Question Set B

TN 12th Standard Chemistry Carbonyl Compounds and Carboxylic Acids Creative Questions Study Material - QB365

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Questions:

Multiple Choice Question

60 x 1 = 60

The charges on the sol particles can be determined by _______.

(a)

Tyndall effect

(b)

Brownian

(c)

electrophoresis

(d)

none

\(\alpha=\frac{\Lambda_{\mathrm{m}}}{\Lambda_{\mathrm{m}}^{0}}\) is called _______.

(a)

dissociation constant

(b)

Degree of dissociation

(c)

Ionisation Constant

(d)

Degree of hydrolysis

Which of the following is Secondary cell?

(a)

Laclanche cell

(b)

Lithium ion battery

(c)

Mercury button cell

(d)

both (a) and (c)

The conjugate base of OH^- is _______.

(a)

O₂

(b)

O^2-

(c)

O^-

(d)

H₂O

The thermal decomposition of HI on gold surface is an example for this order reaction ______.

(a)

second

(b)

Zero

(c)

first

(d)

third

The percentage of free space in simple cubic arrangement is _______.

(a)

47.69%

(b)

28%

(c)

26.52%

(d)

34.75%

To get pure alumina Al₂O₃, Sodium meta aluminate is neutralised by _______.

(a)

H₂SO₄

(b)

HCI

(c)

NaOH

(d)

CO₂

The preliminary step in metallurgical process is ________.

(a)

Roasting

(b)

Concentration of ore

(c)

Calcination

(d)

Smelting

_______ is the reciprocal of resistance.

(a)

specific conductance

(b)

molar conductance

(c)

specific resistance

(d)

conductance

10.

Low molar conductivity at high concentration is due to _______.

(a)

High attractive force between oppositely charged ions

(b)

Viscous drag due to greater solvation

(c)

Both High attractive force between oppositely charged ions and Viscous drag due to greater solvation

(d)

Neither High attractive force between oppositely charged ions and Viscous drag due to greater solvation

11.

An example for 1 : 1 electrolyte is ______.

(a)

H₂SO₄

(b)

Na₂SO₄

(c)

NaCI

(d)

Al₂(SO₄)₃

12.

Which among the following is the strongest reducing agent?

(a)

F₂

(b)

Cl₂

(c)

(d)

13.

Hydrogenation of benzoyl chloride in the presence of Pd on BaSO₄ gives _______.

(a)

phenol

(b)

benzoic acid

(c)

benzyl alcohol

(d)

benzaldehyde

14.

Schiff's reagent gives pink colour with _______.

(a)

acetone

(b)

acetaldehyde

(c)

ethyl alcohol

(d)

methyl acetate

15.

______enzyme hydrolyses starch into maltose.

(a)

pepsin

(b)

diastase

(c)

zymase

(d)

urease

16.

The iron catalyst used in the synthesis of ammonia in Haber's process is poisoned by _______.

(a)

AS₂O₃

(b)

V₂O₅

(c)

H₂5

(d)

Glycerine

17.

Henderson equation for a weak acid and its salt is _______.

(a)

pH = pK_b+ log (Salt) / (Acid)

(b)

pH = pK_a + log (Salt) / (Acid)

(c)

pH = pK_a + log (Salt) / (Base)

(d)

pH = pK_a + log (Acid) / (Salt)

18.

_______ is used as an antifreeze in automobiles radiators.

(a)

Ethanol

(b)

Propanol

(c)

Methanol

(d)

Benzyl alcohol

19.

Formation of o and p - hydroxy benzaldehyde from phenol on treatment with CHCl₃ and NaOH is _______.

(a)

Riemer-Tiemann reaction

(b)

Kolbe's reaction

(c)

Coupling reaction

(d)

Hydrogenation

20.

Ionic product of water increases when _______.

(a)

Pressure decreases

(b)

H⁺ ions are added

(c)

OH^-ions are added

(d)

temperature increases

21.

Alcohols are soluble in polar solvents like water due to ______.

(a)

intermolecular hydrogen bonding

(b)

intramolecular hydrogen

(c)

co-ordiate bonding

(d)

ionic bonding

22.

Which type of colloid is a sol?

(a)

Solid in liquid

(b)

Liquid in solid

(c)

Soild in solid

(d)

Gas in solid

23.

The ionization constant of phenol is higher than that of ethanol because ______.

(a)

phenoxide ion is bulkier than ethoxide

(b)

phenoxide ion is stronger base than ethoxide.

(c)

phenoxide ion is stablized through delocalisation.

(d)

phenoxide ion is less stable than ethoxide ion.

24.

The major product of the following reaction

(a)

(b)

(c)

(d)

25.

C₆H₅NO₂ \(\overset { Fe/Hel }{ \longrightarrow } A\overset { { NaNO }_{ 2 }/HCl }{ \underset { 273K }{ \longrightarrow } } B\overset { { H }_{ 2 }O }{ \underset { 283 }{ \longrightarrow } } C \) C' is _______.

(a)

C₆H₅- OH

(b)

C₆H₅- CH₂OH

(c)

C₆H₅- COH

(d)

C₆H₅NH₂

26.

When aniline reacts with acetic anhydride the product formed is_______.

(a)

o – aminoacetophenone

(b)

m-aminoacetophenone

(c)

p – aminoacetophenone

(d)

acetanilide

27.

Aniline + benzoylchloride \(\overset { NaOH }{ \longrightarrow } \)C₆H₅ - NH - COC₆ H₅ this reaction is known as ______.

(a)

Friedel – crafts reaction

(b)

HVZ reaction

(c)

Schotten – Baumann reaction

(d)

none of these

28.

Which one of the following will not undergo Hofmann bromamide reaction.

(a)

CH₃CONHCH₃

(b)

CH₃CH₂CONH₂

(c)

CH₃CONH₂

(d)

C₆H₅CONH₂

29.

The reagent used to distinguish between acetaldehyde and benzaldehyde is _______.

(a)

Tollens reagent

(b)

Fehling’s solution

(c)

2,4 – dinitrophenyl hydrazine

(d)

semicarbazide

30.

CH₃Br \(\overset { KCN }{ \longrightarrow } (A)\overset { { H }_{ 2 }{ O }^{ + } }{ \longrightarrow } (B)\overset { { PCl }_{ 5 } }{ \longrightarrow } \) (C) product (c) is ______.

(a)

acetylchloride

(b)

chloro acetic acid

(c)

\(\alpha\)- chlorocyano ethanoic acid

(d)

none of these

31.

The reactions
is an example of ______.

(a)

Wurtz reaction

(b)

cyclic reaction

(c)

Williamson reaction

(d)

Kolbe reactions

32.

Which one of the following will react with phenol to give salicyladehyde after hydrolysis.

(a)

Dichlo methane

(b)

trichloroethane

(c)

trichloro methane

(d)

CO₂

33.

Which one of the following is the strongest acid.

(a)

2 - nitrophenol

(b)

4 – chlorophenol

(c)

4– nitrophenol

(d)

3 – nitrophenol

34.

The coagulation values in millimoles per litre of the electrolytes used for the coagulation of As₂S₃ are given below
(I) (NaCl) = 52
(II) ((BaCl₂) = 0.69
(III) (MgSO₄) = 0.22
The correct order of their coagulating power is ________.

(a)

III > II > I

(b)

I > II > III

(c)

I > III > II

(d)

II > III > I

35.

In an electrical field, the particles of a colloidal system move towards cathode. The coagulation of the same sol is studied using K₂SO₄
(i), Na₃ PO₄
(ii), K₄ [Fe(CN)₆]
(iii) and NaCl
(iv) Their coagulating power should be

(a)

II > I > IV > III

(b)

III > II > I > IV

(c)

I > II > III > IV

(d)

none of these

36.

Hair cream is _____.

(a)

gel

(b)

emulsion

(c)

solid sol

(d)

sol.

37.

A gas X at 1 atm is bubbled through a solution containing a mixture of 1MY^-and 1MZ^- at 25^oC. If the reduction potential of Z>Y>X, then_____.

(a)

Y will oxidize X and not Z

(b)

Y will oxidize Z and not X

(c)

Y will oxidize both X and Z

(d)

Y will reduce both X and Z

38.

Among the following cells
I) Leclanche cell
II) Nickel – Cadmium cell
III) Lead storage battery
IV) Mercury cell
Primary cells are ____.

(a)

I and IV

(b)

I and III

(c)

III and IV

(d)

II and III

39.

During electrolysis of molten sodium chloride, the time required to produce 0.1mole of chlorine gas using a current of 3A is _____.

(a)

55 minutes

(b)

107.2 minutes

(c)

220 minutes

(d)

330 minutes

40.

H₂PO₄^- the conjugate base of _______.

(a)

PO₄³⁻

(b)

P₂O₅

(c)

H₃PO₄

(d)

HPO₄^2-

41.

Which of these is not likely to act as Lewis base?

(a)

BF₃

(b)

PF₃

(c)

(d)

F^–

42.

pH of a saturated solution of Ca(OH)₂ is 9. The Solubility product (K_sp) of Ca(OH)₂ _______.

(a)

0.5 × 10^-15

(b)

0.25 × 10^-10

(c)

0.125 × 10^-15

(d)

0.5 × 10^-10

43.

Which of the above graphs is correct for first order reactions?

(a)

I, II

(b)

II, III

(c)

I, IV

(d)

I, III

44.

A reaction having equal activation energies for forward and reverse reactions has ______.

(a)

ΔG = 0

(b)

ΔH = 0

(c)

ΔH = ΔG = ΔS = 0

(d)

ΔS = 0

45.

In an hexagonal crystal _______.

(a)

a=b=c,∝ =β=૪=90°

(b)

a=b=c,∝ =β=૪≠90°

(c)

a=b≠c,∝ =β=૪=90°

(d)

a=b≠c,∝ =β=90°૪=120°

46.

A regular three dimensional arrangement of identical points in space is called _______.

(a)

Unit cell

(b)

Space lattice

(c)

Primitive

(d)

Crystallography

47.

Which of the following is characteristic of ionic solids?

(a)

Very low value of electrical conductivity in the molten state

(b)

Brittle nature

(c)

Very strong forces of attractions

(d)

Anisotropic nature

48.

Which of the following defects decreases the density of the crystal?

(a)

Interstitial defect

(b)

Vacancy defect

(c)

Frankel defect

(d)

None of these above

49.

Semiconductors are purified by_______ method.

(a)

Zone refining

(b)

Electrolytic refining

(c)

Mond's process

(d)

Bessemerisation

50.

Malachite has______ composition.

(a)

2CuCO₃.Cu(OH)₂

(b)

CuCO₃.Cu(OH)₂

(c)

Cu₂O

(d)

Cu₂S

51.

In the froth-floatation process the collectors such as pine oil and xanthates, etc enhance.

(a)

Non-wettability of the mineral particles in froth.

(b)

Non-wettability of the mineral particles in water

(c)

Non-wettability of the gangue particles in froth

(d)

Non-wettability of the gangue particles in water

52.

The correct difference between first and second order reactions is that________.

(a)

A first order reaction can be catalysed; a second order reaction cannot be catalysed.

(b)

The half life of a first order reaction does not depend on [A₀]; the half life of a second order reaction does depend on [A₀].

(c)

The rate of a first order reaction does not depend on reactant concentrations; the rate of a second order reaction does depend on reactant concentrations.

(d)

The rate of a first order reaction does depend on reactant concentrations; the rate of a second order reaction does not depend on reactant concentrations.

53.

For a first order reaction, the rate constant is 6.909 min^-1the time taken for 75% conversion in minutes is _______.

(a)

\(\left( \frac { 3 }{ 2 } \right) { \log 2 }\)

(b)

\(\left( \frac { 2 }{ 3 } \right) \log2\)

(c)

\(\left( \frac { 3 }{ 2 } \right) \log\left( \frac { 3 }{ 4 } \right) \)

(d)

\(\left( \frac { 2 }{ 3 } \right) \log\left( \frac { 4 }{ 3 } \right) \)

54.

For a reaction Rate = k[acetone]^3/2 then unit of rate constant and rate of reaction respectively is _______.

(a)

(mol L^-1 S^-1),(mol^1/2L^1/2S^-1)

(b)

(mol^-1/2L^1/2s^-1),(mol L^-1s^-1)

(c)

(mol^1/2L^1/2s^-1),(mol L^-1s^-1)

(d)

(mol L s^-1),(mol^1/2L^1/2s)

55.

The crystal with a metal deficiency defect is ________.

(a)

NaCl

(b)

FeO

(c)

ZnO

(d)

KCl

56.

The yellow colour in NaCl crystal is due to ________.

(a)

excitation of electrons in F centers

(b)

reflection of light from Cl^- ion on the surface

(c)

refraction of light from Na⁺ ion

(d)

all of the above

57.

The ratio of close packed atoms to tetrahedral hole in cubic packing is ________.

(a)

1:1

(b)

1:2

(c)

2:1

(d)

1:4

58.

In the Ellingham diagram, for the formation of carbon monoxide________.

(a)

\(\left( \cfrac { \Delta { S }^{ 0 } }{ \Delta T } \right) \) is negative

(b)

\(\left( \cfrac { \Delta { G }^{ 0 } }{ \Delta T } \right) \) is positive

(c)

\(\left( \cfrac { \Delta { G }^{ 0 } }{ \Delta T } \right) \) is negative

(d)

initially \(\left( \cfrac { \Delta T }{ \Delta { G }^{ 0 } } \right) \) is positive, after 700^oC,\(\left( \cfrac { \Delta { G }^{ 0 } }{ \Delta T } \right) \) is negative

59.

Electrochemical process is used to extract_______.

(a)

Iron

(b)

Lead

(c)

Sodium

(d)

silver

60.

Roasting of sulphide ore gives the gas (A).(A) is a colourless gas. Aqueous solution of (A) is acidic. The gas (A) is______.

(a)

CO₂

(b)

SO₃

(c)

SO₂

(d)

H₂S

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Answers Key:

Multiple Choice Question

60 x 1 = 60

(b)
Degree of dissociation

(b)
Lithium ion battery

(b)
O^2-

(b)
Zero

(a)
47.69%

(d)
CO₂

(b)
Concentration of ore

(d)
conductance

10.

11.

12.

(d)
Li

13.

(d)
benzaldehyde

14.

(b)
acetaldehyde

15.

(b)
diastase

16.

17.

(b)
pH = pK_a + log (Salt) / (Acid)

18.

19.

(a)
Riemer-Tiemann reaction

20.

(d)
temperature increases

21.

(a)
intermolecular hydrogen bonding

22.

(a)
Solid in liquid

23.

24.

25.

(a)
C₆H₅- OH

26.

(d)
acetanilide

27.

28.

(a)
CH₃CONHCH₃

29.

(b)
Fehling’s solution

30.

31.

32.

trichloro methane

33.

34.

coagulating power ∝ 1/coagulation value

35.

(b)
III > II > I > IV

36.

Emulsion-Dispersed phase
Dispersion meduun -liquid

37.

Z is tie strongest oxidising agent (High SRP)
X is the strongest reducing agent (Low SRP)

38.

(a)
I and IV

39.

mass of 1 mole of CI₂ gas = 71
∴ mass of 0.1 mole of Cl₂ gas = 7.1 g mol^-1
m = Zlt
t = m/ZI
\(= \frac{7.1}{\frac{71}{2 \times 96500} \times 3}\) (2Cl^- ➝ Cl₂+ 2e^-)
\(= \frac{2 \times 96500 \times 7.1}{71 \times 3}\)
= 6433.33s = 107.2 min

40.

H₃PO₄ + H - OH ⇌ H₃O⁺ + H₂PO₄^-
acid 1 base 1 acid 2 base 2
\(\therefore\) H₂PO₄^- the conjugate base of H₃PO₄

41.

BF₃ → electron deficient → Lewis acid
PF₃ → electron rich → Lewis base
CO → having lone pair of electron → Lewis base
F → unshared pair of electron → Lewis base

42.

Ca(OH)₂ ⇌ Ca²⁺ + 2OH^-
Given that pH = 9
pOH = 14 - 9 = 5
[pOH = - log₁₀ [OH]]
[OH^-] = 10^[pOH]
[OH] = 10^-5 M
Ksp = [Ca²⁺] [OH^-]
= 10^-5/2 x (10^-5)² = 0.5 x 10^-15

43.

44.

(b)
ΔH = 0

45.

(d)
a=b≠c,∝ =β=90°૪=120°

46.

(b)
Space lattice

47.

48.

(b)
Vacancy defect

49.

(a)
Zone refining

50.

(b)
CuCO₃.Cu(OH)₂

51.

(b)
Non-wettability of the mineral particles in water

52.

\({ t }_{ 1/2 }=\frac { 0.6932 }{ k } \)
For a second order reaction
\(\mathrm{t}_{1 / 2}=\frac{2^{\mathrm{n}-1}-1}{(\mathrm{n}-1) \mathrm{k} \cdot\left[\mathrm{A}_{0}\right]^{\mathrm{n}-1}}\)
n = 2
\(\mathrm{t}_{1 / 2}=\frac{2^{\mathrm{2}-1}-1}{(\mathrm{n}-1) \mathrm{k} \cdot\left[\mathrm{A}_{0}\right]^{\mathrm{2}-1}}\)
\(\mathrm{t}_{1 / 2} =\frac{1}{ \mathrm{k}\left[\mathrm{A}_{0}\right]}\)

53.

\(k=\frac { 2.303 }{ t } \log\frac { \left[ { A }_{ 0 } \right] }{ \left[ A \right] } \)
[A₀] = 100: [A] = 25
\(6.909=\frac { 2.303 }{ t } \log\frac { \left[ {100 } \right] }{ \left[ 25\right] } \)
\(t =\frac { 2.303 }{ 6.909 } \log(4)\)
\(t =\frac { 1 }{ 3 } \log(2^2)\)
\(= \left( \frac { 2 }{ 3 } \right) \log2\)

54.

Rate = k[A]ⁿ
Rate = \(\frac{-\mathrm{d}[\mathrm{A}]}{\mathrm{dt}}\)
unit of rate = \(\frac{mol L^{-1}}{s}\)=mol L^-1/s^-1
unit of rate constant
\(=\frac{ (mol{ L }^{ -1 }{ S }^{ -1 }) }{ ({ mol }{ L }^{ -1 })^n } \)
= mol^1-nL^n-1s^-1
in the case
rate = k [Acetone]^3/2
n = 3/2
= mol^1-(3/2)L^(3/2)-1s^-1
(mol^-(1/2)L^(1/2)s^-1).