

Pressure

Answer 8

• The amount of force applied to a surface
• Gas pressure results from force exerted by by gas particles per unit surface area as they collide with the walls of their container
• Equation: Pressure = force/ surface area

Question 9

Vacuum

Answer 9

-An empty space with no particles and no pressure

Question 10

What happens to gas particles when heated

Answer 10

• Potential energy increases (No effect on temp)

- Kinetic energy increases, particle movement increases (results in increase in temperature)

Question 11

Volume

Question 12

Pressure Units

Answer 12

• kPa (Kilopascal)
• 1 torr= .13332 kPa
• STP: 101.3 kPa

Question 13

Temperature Units

Answer 13

• K (Kelvin)
• K= C + 273
• C= K-273
• STP: 273 K

Question 14

Volume Units

Answer 14

• L (Liters)

- 1,000 ml = 1 Liter

Question 15

Boyle’s Law

Answer 15

• Temp & # of particles = constant
• Volume & pressure= changing
• Inversely proportional
• Equation: P1V1=P2V2

Question 16

Charles Law

Answer 16

• Temp & Volume= Changing
• Number of particles & Pressure= Constant
• Directly proportional
• V1/T1=V2/T2

Question 17

Gay-Lussac’s Law

Answer 17

• Temp & Pressure= Changing
• Number of Particles & Volume= Constant
• Directly Proportional
• Equation= P1/T1=P2/T2

Question 18

Combine Gas Law

Answer 18

Equation: P1V1/T1= P2V2/T2

Question 19

Gas Constant

Answer 19

-8.31 LkPa/ Kmoles

Question 20

Ideal Gas

Answer 20

• A hypothetical gas hose molecules have no volume and no attraction to other molecules
• At common temp, difference so small it can be ignored

Question 21

Ideal Gas Equation and meaning

Answer 21

• PV= nRT
• P= Pressure in kPa
• V= molar volume (1 mole= 22.4 Liters)
• n= number of moles
• R= Gas constant
• T= Temperature in K

Question 22

Acid

Answer 22

-Any substance that when added to water increases the H3O+ ion concentration in a solution

Question 23

Base

Answer 23

-Any substance that when added to water increases the OH- concentration in a solution (Caustic)

Question 24

Example of Acid & Base

Answer 24

-Water

Question 25

Neutral Solution, Acidic Solution, Basic Solution

Answer 25

• [H3O+] > [OH-] Acidic

- [H3O+]

Question 26

Molarity Equation

Answer 26

-Molarity = moles of compound or ion/ Liters of solution

Question 27

PH Scale

Answer 27

• exponential (10’s)
• Neutral= 7
• Acidic= Lower than 7
• Basic= Higher than 7
• Easier to understand than molarity

Question 28

pH equation

Answer 28

pH= -Log [H3O+]

OR -Log [M]

Question 29

Solid

Answer 29

• Shape: Fixed
• Volume: Fixed
• Little space between particles

Question 30

Tirtation Equation

Answer 30

M1V1=M2V2