Exam 2 study deck

Question 1

Pressure

Answer 1

Force/Area

Question 2

Boyles Law

Answer 2

P1V1=P2V2

Question 3

Charles Law

Answer 3

V1/T1=V2/T2 (volume/time)

Question 4

Gay -Lussac’s Law

Answer 4

P1/T1=P2/T2(pressure/time)

Question 5

Combined Gas Law

Answer 5

P1V1/T1=P2V2/T2

Question 6

Avagadro’s Law

Answer 6

V1/n1=V2/n2 (volume/ moles)

Question 7

STP condition

Answer 7

exactly 0”C (273 K)
exactly 1 atm (760 mmHg)
at STP one mole of any gas occupies 22.4 L=molar volume

Question 8

Ideal Gas Law

Answer 8

PV=nRT

Question 9

R=?

Answer 9

.0821Latm/moleK

Question 10

Dalton’s Law

Answer 10

Ptotal=p1+p2+p3……Pn

Question 11

Solubility

Answer 11

grams of solute/ 100 grams of solvent

Question 12

Soluble

Answer 12

Li+,Na+, K+, NH4+, NO3-,C2H3O2-, Cl-, Br-, I-, SO4^2-

Question 13

Insoluble

Answer 13

Ag+, Pb2+, or HG2^2+, Ba2+, Pb2+, Ca2_, Sr2+, CO3^2-, S2-, PO4^3-, OH-

Question 14

mass percent(m/m)

Answer 14

mass of solute(g)/Mass of solute(g)+mass of Solvent(g)

Question 15

volume Percent(v/v)

Answer 15

volume of solute/volume of solution

Question 16

Mass volume percent (m/v)

Answer 16

grams of solute/milliliters of solution

Question 17

Molarity (M) concentration

Answer 17

Moles of solute/liters of solution

Question 18

Dilution

Answer 18

C1V1=C2V2

Question 19

Colloids

Answer 19

large molecules too large for semi-permiable membrains(homogenious)

Question 20

Suspentions

Answer 20

heterogeneous nonuniform very lare particles that may be visible

Question 21

Changes in Freezing point

Answer 21

1 mole=-1.86’C change

Question 22

Changes in boiling point

Answer 22

1 mole=.52’C change

Question 23

in a solution with a semi-permiable membrane where will the water go

Answer 23

to the side with the higher concentration

Question 24

hypotonic

Answer 24

lower solute concentration

Question 25

hypertonic

Answer 25

higher solute concentration

Question 26

collision theory

Answer 26

reactions take place only when mollecules collide with propper oreintation and with sufficient energy

Question 27

rate of reaction

Answer 27

change in concentration of reactant or product/ change in time

Question 28

as you go higher what happens to the boiling temperature

Answer 28

it decreases

Question 29

conditions required for reaction

Answer 29

1. collision
2. orientation
3. energy

Question 30

how does a catalyst speed up a reaction?

Answer 30

it lowers activation energy

Question 31

Kc (equilibrium constant)

Answer 31

[products]/[reactants] (raised to their coefficients) (only gasses are in equation)

Question 32

Homogeneous equilibrium and Heterogeneous Equilibrium

Answer 32

Homo: Gasses Hetero: two or more states

Question 33

Equilibrium with large Kc

Answer 33

forward reaction produced a lare amoung of poducts when equillibrium is reached

Question 34

Equilibrium with small Kc

Answer 34

has few products and is mostly reactants

Question 35

Le Chatliers Principle

Answer 35

when a system at equilibrium is disturbed the system will shift in the direction that will reduce stress

Question 36

Condition: Endothermic

Answer 36

Raise T-products (remove heat)

Lower T- reactants (add heat)

Question 37

Condition:Exothermic

Answer 37

Raise T- Reactants (remove heat)

Lower T-Products (reverse add heat)