Shared Flashcard Set

Details

AP Chem: States of Matter
Focus on solid, liquids and gases
52
Chemistry
12th Grade
11/02/2010

Additional Chemistry Flashcards

 


 

Cards

Term
What is the pressure exerted by 5 moles of gas in a 40 L container at 300 K?
Definition
Using the ideal gas equation, you can calculate the pressure exerted by the gas is about 3.1 atm.
Term
How many atoms of a substance are in 1 mole of that substance?
Definition
In 1 mole of a given substance, there are                   6.022 x 1023 atoms.
Term
On the periodic table, the masses given for the elements are masses for what quantity of the element?
Definition
The masses given for the elements are for 1 mole of the element. 
Term
Polar substance will only dissolve what other type of substances?
Definition
Other polar substances
Term
In order for a solvent to dissolve a solute, what must be overcome? 
Definition
In order for a solvent to dissolve a solute, intermolecular forces must be overcome. 
Term
What is the freezing point depression equation?
Definition
Tfkf msolute
Term
  1. Physical Change
  2. Chemical Change
Definition
  1. Substance changes form or state only. Boiling, melting, freezing, dissolving, grinding, cutting
  2. Where new substances are formed with new chemical and physical properties. Oxygen and hydrogen form water; sodium and chlorine form salt (sodium chloride)
Term
List the three states if matter in order of increasing density
Definition

Gas: neither definite shape nor volume

 

Liquid: definite volume; takes shape of container

 

Solid: definite size and shape

Term

Phase

Two examples

Definition

A sharply defined, uniforme region in a mixture.

 

Examples- oil and vinegar in salad dressing; ice and water in a frozen pond

Term

Density

General equation and three standard units

Definition

The mass of a unit volume of a substance.

 

Density = mass/volume

 

g/mL g/L kg/L

Term
Calculate the density of a rock with mass = 10g and volume = 5mL
Definition

Density = mass/volume

 

density 10 g/5 mL = 2 g/mL

Term

Element

List some examples

Definition

A substance composed of identical atoms.

 

gold, silver, oxygen, hydorgen, lead, chlorine, helium, iron, copper, fluorine, arsenic

Term

Compound

List some examples

Definition

Substance composed of two or more different elements chemically combined. For example:

Water - H2O

Salt - NaCl

Sugar - C6H12O6

Ammonia - NH3

Term

Mixture

List some examples

Definition

A combination of substaces held together by physical means.

(Dirt, milk, soup, saltwater, granite)

Term

Homogenous ang heterogenous Mixture

Give example

Definition

Homogeneous mixtures are uniforme in composition. (Air, metal, alloy, salt water)

Hetergeneous mixtures are not uniform in composition. (Dirt, spaghetti sauce)

Term

Symbols for:

  1. Barium
  2. Beryllium
  3. Platinum
  4. Arsenic
  5. Tin
Definition
  1. Ba
  2. Be
  3. Pt
  4. As
  5. Sn
Term

Symbols for:

  1. Sodium
  2. Potassium
  3. Calcium
  4. Hydrogen
  5. Magnesium
Definition
  1. Na
  2. K
  3. Ca
  4. H
  5. Mg
Term

Names for:

  1. Fe
  2. Co
  3. Ni
  4. Cu
  5. Zn
Definition
  1. Iron
  2. cobalt
  3. Nickel
  4. Copper
  5. Zinc
Term

Symbols for:

  1. Silver
  2. Gold
  3. Mercury
  4. Aluminum
  5. Lead
Definition
  1. Ag
  2. Au
  3. Hg
  4. Al
  5. Pb
Term

Names for:

  1. C
  2. Si
  3. N
  4. P
  5. O
Definition
  1. Carbon
  2. Silicon
  3. Nitrogen
  4. Phosporous
  5. Oxygen
Term

Symbols for:

  1. Sulfur
  2. Fluorine
  3. Chlorine
  4. Bromine
  5. Iodine
Definition
  1. S
  2. F
  3. Cl
  4. Br
  5. I
Term

Names for:

  1. He
  2. Ne
  3. Ar
  4. Kr
Definition
  1. Helium
  2. Neon
  3. Argon
  4. Krypton
  5. Uranium
Term
Einstein's law of conservation of energy
Definition

The sum-total of mass and energu remains constant in a reaction but mass and energy may be interconverted.

E = mc2

E= energy; m = mass

c= speed of light

Term

Identify as element, compound, or mixture

Sand, air, gold, water, salt, hydrogen

Definition

Sand - mixture

Air - mixture

Gold - element

Water - compound

Salt - compound

Hydrogen - element

Term
  1. Physical Properties
  2. Chemical properties
Definition
  1. Properties which can be observed without changing the substance into something different. Color, odor, hardness, density, luster, state, conductivity, solubility, boiling and melting points.
  2. A chemical property is observed when a substance changes into a new substance. Iron forms rust in air and water; gasoline burns in oxygen.
Term

PRESSURE

Write Normal Atmospheric Pressure in Five Standard Units

 

Definition

Pressure is force per unit of area

 

1 atmosphere= 760 torr

= 760 mm Hg

= 101.3 kilopasca;s

= 14.7 pounds/square inch

Term
  1. Barometer
  2. Manometer
Definition
  1. An instrument, invented by torricelli in 1643, which measures atmospheric pressure. An evacuated glass tube in which a column of mercury rises or falls with change in pressure.
  2. An instrument used to measure pressure of gases in a closed container.
Term

State three postulates of:

The Kinetic

Molecular

Theory of gases

Definition
  1. Matter is composed of very small particles; a gas is mostly empty space.
  2. Particles are in constant random motion.
  3. Collisions are elastic
Term

State the formula for Graham's Law of Diffusion.Do heavy or light gases diffuse faster?

Definition

A mixture of a gas A & B:

(RA)(MWA)1/2 = (RB)(MVB)1/2

MWA,MWB = Molecular weights

RA, RB = Rates of Diffusion

(Light gases diffuse faster)

Term

Charles' Law

Definition

V1/T1 = V2/T2

Pressure and amount of gas are constant

V = volume

T = Kelvin

Term

At 300 K a gas has a volume of 10 liters. Find the volume at 400 K

Definition

Use Charles' Law,

V1/T1 = V2/T2

10/300 = V2/400

V2 = 13.3 L

Term

Boyle's Law

Definition

P1 x V1 = P2 x V2

Pressure and volume are inverse if temperature and amount of gas are constant

P = pressure

V = volume

Term

A sample of gas has a volume of 23 L at 800 torr. find the volume at 400 torr.

Definition

Use Boyle's Law

P1 x V1 = P2 x V2

25 x 800 = 400 x V2

V2 = 50 L

Term
Combined Gas Law
Definition

P1V1/T1 = P2V2/T2

Amount of gas is constant

P = pressure

V = volume

T = kelvin

Term

Dalton's Law of Partial Pressure

Definition

In a gas mixture, the total pressure equals the sum of the partial pressures of each component

Ptotal = P1 + P2 + P3 ...

Term

Ideal Gas Law

Definition

PV = nRT

P = pressure (Atmospheres)

V = volume (Liters)

n = # of Moles

R = 0.0820 L-ATM/MOL-K

T = temperature in K

Term

How many moles of H2 gas are there in 20 L at 4 atm and 400 K?

Definition

Use the Ideal Gas Law

PV = nRT

 

(4 atm)(20 L) = n(0.082)(400)

n = 2.44 moles

Term
  1. STP
  2. Gay-Lussac's Law of Combining Gas Volume
Definition
  1. Standard temperature (0° C or 273 K) and standard pressure (1 atmosphere or 760 torr)
  2. When only gases are involved in a reaction, the volumes of reactants and product are in a small, whole number ratio.
Term
  1. Avogadro's Law (regarding gases)
  2. What is the volume of 1 mole of any gas at STP
Definition
  1. Under the same conditions of temperature and pressure; equal volumes of gases contain equal numbers of moles.
  2. 22.4 L
Term

N2 + 3H2 ↔ 2NH3

In the above reaction how many L of NH3 will be produced from 6L H2

 

Definition

According to Gay-Lussac's Law the volumes of gases are in direct proportion to the coefficients in the equation.

H2 : 3/6 L = NH3 : 2/x

x = 4L of ammonia

 

Term

Sublimation

Definition

The change from a solid to a vapor without the forming of a liquid

Compounds which show sublimation

(CO2, I2)

Term

Describe a phase change from liquid to gas

Definition

When a molecule gains enough kinetic energy to overcome the intermolecular attractive forces within a liquid, it escapes the surface and becomes gas.

Term
  1. Phase equilibrium
  2. Dynamic equilibrium
Definition
  1. For a liquid in a closed container; when the rates of evaporation (liquid to gas) and condesation (gas to liquid) equalize: the concentration of each is stable.
  2. In a closed container where opposing changes are taking place at equal rates; the concentration of all components remains constant.
Term

Normal Boiling Point

Definition

The temperature at which a liquid phase becomes a gas phase when vapor reaches atmospheric pressure.

Pressure = 1 atm

Term

Define:

  1. Critical temperature
  2. Critical pressure
Definition
  1. The temperature above which the liquid phase of a substance can no longer exist.
  2. Minimum pressure required to liquify a gas at its critical temperature
Term

Melting Point

Definition

The temperature at which the solid and liquid phases co-exist

Term
  1. Heat of fusion (value for water)
  2. Heat of vaporization (value for water)
Definition
  1. The amount of energy required to change a gram of substance from liquid at its melting point. (Water - 80 calories/gram)
  2. The amount of energy required per gram to change a liquid to gas at its boiling point. (Water - 540 calories/gram)
Term
  1. Triple point
  2. Vapor pressure
Definition
  1. The only temperature and pressure combination at which the 3 phases of a substance (solid, liquid and gas) can co-exist at equilibrium
  2. The pressure the gas phase exerts on its liquid phase in a close container. This pressure varies with temperature.
Term

Define boiling point in terms of vapor pressure

Definition

The temperature at which the vapor pressure over a liquid reaches atmospheric pressure. The substance boils (liquid to gas)

Term
  1. How much heat is required to change 10 grams of water to steam at 100° C
  2. How much heat is required to melt 0.5 grams of ice at 0° C
Definition
  1. Heat of vaporization of water is 540 cal/g

10g x 540 cal/g = 5400 cal

 

2. Heat of fusion of water is 80 cal/gram

(0.5 grams)(80 cal/gram) = 40 cal

Supporting users have an ad free experience!