Module 2

Question 1

1 atm is equal equal to

Answer 1

760 mmHg, torr

Question 2

Definition of gases

Answer 2

Made up of small atoms or molecules that are constant, random, in linear motion
-the distance of separation is very large

Question 3

Boyles law

Answer 3

-use if constant temperature
P1V1=PfVf

Question 4

Charles law

Answer 4

• use if Pressure is constant
  Vi = Vf
  — —
  Ti Tf

Question 5

Combined gas law

Answer 5

PiVi = PfVf
—— ——
Ti Tf

Question 6

Avocados law

Answer 6

-use of temperature and pressure are constant
Vi = Vf
—- —-
ni nf

Question 7

Standard temperature and pressure

Answer 7

T= 273K
P= 1 atm
V= 22.4L
R= 0.0821 L•atm/ mol• K

Question 8

Ideal gas law

Answer 8

PV=nRt

Question 9

Condensation

Answer 9

Energy + h20(l) —-> H2O (g)

Question 10

Evaporation

Answer 10

H20(g) —-> H20(l) + energy

Question 11

Dipole dipole interaction

Answer 11

Attractive forces between polar molecules

HCl <—> HCl

Question 12

London dispersion forces

Answer 12

Electrons in continuous motion, a nonpolar molecule, having instantaneous dipole
-* weakest force*

Question 13

Hydrogen bonding

Answer 13

Very strong, intermolecular attraction, causing higher than expected boiling points in melting points
Ex: h20, nh3

Question 14

Electrolytes

Answer 14

Salutes that are soluble ionic compounds

Question 15

Mass/volume percent

Answer 15

G of solute
—————- x 100
mL of solution

Question 16

Mad/ mass percent

Answer 16

G of solute
—————- x100
G of solution

Question 17

Morality

Answer 17

Mole of solute
M=. ———————
L of solution

Question 18

Dilution equation

Answer 18

M1v1= M2V2
Involves molarity

Question 19

Molality

Answer 19

Mole of solute
———————
Kg of solvent

Question 20

Calculating osmolarity

Answer 20

O= i• M
Molarity x Coefficient of products

Question 21

Calculating osmotic pressure

Answer 21

Pie=iMRT
Moles• M • 0.0821• 273

Question 22

Calculating ions

Answer 22

Ion= molar mass of ion
———————————-
# of charges on ion

Question 23

Calculating ion concentration

Answer 23

Eq/L = (eq/mol ion) • M

Question 24

Exothermic reactions

Answer 24

A-B+ C-D—> A-D+ C-B + energy
Combustion

Question 25

Endothermic reactions

Answer 25

Energy + A-B + C-D—> A-D+ C-B Decomposition

Question 26

Enthalpy

Answer 26

Delta H = 🔼H products -🔼H reactants Exothermic: - kcal Endothermic: + kcal

Question 27

Specific heat

Answer 27

Q= ms• 🔼T• 1.00cal/g*C

Question 28

Catalyst

Answer 28

As substance that increases the reaction rate

Question 29

General equilibrium rxn

Answer 29

aA +bB<_—> cC + dD [C]^c+ [D]^d Keq: ————— [A]^a+. [B]^b

Question 30

Equilibrium constant

Answer 30

2HI<—->. H2+ I2 HI= 0.54M H2: 1.72M I2: 1.72M 1.72•1.72/ 0.54= 10.1

Question 31

Acid ls and bases

Answer 31

Acid: proton H+ donor Base: proton H+ acceptor

Question 32

Strong acids

Answer 32

HCI, HBr, HNO3, H2SO4, CIO4

Question 33

Strong acids

Answer 33

HCI, HBr, HNO3, H2SO4, CIO4

Question 34

Strong bases

Answer 34

NaOH, KOH, Ba(OH)2

Question 35

Acid base dissociation

Answer 35

HX+Y<-> X- + HY+

Question 36

Hydronium ion

Answer 36

Keq: [H3O+] [OH-] = 1.0• 10^-14

Question 37

Calculating pH

Answer 37

pH= -log[H30]

Question 38

Calculating pH and molarity

Answer 38

1.0•10^-14 = H3O [OH]

Question 39

Calculating ph and buffers

Answer 39

Ka= [H3O] [CH3COO-]\ [CH3COOH]