Chapter 14 Test Flashcards
Liquid
- Shape: Takes shape of container
- Volume: Fixed
- Moderate space between particles
Gas
- Shape: Takes shape of space
- Volume: Not fixed
- Great deal of space between particles
Characteristics of Gases
- 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)
Kinetic Energy
-Energy an object has because of its motion
Potential Energy
-Energy stored by a body by virtue of its position relative to others, stresses within itself, electric charge and other factors
Assumptions for Kinetic Theory
- 1). Gas Particles have no volume (gas has volume)
- Gas Particles relatively far apart (False because collide)
- 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)
Factors which effect gases
- Temperature (K)
- Pressure (kPa)
- Volume (L)
- Amount of gas in moles (n)
Pressure
- 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
Vacuum
-An empty space with no particles and no pressure
What happens to gas particles when heated
- Potential energy increases (No effect on temp)
- Kinetic energy increases, particle movement increases (results in increase in temperature)
Volume
Pressure Units
- kPa (Kilopascal)
- 1 torr= .13332 kPa
- STP: 101.3 kPa
Temperature Units
- K (Kelvin)
- K= C + 273
- C= K-273
- STP: 273 K
Volume Units
- L (Liters)
- 1,000 ml = 1 Liter
Boyle’s Law
- Temp & # of particles = constant
- Volume & pressure= changing
- Inversely proportional
- Equation: P1V1=P2V2
Charles Law
- Temp & Volume= Changing
- Number of particles & Pressure= Constant
- Directly proportional
- V1/T1=V2/T2
Gay-Lussac’s Law
- Temp & Pressure= Changing
- Number of Particles & Volume= Constant
- Directly Proportional
- Equation= P1/T1=P2/T2
Combine Gas Law
Equation: P1V1/T1= P2V2/T2
Gas Constant
-8.31 LkPa/ Kmoles
Ideal Gas
- A hypothetical gas hose molecules have no volume and no attraction to other molecules
- At common temp, difference so small it can be ignored
Ideal Gas Equation and meaning
- 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
Acid
-Any substance that when added to water increases the H3O+ ion concentration in a solution
Base
-Any substance that when added to water increases the OH- concentration in a solution (Caustic)
Example of Acid & Base
-Water
Neutral Solution, Acidic Solution, Basic Solution
- [H3O+] > [OH-] Acidic
- [H3O+]
Molarity Equation
-Molarity = moles of compound or ion/ Liters of solution
PH Scale
- exponential (10’s)
- Neutral= 7
- Acidic= Lower than 7
- Basic= Higher than 7
- Easier to understand than molarity
pH equation
pH= -Log [H3O+]
OR -Log [M]
Solid
- Shape: Fixed
- Volume: Fixed
- Little space between particles
Tirtation Equation
M1V1=M2V2
