Chem 4 Exam

Front 1

Pressure-

Back 1

Force applied in an area. Gas exerts pressure from the collision of atoms .

Front 2

Diffusion-

Back 2

Property of a gas going from area of greater concentration to area of lesser concentration often mixing with other gases.

Front 3

Barometer-

Back 3

Measures atmospheric pressure. Uses a column of Hg inverted in an open dish of Mercury to determine pressure

Front 4

Standard Conditions-

Back 4

STP
Temp= 0 C & 1 atm=760 torr

Front 5

Ideal gas-

Back 5

One that behaves exactly as KMT predicts, but no gas is exactly ideal.

Front 6

atmospheric pressure-

Back 6

Pressure exerted by the mix of gases in the atmosphere.

Front 7

one atmosphere-

Back 7

The pressure exerted by by a column of Hg 760 mm high @ a temp of 0 C
1 atm= 760 torr=760 mm Hg
1 atm= 1013 millibar=29.9 in.

Front 8

molar volume-

Back 8

volume occupied by 1 mole of a substance at STP.
1 mole= 22.4 L

Front 9

What are the principle assumptions of kinetic molec. theory?

Back 9

1. Gases consist of tiny particles
2. Distances b/t particles are large relative to size of particles
3. Gas parts have no attraction to each other
4. Gas parts move in straight lines in all directions w/ frequent collisions
5. No energy is lost in collisions
6. Avg. KE for parts is same for all gases at the same temp. & is proportional to the Kelv. temp.

Front 10

How does gas exert pressure?

Back 10

Results from the collision of atoms on the surface of a container.

Front 11

How does a barometer work?

Back 11

when pressure increases the barometer goes up.

Front 12

What is 1 atm in mm of Hg, inches of Hg, torr, & lbs/in.

Back 12

1 atm= 760mm Hg
29.9 in.
760 torr
14.7 lbs/in
1013 millibar

Front 13

Boyles Law?

Back 13

At constant temp. the volume of a fixed mass of gas is inversely proportional to the pressure
(pressure increase- volume decrease)
P1 V1= P2 V2

Front 14

Charles Law?

Back 14

@ cp, the volume of affixed mass of any gas is directly prop. to the absolute temp.
(V1/T1 = V2/T2)

Front 15

Gay-Lussac's Law?

Back 15

States that the pressure of a fixed mass of a gas at constant volume is directly prop. to the Kelvin temp.
(P1/T1= P2/T2)

Front 16

Density of an Ideal gas?

Back 16

D= m/v (in g/L) at STP L=22.4

Front 17

Dalton's Law of Partial Pressures?

Back 17

The pressure of a mixture of gases is the sum of the partial pressures exerted by each of the gases in the mixture.
Patm= Po2 + Pn2 + Par + P other

Front 18

Avogadros Law?

Back 18

Equal volumes of diff. gases at the same temp. & press. contain the same # of molecules.

Front 19

Ideal Gas?

Back 19

any gas that behaves according the Kinetic Molecular theory.

Front 20

What are 2 reasons why real gases may no behave as an ideal gas?

Back 20

1. High pressure- compress to liquid
2. Low temp.- slow down and freeze

Front 21

What is the ideal gas equation?

Back 21

V= nRT/P
(V is in L, n is moles, T is temp in K, P in atm, R is 0,0821

Front 22

Melting point-

Back 22

where the solid phase of liquid is in equilibrium w/ its liquid phase.
*temp remains same until completely melted
*changes only slightly w/ pressure unless very large

Front 23

normal boiling point-

Back 23

Boiling point (temp when vapor press of liquid is = ext. press above liquid) at STP
*higher pressure = higher temp

Front 24

heat of fusion-

Back 24

Amount of heat needed to change 1 g of solid to liquid

Front 25

heat of vaporization-

Back 25

Amount of heat needed to change 1 gram of liquid to gas

Front 26

specific heat-

Back 26

1 gram of water needs 418J or 100 cal to heat from 0- 100 C

Front 27

Density @ 4 C of water-

Back 27

1 g/mL

Front 28

Describe water molecule w/ respect to electron dot config & polarity?

Back 28

Bent molecule w/ angle of 105 between 2 H's coming of O.
*Bonds are polar covalent, giving rise to the polar nature of molecule.

Front 29

Explain the effect of Hydrogen bonding on the physical prop. of water?

Back 29

Causes a higher melting & boiling point. More energy is required to break apart bonds.
*Gives water a large specific heat capacity

Front 30

Complete & balance equations for acid-base neutralization

Back 30

on notes; p. 26

Front 31

Given a list of hydrates, write balanced equations for their reactions w/ water.

Back 31

CuSO4 x 5H2O --> CuSO4 + 5H2O

Front 32

Discuss occurrenes of ozone & its effects on humans?

Back 32

car emissions & some cities; makes breathing more difficult b/c molecules get deeper in lungs.

Front 33

solution-

Back 33

Systems of 1 or more substances dissolved or homogenously mixed in another substance.

Front 34

solvent-

Back 34

The dissolving agent & most abundant solution.

Front 35

miscible-

Back 35

Capable of mixing & forming a homogenous mixture

Front 36

dilute solution-

Back 36

Solution that contains small amt. of dissolved solute

Front 37

concentrated solution-

Back 37

Contains a large amt. of dissolved solute

Front 38

saturated solution-

Back 38

Has the max amt of solute dissolved in solvent for a given temp. (limit reached)

Front 39

mass-percent-

Back 39

Mass of solute divided by the total mass of solute & solvent x 100

Front 40

normality-

Back 40

?

Front 41

solute-

Back 41

the dissolved or least abundant substane.

Front 42

solubility-

Back 42

The amt. of solute that will dissolve in a specified amt of solvent at a specified temp.

Front 43

immiscible-

Back 43

Incapable of mixing to form a homogenous mixture.

Front 44

concentration of solution-

Back 44

Describes the quantity of solute to dissolve in a quantity of solvent.

Front 45

unsaturated solution-

Back 45

Has less solute than is needed to reach saturation (limit not reached)

Front 46

supersaturated solution-

Back 46

solution has more solute dissolved that the saturated solution (can precipitate from solution)

Front 47

molarity-

Back 47

The moles of solute in 1 L of solution.

Front 48

Qualitatively predict the effect of temp. change on the solubility of solids & gases in liquids?

Back 48

Solids will dissolve better in heat while gases are the opposite.

Front 49

Calc. mass % of solution

Back 49

Mass of solute/total mass x 100

Front 50

Salt-

Back 50

crystalline resulting from acid&base that has high melting & boiling pt. & consists of + charged metal & - charged nonmetal

Front 51

amphoteric-

Back 51

Base in the presence of acid & acid in presence of base

Front 52

nonelectrolyte-

Back 52

substances which in solution do not conduct electricity

Front 53

ionization-

Back 53

Formation of ions

Front 54

weak electrolyte-

Back 54

Don't ionize well

Front 55

pH-

Back 55

extends from 0-14
<7 is acidic
7 is neutral
>7 is basic

Front 56

neutralization-

Back 56

Of an acid & base forms salt & water

Front 57

spectator ions-

Back 57

Do not react in solution (stay dissolved)

Front 58

Hydronium ions-

Back 58

Proton associated with water molecule (H3O)

Front 59

electrolyte-

Back 59

Substances which in solution conduct electricity.

Front 60

dissociation-

Back 60

The separation of ions when placed in a solution.

Front 61

strong electrolyte-

Back 61

Ionize almost completely

Front 62

titration-

Back 62

process of using a known concentration of 1 reagent to neutralize an unknown conc. of a 2nd reagent using a pH indicator.

Front 63

Arrhenius acid-

Back 63

produces H+ ions in solution

Front 64

Arrhenius base-

Back 64

produces OH- in solution

Front 65

Bronsted-Lowery acid-

Back 65

proton donor

Front 66

Bronsted-Lowery base-

Back 66

proton acceptor

Front 67

Lewis acid

Back 67

electron pair acceptor

Front 68

Lewis base

Back 68

electron pair donor

Front 69

Relate pH & Hydrogen ion concentration?

Back 69

[H+] = 1 x 10 -3.6
pH= 3.6