Chemistry exam 01.06-2016 Flashcards Preview

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Flashcards in Chemistry exam 01.06-2016 Deck (27):
1

MCQ General Chemistry
1) Units for ppb

[ppb]=μg/L
[ppm]=mg/L

2

MCQ General Chemistry
2) Diameter of colloidal particals

1-500 nm

3

MCQ General Chemistry
3) In an isolated system

a. Entropy will always increase

4

MCQ General Chemistry
4) Cathode (+) of Cu/CuSO4 cell will be merged into a solution of what conc.

Cathode (+) 1 M Cu(NO3)2 (aq)
Anode (-) 1 M Zn(NO3)2 (aq)

5

MCQ General Chemistry
5) Sodium Bromide is dissolved in H2O, what happens to the solution

NaBr + H2O = Na+ +Br-

6

MCQ General Chemistry
6) Fog in colloidal system is

L/G (liquid particles dispersed in gas)

7

MCQ General Chemistry
7) Solution A has pOH 2, Solution B pOH 1, how is the H+ concentration

Solution A has 10 times higher amount H+-ions than Solution B

8

MCQ General Chemistry
8) In thin liquid chromotography (TLC), quality analysis is

Retention factor
Rf = Distance to plupp from baseline/Distance to topline from baseline

9

Brief General Chemistry
1) Define and give examples of reference electrodes

The e. p. of a reference electrode remains constant during the operation of the cell at a given temperature
(e.g. Ag/AgCl-, or the calomel, Hg/Hg2Cl2- electrode).

10

Brief General Chemistry
2) Boiling point of liquids

The temperature at which the vapour pressure of a liquid equals the external pressure.

The normal freezing point of a liquid is the temperature at which solid
and liquid are in equilibrium.

11

Brief General Chemistry
1) Define critical temperature and pressure

Critical temperature: the temperature above which it is impossible to liquefy the gas, no matter how high the applied pressure.

Critical pressure: it is the minimum pressure needed to liquefy a gas at its critical temperature.

12

Brief General Chemistry
2) 1st law of thermodynamics

{∆E} = Ein – Eout
Energy can neither be created nor destroyed, only interconverted between forms.

“The change of energy in a system is constant, any decrease must be exactly balanced by an increase”

13

Brief General Chemistry
3) Define Gibbs Energy and give equation, naming symbols

∆G ≝ ∆H - T x ∆S

G= Gibbs energy
H= Enthalpy
T=Temperature
S=Entropy
“Gibbs energy change combines enthalpy and entropy into a single state function.”

14

Brief General Chemistry
4) Anionic surfactant

Soap

15

Brief General Chemistry

5) Strong acid (high tendency to donate protons), weak base (weak tendency to accept protons)

Strong acids: HCl, H2SO4, HNO3
Strong bases: NaOH, Ba(OH)2
Weak acids: CH3COOH
Weak bases: Cl-

16

Brief General Chemistry
6) Raoults law

P = xA . PAo + xB . PBo

17

Brief General Chemistry
1) Define lyophilic, hypertonic solution, emulsion

Lyophilic=Hydrophilic
(Proteins, Nucleic acids, Emulsifiers, Micelles)

Hypertonic= A solution having a greater effective concentration than the cell fluid (shrink)

Emulsion= A mixture of two or more liquids that are normally immiscible
(O/W & W/O)

18

Brief General Chemistry
2) Define pressure

p=F/A

19

Brief General Chemistry
3) Define state function

A state function is a function that depends only on the current state of the system, i.e the initial and final state of the system.

20

Brief General Chemistry
4) 2 examples of ionic and metallic cystalline substances

Ionic: NaCl, CaF2
Metallic: HG, Au

21

MCQ Bioorganic & Food chemistry
1) Vitamin A structural characteristics

B-inone ring + All-trans arrangement

22

MCQ Bioorganic & Food chemistry
2) Starting unit in terpenes

(C5H8)n

23

MCQ Bioorganic & Food chemistry
3) Which has a chiral atom:
a. pyridine,
b. piperazine,
c. piperdine,
d. tropan,
e. coniine

e. coniine

24

MCQ Bioorganic & Food chemistry
4) Purine heterocycle

Adenine, Guanine

25

MCQ Bioorganic & Food chemistry
5) Metal in heamoglobin

Fe

26

MCQ Bioorganic & Food chemistry
8) Antioxidant

Flavonoids,
a subset of polyphenol antioxidants, are present in many berries, as well as in coffee and tea.

27

MCQ Bioorganic & Food chemistry
9) Retrogradation

Recrystallisation of starch