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SIMULASI KSNP KIMIA TK. PROVINSI 1

Total questions: 105

Worksheet time: 2hrs 47mins

Name
Class
Date
1.
a)

A

b)

B

c)

C

d)

D

e)

E

2.
a)

A

b)

B

c)

C

d)

D

e)

E

3.
a)

A

b)

B

c)

C

d)

D

e)

E

4.
a)

A

b)

B

c)

C

d)

D

e)

E

5.

Suatu atom X memiliki 16 proton dan 16 netron, atom X terletak pada golongan/periode…

a)

VI A/3

b)

VI A/2

c)

VI A/4

d)

V 4/3

e)

V A/2

6.

Senyawa yang berikatan kovalen adalah ......

a)

NaCl

b)

BaCl2

c)

KBr

d)

CH4

e)

AgBr

7.

Konfigurasi electron atom suatu unsure A : 2 7 dan B: 2 8 2. Jika A dan B bereaksi senyawa yang terbentuk dan jenis ikatannya adalah…

a)

BA2, ikatan ion

b)

BA, ikatan ion

c)

BA2, ikatan kovalen

d)

B2A, ikatan ion

e)

B2A, ikatan kovalen

8.

1. Berbagai model atom digambarkan sebagai berikut:

Gambar 1 merupakan model atom yang dikemukakan

oleh…

a)

J.J. Thomson

b)

John Dalton

c)

Schrodinger

d)

Niels Bohr

e)

Rutherford

9.

1. Suatu unsur X mempunyai konfigurasi electron 1s2 2s2 2p5. Harga keempat bilangan kuantum unsur X adalah…

a)

n = 2, l = 0, m = 0, s = -1/2

b)

n = 2, l = 1, m = 0, s = -1/2

c)

n = 3, l = 0, m = 0, s = -1/2

d)

n = 2, l = 1, m = 0, s = +1/2

e)

n = 1, l = 0, m = 0, s = -1/2

10.

Pernyataan berikut yang paling benar tentang keelektronegatifan adalah …

a)

Energi yang dibebaskan ketika suatu atom dalam wujud gas menyerap elektron membentuk ion negatif

b)

Energi yang diperlukan untuk melepaskan satu elektron dari suatu atom dalam wujud gas membentuk ion positif

c)

Energi yang dibebaskan pada pembentukan suatu ikatan kimia

d)

Bilangan yang menyatakan kecenderungan dari suatu unsur menarik elektron ke pihaknya dalam suatu molekul/senyawa

e)

Bilangan yang menyatakan perbandingan energi ionisasi dari suatu unsur dengan unsur lainnya

11.

Diantara unsur-unsur berikut 3Li, 11Na, 19K, 37Rb dan 55Cs yang memiliki jari-jari atom terkecil adalah…

a)

3Li

b)

11Na

c)

19K

d)

37Rb

e)

55Cs

12.

Suatu atom yang mempunyai 3 kulit elektron dan 5 elektron valensi, nomor atomnya adalah

a)

11

b)

13

c)

15

d)

17

e)

19

13.

Which of the following compounds has the lowest molar solubility in mol/L in water at 25°C?

a)

Ag3PO4 Ksp = 1.8 x 10–18

b)

Sn(OH)2 Ksp = 5 x 10–26

c)

CdS Ksp = 3.6 x 10–29

d)

Al(OH)3 Ksp = 2 x 10–33

14.

Sodium chloride is added slowly to a solution that is 0.010 M in Cu+, Ag+, and Au+. The Ksp values for the chloride salts are 1.9 x 10-7, 1,6 x 10-10, and 2.0 x 10-13, respectively. Which compound will precipitate first?

a)

CuCl(s)

b)

AgCl(s)

c)

AuCl(s)

d)

All will precipitate at the same time.

15.

If 30 mL of 5.0 x 10-4 M Ca(NO3)2 are added to 70 mL of 2.0 x 10-4 M NaF, will a precipitate occur? (Ksp of CaF2 = 4.0 x 10–11)

a)

No, because the ion product (Qsp) is greater than Ksp.

b)

Yes, because the ion product (Qsp) is less than Ksp.

c)

No, because the ion product (Qsp) is less than Ksp

d)

Yes, because the ion product is (Qsp) greater than Ksp.

16.

How many moles of Ca(NO3)2 must be added to 1.0 L of a 0.100 M HF solution to begin precipitation of CaF2 (s)? For CaF2, Ksp = 4.0 x 10–11.

a)

5.8 x 10–7

b)

1.6 x 10–9

c)

7.0 x 10–11

d)

4.0 x 10–9

17.

If 50.0 mL of 0.0010 M BaCl2 is added to 50.0mL of 0.00010 M Na2SO4, what is the ionic product value of BaSO4 ?

a)

Q = 5.0 x 10-4

b)

Q = 2.5 x 10-8

c)

Q = 5.0 x 104

d)

Q = 2.5 x 108

18.
How does a solution become supersaturated?
a)
dissolve lots of solute in it.
b)
dissolve a little solute in it. 
c)
dissolve more solute than you should be able to. 
d)
dissolve a super amount of solvent in it. 
19.

"As temperature increases, the solubility for a slightly soluble salt will also increases."

Is the above statement correct?

a)

Yes, because as the temperature increases, solubility of the ionic compound increases.

b)

No, because the Ksp is the same at all the temperature.

c)

No, because the Ksp will change as the temperature change and it is depends on the type of reaction (endothermic or exothermic reaction)

d)

Yes, because as the temperature increases, solubility of ionic compound decreases and Ksp increases.

20.

For an endothermic reaction,

as the temperature of the solution increases,

a)

solubility of the salt increases ; Ksp increases

b)

solubility of the salt increases ; Ksp decreases

c)

solubility of the salt decreases ; Ksp increases

d)

solubility of the salt decreases ; Ksp decreases

21.

Na2SO4 solution is slowly added to a solution which contains 0.10 M Ba2+ and 0.10 M Pb2+.


Ksp BaSO4 = 1.08 x 10-10

Ksp PbSO4 = 2.53 x 10-8


Which of the followinfg statements correctly describes the result of the slow addition of Na2SO4 ?

a)

BaSO4 precipitates first because it is more soluble

b)

PbSO4 precipitates first because it is less soluble

c)

BaSO4 precipitates first because it is less soluble

d)

PbSO4 precipitates first because it is more soluble

22.

An equal number of moles of Na2CO3 is added to four different sample whose volume is 10 ml each


Sample 1 : 0.5 M Ba2+

Sample 2 : 0.5 M Ca2+

Sample 1 : 0.5 M Mg2+

Sample 1 : 0.5 M Sr2+


A precipitate only forms in one of the samples. Indentify the cation which is present in the precipitate


Ksp BaCO3 = 2.58 x 10-9

Ksp CaCO3 = 3.36 x 10-9

Ksp MgCO3 = 2.58 x 10-6

Ksp SrCO3 = 5.60 x 10-10

a)

Ba2+

b)

Mg2+

c)

Sr2+

d)

Ca2+

23.
Which of the following is a conjugate acid/base pair?
a)
HCl/OCl-
b)
H2SO4/SO42-
c)
NH4+/NH3
d)
H3O+/OH-
24.
Calculate the pH of a 0.47M NH3 (Kb = 1.8 x 10-5) solution.
a)
2.54
b)
8.93
c)
5.07
d)
11.46
25.
A weak acid, HF, is in solution with dissolved sodium fluoride, NaF. If HCl is added, which ion will react with the extra hydrogen ions from the HCl to keep the pH from changing?
a)
OH-
b)
Na+
c)
F-
d)
Na-
26.
At what time does the reaction reach equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
27.
For the reaction...
SO2 + O2  <−>  SO3
If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right 
d)
neither left nor right
28.
For the reaction...
SO2 + O2 <−>  SO3
If the concentration of O2 is decreased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right
d)
neither left nor right
29.
For the reaction...
N2 (g) +  3 H2 (g) <−> 2 NH3 (g)

If the pressure in the system is increased,  which substance will increase in concentration?
a)
N2
b)
H2
c)
N2 and H2
d)
NH3
30.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If the heat is added to the chemical system, the equilibrium will shift _______.
a)
left
b)
right
c)
left and right
d)
neither left nor right
31.
A chemical reaction takes place in a beaker.  What is the system and what are the surroundings?
a)
System:  Beaker
Surroundings: Everything 
b)
System:  Everything
Surroundings: Everything 
c)
System:  Everything
Surroundings: Beaker 
d)
System:  Beaker
Surroundings: Beaker 
32.
Which is the correct equilibrium constant expression for the reaction 
CaCO3(s) ⇋ CaO(s) + CO2(g)
a)
[CaO]/[CO2]
b)
[CO2]
c)
1/[CO2]
d)
[CO2][CaO] / [CaCO3
33.
A mixture of 0.500 mol H2 and 0.500 mol I2 was placed in a 1.00L flask.  The equilibrium constant Keq for the reaction H2(g) + I2(g) ↔ 2HI(g) is 54.3.  What is the concentration of HI at equilibrium?
a)
0.5M
b)
1.0M
c)
0.786M
d)
3.7M
34.
An exothermic reaction is allowed to reach equilibrium. If heat energy is then removed, the equilibrium will shift
a)
toward the middle
b)
toward the reactant side
c)
toward the product side
d)
No shift.
35.
Given the equation representing a reaction:
N2O4(g) ↔ 2NO2(g)

Which statement describes this reaction at equilibrium?
a)
The concentration of N2O4(g) must equal the concentration of NO2(g).
b)
The concentration of N2O4(g) and the concentration of NO2(g) must be constant.
c)
 The rate of the forward reaction is greater than the rate of the reverse reaction.
d)
The rate of the reverse reaction is greater than the rate of the forward reaction.
36.
Which of the two graphs reaches equilibrium?
a)
The left one.
b)
The right one.
c)
Both of them.
d)
Neither.
37.
When Keq > 1, 
a)
There are more products than reactants when the reaction reached equilibrium.
b)
There are more reactant than products when the reaction reached equilibrium.
c)
The amount of reactants is equal to the amount of products.
38.

Grafik berikut yang menunjukkan kurva titrasi basa kuat dengan asam lemah adalah…

a)
b)
c)
d)
e)
39.

Which of the following compounds cannot be a Brønsted–Lowry base?

a)

OH–

b)

NH4+

c)

H2O

d)

HNO3

40.

Jika ditentukan pembentuk senyawa adalah :   SO42−​; PO43−​; NO3− ; NH4+​ ; Fe2+; dan Al3+,\ SO_4^{2-}​;\ PO_4^{3-}​;\ NO_3^-\ ;\ NH_4^+​\ ;\ Fe^{2+};\ dan\ Al^{3+},  maka rumus kimia senyawa yang benar adalah .... 

a)

 Fe3(SO4)2Fe_3(SO_4)_2  

b)

 FePO4FePO_4  

c)

 Al2(SO4)3Al_2(SO_4)_3  

d)

 (NH)3(NO)4(NH)_3(NO)_4  

e)

 Al3(NO3)Al_3(NO_3)  

41.

pada percobaan 1 dan 3, laju reaksi dipengaruhi oleh ....

a)

konsentrasi

b)

sifat zat

c)

suhu

d)

luas permukaan

e)

katalis

42.

sejumlah magnesium dengan massa sama bereaksi dengan asam sulfat dengan jumlah yang sama pula. kondisi berikut yang menghasilkan reaksi tercepat adalah ...

a)

pita magnesium + 1 M asam sulfat pada suhu 80oC

b)

serbuk magnesium + 0,5 M asam sulfat pada suhu 20oC

c)

pita magnesium + 0,5 M asam sulfat pada suhu 80oC

d)

sebuk magnesium + 1 M asam sulfat pada suhu 20oC

e)

serbuk magnesium + 1 M asam sulfat pada suhu 80oC

43.

makanan lebih tahan lama jika disimpan dalam udara dingin. hal itu disebabkan ....

a)

laju pertumbuhan bakteri dapat dihambat

b)

berhentinya proses tumbukan dalam bahan makanan

c)

menurunkan laju pertumbuhan energi kinetik dalam bahan makanan

d)

bakteri membeku

e)

energi aktivasi bahan makanan turun dengan drastis

44.

The equilibrium constant, Kc, for the reaction to form ethyl ethanoate from ethanol and ethanoic acid,

C2H5OH + CH3CO2H → CH3CO2C2H5 + H2O,


at 60oC is 4.00.


When 1.00 mol each of ethanol and ethanoic acid are allowed to reach equilibrium at 60oC, what is the number of moles of ethyl ethanoate formed?

a)

13\frac{1}{3}

b)

23\frac{2}{3}

c)

14\frac{1}{4}

d)

34\frac{3}{4}

45.

Stomach juices have a pH of 1.0. aspirin is a monobasic acid represented by HA (Ka = 10-4 mol dm-3) which dissociation into ions H+ and A-. What are the relative concentrations of H+, A- and HA when aspirin from a tablet enters the stomach?

a)

[H+] > [HA] > [A-]

b)

[HA] > [H+] = [A-]

c)

[H+] > [A-] > [HA]

d)

[H+] = [A-] > [HA]

46.

Which one of the following acid solution can be used to give an effective buffer solution at a pH < 7 by partial neutralization with aqueous NaOH?

a)

0.01 mol dm-3 CH3CO2H

b)

0.1 mol dm-3 HI

c)

0.01 mol dm-3 HCl

d)

0.1 mol dm-3 HNO3

47.

Which statement explains the observation that magnesium hydroxide dissolves in aqueous ammonium chloride, but not in aqueous sodium chloride?

a)

ionic radius of the NH4+ ion is similar to that of Mg2+ but not that of Na+

b)

NH4Cl dissociates less fully than NaCl.

c)

The ions Na+ and Mg2+ are isoelectronic (have the same number of electrons).

d)

The ion NH4+ acts as an acid.

48.

Why is ethanoic acid a stronger acid in liquid ammonia than in its aqueous solution

a)

ammonia is a stronger base than water

b)

ammonium ethanoate is completely ionized in aqueous solution

c)

ammonium ethanoate is strongly acidic in aqueous solution

d)

liquid ammonia is a more polar solvent than water

49.

What is the mole ratio between EDTA and metal cation in complexometric titration?

a)

1:6

b)

1:4

c)

1:2

d)

1:1

50.

What is the pH of the buffer solution used in a normal EDTA titration?

a)

8

b)

9

c)

10

d)

11

51.

How many sites on the ethylenediaminetetraacetic acid are able to form dative covalent bonds with the metal ion?

a)

2

b)

4

c)

6

d)

None of the above

52.

Which of these are the standard conditions to calculate standard cell potential?

a)

T = 298 K

b)

Solution concentration at 1M

c)

Pressure at 100kPa

d)

All of the above

53.

Which of these statement is correct?

a)

Q > Ksp ; salt will precipitate

b)

Q = Ksp ; solution is unsaturated

c)

Q < Ksp : more salt will precipitate

d)

All of the above

54.

Which of these steps are not the procedure for precipitation method?

a)

Washing

b)

Weighing

c)

Analysing

d)

Filtration

55.

Di antara larutan berikut yang dapat membentuk larutan garam yang terhidrolisis, kecuali...

a)

100 mL larutan CH3COOH 0,1 M + 100 mL larutan NaOH 0,1 M

b)

100 mL larutan HF 0,1 M + 100 mL larutan KOH 0,1 M

c)

100 mL larutan HCl 0,1 M + 100 mL larutan NaOH 0,1 M

d)

100 mL larutan HCl 0,1 M + 100 mL larutan NH4OH 0,1 M

e)

100 mL larutan HCOOH 0,1 M + 100 mL larutan KOH 0,1 M

56.

Larutan di bawah ini yang dapat mengubah lakmus merah menjadi biru adalah...

a)

CH3COONa

b)

CH3COONH4

c)

Al2(SO4)3

d)

NH4CN

e)

NaCl

57.

Garam yang dalam air dapat terhidrolisis membentuk larutan dengan pH lebih kecil dari 7 adalah...

a)

NaCl

b)

Na2CO3

c)

NaNO3

d)

CH3COONa

e)

NH4Cl

58.

Larutan KCN dalam air akan bersifat basa. Reaksi yang menunjukkan terjadinya sifat basa tersebut adalah...

a)

K+ + OH−→ KOHK^{+\ }+\ OH^-\rightarrow\ KOH

b)

CN− + H+ → HCNCN^{-\ }+\ H^{+\ }\rightarrow\ HCN

c)

K+ +H2O→KOH+H+K^{+\ }+H_2O\rightarrow KOH+H^+

d)

CN−+KOH →KCN+OH−CN^-+KOH\ \rightarrow KCN+OH^-

e)

CN− +H2O→HCN+OH−CN^{-\ }+H_2O\rightarrow HCN+OH^-

59.

Derajat hidrolisis (Kh) dari larutan NH4Cl 0,001 M (Kb NH4OH = 10-5) adalah...

a)

10-2

b)

10-3

c)

10-4

d)

10-5

e)

10-6

60.

Jika Ka CH3COOH = 10-5, maka pH larutan CH3COONa 0,01 M adalah...

a)

7

b)

7,5

c)

8

d)

8,5

e)

9

61.

Massa CH3COONa (Mr = 82) yang terlarut dalam 10 mL larutan CH3COONa pH = 9 adalah... (Ka CH3COOH = 10-5)

a)

8,20 gram

b)

4,10 gram

c)

2,05 gram

d)

0,082 gram

e)

0,041 gram

62.

pH larutan (NH4)2SO4 0,1 M. Jika Kb NH4OH = 2 x 10-5 adalah...

a)

3 - log 4

b)

5

c)

6 - log 7

d)

8 + log 7

e)

9

63.

Ke dalam 50 mL HCl 0,2 M ditambahkan 50 mL NH4OH 0,2 M (Kb = 10-5), pH larutan yang terbentuk adalah...

a)

3

b)

5

c)

8

d)

9

e)

12

64.

1. Which reaction is NOT Lewis acid-base reaction?

a)

C+O2→CO2C+O_2\rightarrow CO_2

b)

BeF2+2F−→BeF42−BeF_2+2F^-\rightarrow BeF_4^2-

c)

NH3+BF3 →H3NBF3NH_3+BF_3\ \rightarrow H_3NBF_3

d)

(C4H9)3N+SO3 → (C4H9)3NSO3(C_4H_9)_3N+SO_{3\ }\rightarrow\ (C_4H_9)_3NSO_3

65.

A solution of weak acid, HA 0.2 M ionises 1.8%. Calculate the value of Ka for this acid.

a)

3.6x10-5

b)

1.8x10-5

c)

0.9x10-5

d)

6.5x10-5

66.

What is meant by salt hydrolysis?

a)

The producing of cation and anion from the reaction between strong base and strong acid.

b)

Salt hydrolysis occurs when any soluble salts dissolve in water

c)

The producing of cation and anion from the reaction between weak acid and weak base.

d)

Salt hydrolysis occurs when there is a reaction between cation, or anion or both and water.

67.

Each of the following pairs of substances form(s) buffer solution(s) EXCEPT

a)

NaH2PO4(aq) + Na2HPO4(aq)

b)

NH3(aq) + NH4Cl(aq)

c)

HCl(aq) + NaCl(aq)

68.

For a titration between sulphuric acid and an aqueous solution of ammonia, the most suitable indicator used is

a)

ethyl red 4.5-6.5

b)

phenol red 6.7-8.5

c)

phenolphthalein 8.3-10.0

d)

alizarin yellow 10.1-12.0

69.

Which of the following solutions has the highest pH at 25oC? (No calculations required.)

a)

Ammonium ion, Ka = 5.8 x 10-10

b)

Hydrogen sulfate ion, Ka = 1.0 x 10-2

c)

Hydrogen carbonate ion, Ka = 4.7 x 10-11

d)

Hydrogen phosphate ion, Ka = 4.2 x 10-13

70.

_________ indicates the equivalent quantities of reactants that have been mixed in a titration according to stoichimetric equation.

a)

end point

b)

equivalence point

c)

indicator point

d)

starting point

71.

Given the following general equilibrium equation,

A + 2B ⇄ AB2 K << 1, if the initial concentration of all species is 1, what species will have the greater concentration at equilibrium

a)

A

b)

B

c)

AB2

72.

Given the following equilibrium equation,

A (g) + 2B (g) ⇄ AB2 (g) ΔH > 0, which of the following changes will increase the amount of AB2 in the vessel?

a)

Decreasing the temperature

b)

Increasing the concentration of A

c)

Removing a small amount of B

d)

Decreasing the pressure

73.

The following system at equilibrium is exothermic. If the temperature is increased...

A (g) + 2B (g) ⇄ AB2 (g)

a)

[A] will increase the most

b)

[B] will increase the most

c)

[AB2] will increase the most

74.

For the reaction,

CO2(g) + 4 H2(g) ↔ CH4(g) + 2 H2O(g),

K = 8.2 x 1019 at 25°C.

Initially CO2(g) and H2(g) are 1.0atm at 25°C in an evacuated container, which substance will have the highest pressure when the system is at equilibrium?

a)

CO2(g)

b)

H2(g)

c)

CH4(g)

d)

H2O(g)

75.

Identify the spectator ion(s) in the equation: 2Ag+(aq) + 2NO3–(aq) + 2Na+(aq) + S2–(aq) --> Ag2S(s) + 2Na+(aq) + 2NO3–(aq)

a)

2Ag+(aq) + 2NO3–(aq)

b)

2Na+(aq) + 2NO3–

c)

2Na+(aq) + S2–(aq)

d)

Ag2S(s) + 2Na+(aq

76.
At what time (in seconds) is equilibrium established?
a)
0 seconds
b)
1 second
c)
5 seconds
d)
10 seconds
77.

Which of the following must be true for a reaction that proceeds spontaneously from initial standard state conditions?

a)

ΔG° > 0 and Keq > 1

b)

ΔG° > 0 and Keq < 1

c)

ΔG° < 0 and Keq > 1

d)

ΔG° < 0 and Keq < 1

78.
Entropy increases from solid, liquid to gas. Why?
a)
Molecular disorder increases
b)
Molecular randomness decreases
c)
Molecules are more energetic
d)
Molecules are more reactive
79.

Given the change of phase:


CO2(g) → CO2(s)


As CO2(g) changes to CO2(s), the entropy of the system

a)

decreases

b)

increases

c)

remains the same

80.

Which of these have a DECREASE in entropy?

a)

CaCO3(s) → CaO(s) + CO2(g)

b)

2NO2(g) → N2O4(g)

c)

2NH3(g) → 3H2(g) + N2(g)

d)

C6H6(l) → C6H6(g)

81.
a)

ZnSZnS

b)

FeSFeS

c)

MnSMnS

d)

CuSCuS

e)

Ag2SAg_2S

82.

0,35 gram  BaF2BaF_2  (Mr/175) larut dalam air murni 1 liter menghasilkan larutan jenuh. Hasil kali kelarutan  BaF2BaF_2  adalah....

a)

 1,7 . 10−21,7\ .\ 10^{-2}  

b)

 3,2 . 10−63,2\ .\ 10^{-6}  

c)

 3,2 . 10−83,2\ .\ 10^{-8}  

d)

 3,2 . 10−93,2\ .\ 10^{-9}  

e)

 4,0 . 10−94,0\ .\ 10^{-9}  

83.
The element with the ground state electron configuration of [Ar]3d74s2 is
a)
Mg
b)
K
c)
Ar
d)
Co
84.
Small drops of water tend to bead up because of
a)
high capillary action.
b)
the shape of the meniscus.
c)
the resistance to increased surface area.
d)
low London dispersion forces.
85.

All of the following statements concerning voltaic cells are true except

a)

the two half-cells are connected by a salt bridge.

b)

electrons flow from the anode to the cathode.

c)

oxidation occurs at the cathode.

d)

voltaic cells can be used as a source of energy.

86.
Atomic radii decrease from left to right across a period because of
a)
an increase in the effective nuclear charge.
b)
an increase in the gross energy level (n).
c)
an increase in the sublevel (l).
d)
an increase in shielding.
87.
The compound most likely to be ionic is
a)
KF
b)
CCl4
c)
CO2
d)
ICl
88.
The total number of lone pairs in PCl3 is
a)
1
b)
8
c)
10
d)
12
89.
When a salt dissolves in water, the solute-solvent interaction is
a)
hydrogen bonding.
b)
London dispersion forces.
c)
dipole-dipole forces.
d)
ion-dipole forces.
90.
A compound of nitrogen and oxygen is 63.64% nitrogen by mass. What is the empirical formula of this compound?
a)
NO
b)
NO2
c)
NO3
d)
N2O
91.
Nitrogen gas diffuses through a porous barrier at the rate of 5.80 liters per minute. An unknown gas under the same conditions diffuses through the same barrier at a rate of only 1.80 liters per minute. What is the molar mass of the unknown gas?
a)
291
b)
145
c)
90.3
d)
50.3
92.

Apa Kepanjangan dari Covid-19

a)

Coronavirus Defect 2019

b)

Coronavirus Disease 2019

c)

Coronavirus Detention 2019

d)

Coronavirus 2019

93.

Berikut merupakan gejala Covid-19, kecuali ?

a)

Demam tinggi

b)

Sesak napas

c)

Telinga berdengung

d)

Batuk kering

94.

Berapa lama masa inkubasi penyakit COVID19 ?

a)

1 Bulan

b)

2 Bulan

c)

90-120 Hari

d)

2-14 Hari

95.

Penyakit COVID19 disebabkan oleh ?

a)

Bakteri

b)

Kontaminasi Kimia

c)

Virus

d)

Jamur

96.

Social distancing penting dalam langkah pencegahan penyebarluasan Covid-19, yang berarti :

a)

Harus mencuci baju dengan disinfektan

b)

Harus menjaga jarak dengan orang-orang sekitar

c)

Harus makan dengan alat sendiri

d)

Harus menjaga hubungan baik antar sesama

97.

When zinc carbonate powder is heated strongly, it produces colourless gas M. What is gas M?

Apabila serbuk zink karbonat dipanaskan dengan

kuat, gas tanpa warna M dihasilkan. Apakah gas M?

a)

Hydrogen gas / Gas hidrogen

b)

Carbon dioxide / Karbon dioksida

c)

Inert gas / Gas adi

d)

Oxygen gas / Gas oksigen

98.

State the observation when gas M passed through the lime water.

Nyatakan pemerhatian apabila gas M dilalukan ke atas air kapur.

a)

Lime water turn blue / Air kapur berubah warna ke biru

b)

Lime water turns cloudy / Air kapur menjadi keruh

c)

Nothing change / Tiada perubahan

d)

Black precipitate form / Mendakan hitam terbentuk

99.

Perhatikan beberapa proses pembuatan koloid berikut


(1) H2S ditambah ke dalam endapan NiS

(2) Sol logam dibuat dengan cara busur Bredig

(3) Larutan AgNO3 diteteskan kedalam larutan HCl

(4) Larutan FeCl3 diteteskan ke dalam air mendidih

(5) Agar - agar dipeptisasi ke dalam air


Contoh pembuatan koloid dengan cara kondensasi adalah ....

a)

1 dan 2

b)

1 dan 3

c)

3 dan 4

d)

4 dan 5

e)

4 saja

100.

Agar agar, sirup, es krim termasuk pembuatan koloid dengan cara...

a)

Homogenisasi

b)

Mekanik

c)

Peptisasi

d)

Bredig

e)

redoks

101.

What are chemical compounds that give the characteristic odors and flavors of fruits?

a)

Esters

b)

Hormones

c)

acids

d)

water

102.

Which of the following is the correct apparatus set-up for the preparation of an ester?

Antara berikut, yang manakah susunan radas yang betul untuk penyediaan suatu ester?

a)
b)
c)
d)
103.

The following data were obtained for the reaction of NO with O2. Concentrations are in molecules/cm3 and rates are in molecules/cm3⋅s.

a)

Rate = k[NO][O2]

b)

Rate = k[NO][O2]2

c)

Rate = k[NO]2[O2]

d)

Rate = k[NO]2

e)

Rate = k[NO]2[O2]2

104.

What is the numerical value of the rate constant?

a)

0.053

b)

1.19

c)

2.37

d)

5.63

e)

none of these

105.

The rate law for a given reaction is found to be Rate = k[A]2[B]. Which of the following mechanisms gives this rate law? (choose all that apply)

a)

I

b)

II

c)

III

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