Examples

Question 1

Arrhenius equation

Answer 1

k = rate constant
A = total number of collisions (leading to a reaction or not)
e-Ea/(RT) = the probability that any given collision will result in a reaction
R= universal gas constant T = absolute temperature

Question 2

The Lewis Acid ex

Answer 2

Lewis acid: free electron pair acceptor (Example: BF3)

Question 3

Lewis base

Answer 3

Lewis base: free electron pair donor (Example: NH3)

Question 4

Gibbs energy

Answer 4

ΔG= ΔH-TΔS

Question 5

Example of adsorbent, adsorbate

Answer 5

Adsorbent: Silica gel (SiO2) Adsorbate: fluid

Question 6

strong acid

Answer 6

HCl , HI, HBR

Question 7

WEAK ACID

Answer 7

HCOOH, CH3COOH

Question 8

WEAK BASE

Answer 8

NH3, NH2OH

Question 9

STROGN BASE

Answer 9

LiOH, NaOH

Question 10

ALKALINE SUB

Answer 10

KOH, NaOH

Question 11

Complex ion

Answer 11

[Zn(OH)4]2- , [Pb(OH)4]2-

Question 12

acidic buffer system

Answer 12

NH3 + H20 -> NH4+ + OH-

Question 13

Colligative properties ex

Answer 13

osmotic pressure, boiling point

Question 14

micelle ex

Answer 14

soap

Question 15

coagulation ex

Answer 15

blood

Question 16

suspension ex

Answer 16

salt and water

Question 17

emulsion ex

Answer 17

milk, oil and water

Question 18

Ligand ex

Answer 18

NH3, H20

Question 19

Faraday’s law equation

Answer 19

m=(M/Z)(Q/F)
m= mass of a substance liberated at an electrode in grams
M = molar mass of the substance
z = charge of the ion
Q = the total electric charge passed through the substance
F = the Faraday Constant

Question 20

How can be calculated the standard reaction enthalpies?

Answer 20

product - starting material

Question 21

solubility product for iron(II) hydroxide

Answer 21

[Fe2+][OH-]2+

Question 22

solubility product for silver(I) chloride

Answer 22

[Ag+][Cl-]

Question 23

solubility product for lead(II) sulfide

Answer 23

[Pb2+][S-]