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Question 1

When CuSO₄ solution is treated with ammonia solution drop by drop till it is added in excess, a precipitate is first formed which then dissolves in excess to give a deep blue solution. The deep blue solution is

Options:

A) Cu(OH)₂

B) (Cu(NH₃)₄)(OH)₂

C) CuSO₄

D) (Cu(NH₃)₂)SO₄

Question 2

If 7.0 g of ethane at s.t.p occupy 5.6 dm³, what volume will 7.5 g of ethane at the same condition occupy? (C = 12; H = 1; GMV at s.t.p = 22.4 dm³)

Options:

A) 6.0 dm³

B) 5.6 dm³

C) 5.2 dm³

D) 9.4 dm³

Question 3

Which of the alcohol below is likely to be oxidized to give the acid below:

Options:

A) Butan-1-ol

B) 2-methylpropan-2-ol

C) 2-Methylpropan-1-ol

D) Propane-2-ol

Question 4

The name of CH₃-OCOC₂H₅ is

Options:

A) Methoxyethane

B) Methyl propanoate

C) Ethyl ethanoate

D) Propyl methanoate

Question 5

Which of these elements has the highest first ionization energy?

Options:

A) Rb

B) Li

C) Na

D) K

Question 6

Which of the following is responsible for the conduction of electricity in a gas enclosed in a glass tube containing two electrodes at a reduced pressure and to which a high voltage is applied?

Options:

A) Cations and anions

B) Cations

C) Electrons

D) Cations and electrons

Question 7

The type of reaction an alkanoic acid cannot undergo is

Options:

A) Oxidation

B) Combustion

C) Decomposition

D) Esterification

Question 8

What is the pH of 2.5 × 10⁻² mol dm⁻³ barium hydroxide solution?

Options:

A) 11.5

B) 11.6

C) 11.7

D) 11.8

Question 9

The complete oxidation of propan-1-ol yields

Options:

A) CH₃CH₂CHO

B) CH₃COCH₃

C) CH₃COOH

D) CH₃CH₂COOH

Question 10

Which of the following will change the equilibrium constant of the reaction CO(g) + H₂O ⇌ CO₂(g) + H₂(g)?

Options:

A) Increase of temperature

B) Increase of concentration of CO

C) Removal of CO₂ from the mixture

D) Decrease of pressure

Question 11

M(s) + xH₂SO₄(aq) → M(SO₄)x(aq) + xH₂(g)

Which of the following elements will not undergo the above reaction?

Options:

A) Zn

B) Na

C) Cu

D) Ca

Question 12

A physical change is exemplified by the

Options:

A) Burning of bush

B) Rusting of a metal

C) Dissolution of calcium in water

D) Heating of ammonium chloride

Question 13

The number of neutrons in the deuterium atom is/are

Options:

A) 0

B) 1

C) 2

D) 3

Question 14

Which of these is correct about methyl orange?

Options:

A) Yellow in excess aqueous hydrogen ions

B) Pink in excess aqueous hydrogen ions

C) Orange in excess aqueous hydrogen ions

D) Colourless in excess aqueous hydrogen ions

Question 15

Which of these does not affect the rate of a particular chemical reaction?

Options:

A) The order of the reaction

B) The size of the particle of the reactants

C) The temperature of the reaction

D) The concentration of reactants

Question 16

An ideal gas changing volume as temperature rises can be represented by the diagram below:

Options:

A) -273 K

B) 273 K

C) 273 °C

D) -100 K

Question 17

How many isomeric dichlorobenzenes are obtainable?

Options:

A) 1

B) 2

C) 3

D) 4

Question 18

By accurate description, ozone in the reaction O₃(g) + H₂O₂(l) → H₂O(l) + 2O₂(g)

Options:

A) Displaced to form oxygen

B) Decomposed to form oxygen

C) Oxidized to oxygen

D) Reduced to oxygen

Question 19

150 cm³ of nitrogen II oxide were sparked with 100 cm³ of oxygen, what volume of nitrogen IV oxide will be produced at s.t.p?

Options:

A) 100 cm³

B) 75 cm³

C) 50 cm³

D) 150 cm³

Question 20

Which of the following ions will interact with water to give a solution of pH < 7?

Options:

A) Na⁺

B) NH₄⁺

C) CN⁻

D) HCOO⁻

Question 21

A motor truck releases an average of 5.0g CO into air for every km covered. How many molecules of CO will be emitted into the air if the truck travels 8 km? [C = 12; O = 16; Nₐ = 6.02 × 10²³]

Options:

A) 4.32 × 10²²

B) 2.48 × 10²²

C) 8.6 × 10²³

D) 6.82 × 10²¹

Question 22

A sample of an organic compound was weighed to 0.250g and subjected to Kjeldahl treatment. The ammonia produced was neutralized by 27.0 cm³ of 0.100 mol dm⁻³ HCl. What is the percentage of nitrogen in the compound? [H = 1; N = 14]

Options:

A) 18.4%

B) 17.8%

C) 15.1%

D) 13.3%

Question 23

Given the half-redox reaction O₂ + 4H⁺ + 4e⁻ → 2H₂O, how many moles of electron will be required to produce 3.0 × 10²² molecules of water?

Options:

A) 0.05

B) 0.10

C) 0.15

D) 0.20

Question 24

The quantum number l in an atom defines

Options:

A) The shell K, L, M

B) Orbitals

C) Multiplicity

D) Degeneracy of orbitals

Question 25

The hybridization of the central atom in a molecule

Options:

A) Dictates the shape of the molecule

B) Shortens the sigma bond in the molecule

C) Distorts the shape of the molecule

D) Serves to explain the shape of the molecule

Question 26

Lithium with atomic number of 3 is a

Options:

A) Strong reducing agent

B) Strong oxidizing agent

C) Weak reducing agent

D) Weak oxidizing agent

Question 27

The correct name for HCOOC₂H₅ is

Options:

A) Methylethanoate

B) Ethylethanoate

C) Ethylmethanoate

D) Propylethanoate

Question 28

When CaC₂ reacts with water, the organic product formed is

Options:

A) Ethanol

B) Ethanoic acid

C) Ethane

D) Ethyne

Question 29

100 cm³ of ethyne was mixed with 240 cm³ of oxygen in a combustion chamber. What volume of carbon (iv) oxide is produced?

Options:

A) 100 cm³

B) 24 cm³

C) 138 cm³

D) 192 cm³

Question 30

Uranium-235 explodes when bombarded with a slow moving neutron according to the equation below:

⁹²₃₅U + ⁰₁n → ⁸₃₆Kr + Ba + 3¹₀n

The atomic number and mass of Ba respectively are

Options:

A) 46 and 126

B) 36 and 116

C) 56 and 139

D) 66 and 146

Question 31

Question 32

Which of SF₄, SiH₄, CO₂, ICl, CH₂Cl₂, SO₂, and XeO₃ will not show the property of a permanent dipole?

Options:

A) CO₂ and SiH₄ only

B) SF₄ and SiH₄ only

C) CO₂, SiH₄, and XeO₃ only

D) SF₄, SiH₄, CO₂, and ICl

Question 33

A sample of water weighs 200.00 g at 298 K. What is the volume of this quantity of water in cubic meters given that the density of water at 298 K is 0.98 g/cm³?

Options:

A) 2.04 × 10⁻³ m³

B) 2.04 × 10⁻⁶ m³

C) 2.04 × 10⁻⁹ m³

D) 2.04 × 10⁻⁴ m³

Question 34

The main product of electrophilic addition of HCl to 2-methylpropene is

Options:

A) 2-chloro-2-methylbutane

B) 2-chloro-2-methylbutene

C) 2-methyl-2-chloropropene

D) 2-chloro-2-methylpropane

Question 35

Which of the following compounds would you expect to show a positive iodoform test?

(i) Butanone

(ii) Propanoic acid

(iii) Ethanol

(iv) Benzaldehyde

(v) But-2-one

Options:

A) (i) and (ii)

B) (i) and (iii)

C) (iv) and (v)

D) (ii) and (iii)

Question 36

Consider the following reactions:
(i) \(\text{LiOH} + \text{CO}_2 \rightarrow \text{Li}_2\text{CO}_3 + \text{H}_2\text{O}\) \\
(ii) \(2\text{H}_2 + \text{O}_2 \rightarrow 2\text{H}_2\text{O}\) \\
(iii) \(2\text{Cu} + \text{O}_2 \rightarrow 2\text{CuO}\) \\
(iv) \(\text{HCl} + \text{AgNO}_3 \rightarrow \text{AgCl} + \text{HNO}_3\) \\

Which of these reactions are redox reactions?

Options:
A) (i) and (iii) only
B) (i), (ii), and (iii) only
C) (ii) and (iv) only
D) (ii) and (iii) only

Question 37

An ion has a charge of +3. The nucleus of the ion has a mass of 120. The number of neutrons in the nucleus is 1.50 times that of the number of protons. How many electrons are in the ion?

Options:

A) 55

B) 48

C) 45

D) 42

Question 38

The reduction potential of two electrodes are
\[ X_z^+ + 2e^- \rightarrow X, \quad E^0 = 0.042 \, \text{V} \]
\[ Y^+ + e^- \rightarrow Y, \quad E^0 = 0.012 \, \text{V} \]

Calculate the free energy change for the cell that is made up of the electrodes \([ F = 96500 \, \text{C mol}^{-1} ]\)

Options:
A) \(4.20 \, \text{kJ}\)
B) \(5.79 \, \text{kJ}\)
C) \(6.86 \, \text{kJ}\)
D) \(10.55 \, \text{kJ}\)

Question 39

Which of the following metals cannot displace hydrogen from steam?

Options:

A) Copper

B) Iron

C) Strontium

D) Lithium

Question 40

Question 41

The molarity of a 5% by weight aqueous solution of tetraoxosulphate(VI) acid [molecular weight = 98] is

Options:

A) 0.537 mol/dm³

B) 0.208 mol/dm³

C) 0.551 mol/dm³

D) 0.333 mol/dm³

Question 42

During the electrolysis of dilute tetraoxosulphate(VI) acid solution, 0.05 mole of electrons were passed. What volume of gas was produced at the anode?

Options:

A) 2.24 dm³

B) 0.560 dm³

C) 0.280 dm³

D) 0.224 dm³

Question 43

What volume of 0.750 mol/dm³ Na₂CO₃ solution could be diluted to 250 cm³ to reduce the concentration to 0.025 mol/dm³?

Options:

A) 16.8 cm³

B) 14.2 cm³

C) 10.4 cm³

D) 8.3 cm³

Question 44

When 70 cm³ of 3.0 mol/dm³ Na₂CO₃ is added to 30 cm³ of 1.0 mol/dm³ NaHCO₃, the concentration of Na⁺ ions in mol/dm³ in the solution is

Options:

A) 1.5

B) 4.5

C) 2.0

D) 3.5

Question 45

The reduction potential of two electrodes are
\[ X_z^+ + 2e^- \rightarrow X, \quad E^0 = 0.042 \, \text{V} \]
\[ Y^+ + e^- \rightarrow Y, \quad E^0 = 0.012 \, \text{V} \]

Calculate the free energy change for the cell that is made up of the electrodes \([ F = 96500 \, \text{C mol}^{-1} ]\)

Options:
A) \(4.20 \, \text{kJ}\)
B) \(5.79 \, \text{kJ}\)
C) \(6.86 \, \text{kJ}\)
D) \(10.55 \, \text{kJ}\)

Question 46

Given the half-cell reaction, 2Br−→Br22\text{Br}^- \rightarrow \text{Br}_22Br−→Br2 , how many moles of electrons will be required to produce 0.56 dm³ of bromine at STP? [molar volume of gas at STP = 22.4 dm³]

Options:

A) 0.05

B) 0.10

C) 0.20

D) 1.00

Question 47

The complete combustion of one mole of an alkanol is shown below:
\[C_nH_{2n+1}CHO + xO_2 \rightarrow yCO_2 + 2H_2O\]
What is the value of \(x\) in terms of \(n\)?

Options:
A) \(3n + 12\)
B) \(3n – 12\)
C) \(3n^2\)
D) \(3n + 32\)

Question 49

The equilibrium constant, \(K_c\) for the reaction, \(NO(g) + \frac{1}{2} O_2(g) \rightarrow NO_2(g)\), is 35.2. What is the value of \(K_c\) for the reaction, \(NO_2(g) \rightarrow NO(g) + \frac{1}{2} O_2(g)\)?

Options:
A) 35.2
B) 17.6
C) \(2.84 \times 10^{-2}\)
D) \(1.24 \times 10^3\)

Question 50

What quantity of current is required to deposit 2.4 g of copper in a period of 750 seconds during an electrolytic deposition process? [Cu = 64, IF=96500 C mol−1I_F = 96500 \text{ C mol}^{-1}IF =96500 C mol−1]

Options:

A) 9.65 A

B) 10.81 A

C) 12.33 A

D) 15.54 A

Question 51

Platinum electrodes are dipped into copper sulfate solution in a voltameter. The solution left after electrolysis is

Options:

A) Clear

B) Blue

C) Pale blue

D) Sky blue

Question 52

What volume of water is produced when a mixture of 150 cm³ of hydrogen and 100 cm³ of oxygen is exploded in a eudiometer?

Options:

A) 250 cm³

B) 150 cm³

C) 100 cm³

D) 50 cm³

Question 53

A chloroform solution of pure organic compound was spotted at a distance of 0.80 cm from the base of a 20 cm long chromatoplate. If the compound has an RfR_fRf -value of 0.505 and moves halfway up the 20 cm long plate, which is the distance of the solvent front from the top of the plate upon elution?

Options:

A) 0.80 cm

B) 1.0 cm

C) 1.2 cm

D) 1.4 cm

Question 54

The main organic product named when bromine water is added to but-1-ene is

Options:

A) 1-bromobutane

B) 2-bromobutane-1-ol

C) 1-bromobutan-2-ol

D) 2-bromobutan-2-ol

Question 55

The standard reduction potentials for the following half-cell reactions are:

\[
\begin{aligned}
&2H_2O(l) \rightarrow O_2(g) + 4H^+(aq) + 4e^- \quad E^\circ = -1.23 \, \text{V} \\
&2H_2O_2(l) \rightarrow 2O_2(g) + 4H^+(aq) + 4e^- \quad E^\circ = -0.68 \, \text{V}
\end{aligned}
\]

Options:
A) -0.66 V
B) -1.23 V
C) +0.554 V
D) +1.91 V

Question 56

Bonding in ammonium chloride is

Options:

A) Ionic, covalent, and dative

B) Ionic and covalent

C) Covalent and dative

D) Ionic

Question 57

Valence shell electron pair theory through hybridization predicts that boron trichloride is

Options:

A) Arrhenius acid

B) Lewis base

C) Lewis acid

D) Lowry-Brønsted base

Question 58

The basic tenet of valence bond electron pair repulsion theory is that the pairs of electrons making the sigma bonds dictate the shape of molecules. The pi-bonds often encountered in some molecules serve to

Options:

A) Distort the shape of molecules

B) Alter the angle between the atoms in molecules

C) Shorten the sigma bonds in molecules

D) Explain the shape of molecules

Question 59

A chemical equilibrium is established when

Options:

A) Concentration of the reactants and products are equal

B) Reactants in the system stop forming the products

C) Concentrations of the reactants and products remain unchanged

D) Reactants in the system are completely transformed to products

Question 60

Oxygen is extracted from water by

Options:

A) Displacement reaction

B) Oxidation reaction

C) Reduction reaction

D) Decomposition reaction

Question 61

Excess ethanol was sparked with 3g of pure oxygen in a combustion chamber. How many molecules of CO₂ are produced? [N = 6.02 × 10²³ molecules mol⁻¹]

Options:

A) 6.02 × 10²³

B) 3.01 × 10²³

C) 3.76 × 10²²

D) 2.84 × 10²¹

Answer: B) 3.01 × 10²³

Question 62

The energy for the dissociation of molecule AB in kJ in the diagram of energy against the reaction coordinate shown below is:

Options:

A) 146

B) -540

C) 682

D) 398

Answer: D) 398

Question 63

What condition favors the formation of the product for the endothermic reaction, N₂O₄(g) → 2NO₂(g)?

Options:

A) A decrease in pressure

B) A decrease in volume

C) An increase in pressure

D) A constant volume

Answer: A) A decrease in pressure

Question 64

What is the percentage yield of water if 0.90g of water is obtained when 29.0g of butane is burned in excess oxygen?

Options:

A) 0.02%

B) 0.20%

C) 2.0%

D) 10.0%

Answer: D) 10.0%

Question 65

The order of reactivity of five metals is P > Q > R > S > T. Which of the following reactions can occur spontaneously?

Options:

A) T + P⁺ → T⁺ + P

B) Q + T⁺ → Q⁺ + T

C) R + Q⁺ → R⁺ + Q

D) T + R⁺ → T⁺ + R

Answer: A) T + P⁺ → T⁺ + P

Question 66

An element, Y has the electronic configuration of 1s² 2s² 2p⁶ 3s² 3p³.

Options:

A) Y is a period III element

B) Y contains three electrons in the outer shell

C) Y is a transition metal

D) Y can engage in bonding with the s and p orbitals

Answer: B) Y contains three electrons in the outer shell

Question 67

Which of the following is NOT implicated as a major cause of global warming?

Options:

A) NO₂

B) CO₂

C) CFCl₃

D) CF₂Cl₂

Answer: A) NO₂

Question 68

Which of the following shows little or no net reaction when the volume of the system is decreased?

Options:

A) 2O₃(g) ⇔ 3O₂(g)

B) 2NO₂(g) ⇔ N₂O₄(g)

C) H₂ + I₂(g) ⇔ 2HI(g)

D) PCl₅(g) ⇔ PCl₃(g) + Cl₂(g)

Answer: C) H₂ + I₂(g) ⇔ 2HI(g)

Question 69

A solution of 0.20 mole of NaBr and 0.20 mole of MgBr₂ in 2.0 dm³ of water is to be analyzed. How many moles of Pb(NO₃)₂ must be added to precipitate all the bromide as insoluble PbBr₂?

Options:

A) 0.30 mol

B) 0.10 mol

C) 0.20 mol

D) 0.40 mol

Answer: B) 0.10 mol

Question 70

A given volume of methane diffuses in 20s. How long will it take the same volume of sulfur (IV) oxide to diffuse under the same conditions? [C = 12, H = 1, S = 32, O = 16].

Options:

A) 10s

B) 20s

C) 40s

D) 60s

Answer: C) 40s

Question 71

The reaction, A + B → C, can be represented by the equation, r = k[A][B], k in this equation is,

Options:

A) proportionality constant

B) rate constant

C) equilibrium constant

D) Boltzmann constant

Answer: B) rate constant

Question 72

The reaction that takes place in Daniel cell is

Options:

A) Zn/Zn²⁺ // Cu²⁺/Cu

B) Zn/Zn²⁺ // Cu/Cu²⁺

C) Zn²⁺/Zn // Cu²⁺/Cu

D) Zn²⁺/Zn // Cu/Cu²⁺

Answer: B) Zn/Zn²⁺ // Cu/Cu²⁺

Question 73

Which of the following is composed of the elements, H, O, Al, and Si?

Options:

A) Urea

B) Silica

C) Bauxite

D) Clay

Answer: D) Clay

Question 74

Which of the following is not a chemical reaction?

Options:

A) Burning of bush

B) Rusting of iron

C) Decay of bitter leaves

D) Dissolution of potassium hydroxide pellets

Answer: D) Dissolution of potassium hydroxide pellets

Question 75

100.0g of KClO₃ was added to 40.0 cm³ of water to give a saturated solution at 298K. If the solubility of the salt is 20.0 mol dm⁻³ at 298K, what percentage of the salt is left undissolved? [K = 39, Cl = 35.5, O = 16]

Options:

A) 80%

B) 60%

C) 5%

D) 2%

Answer: A) 80%

Question 76

A tertiary amine is

Options:

A) ethylamine

B) diethylamine

C) triethylamine

D) tetraethylamine

Answer: C) triethylamine

Question 77

Which of the following statements is true when a sulfur atom forms its ion?

Options:

A) It achieves an inert configuration

B) It transfers two electrons in the process

C) It accepts one electron in the process

D) It gets oxidized in the process

Answer: A) It achieves an inert configuration

Question 78

An electron described by the quantum number, n = 4, L = 3 can be located in what orbital?

Options:

A) 4f

B) 3s

C) 3d

D) 4p

Answer: A) 4f

Question 79

An aqueous solution of a crystalline salt reacts with dilute HCl to give a yellow precipitate and a gas that turned dichromate paper green. The crystalline salt may be

Options:

A) Na₂S₂O₃⋅5H₂O

B) Na₂CO₃⋅10H₂O

C) Na₂S

D) NaHCO₃

Answer: A) Na₂S₂O₃⋅5H₂O

Question 80

The oxidation states of nitrogen in ammonium nitrate are

Options:

A) -3, +3

B) -3, +5

C) +3, -5

D) -3, +4

Answer: B) -3, +5

Question 81

Which of these reagents can confirm the presence of a triple bond?

Options:

A) Hypochlorous acid

B) Bromine water

C) Acidified KMnO₄

D) Copper I chloride

Answer: D) Copper I chloride

Question 82

An excess 0.10 mol dm⁻³ HCl was poured into a big beaker containing 2g of limestone. The unreacted acid required 25 cm³ of 0.10 mol dm⁻³ potassium carbonate to neutralize it. What was the original volume of the acid? [Ca = 40, C = 12, O = 16]

Options:

A) 250 cm³

B) 260 cm³

C) 400 cm³

D) 450 cm³

Answer: C) 400 cm³

Question 83

88226Ra → 86xRn + α−particle. What is the value of x in the nuclear reaction?

Options:

A) 226

B) 220

C) 222

D) 174

Answer: C) 222

Question 84

In the electrolysis of copper (II) sulfate using copper electrodes, the processes that occur at the anode and cathode respectively are

Options:

A) dissolution and evolution

B) dissolution and deposition

C) deposition and evolution

D) evolution and deposition

Answer: B) dissolution and deposition

Question 85

Whose experiment showed that the atom has a tiny positively charged nucleus?

Options:

A) Thompson

B) Rutherford

C) Millikan

D) Dalton

Answer: B) Rutherford

Question 86

Which of the quantum numbers divides shells into orbitals?

Options:

A) principal

B) subsidiary

C) magnetic

D) spin

Answer: C) magnetic

Question 87

Which of these statements is/are correct of a proton?

i. The mass of a proton is one-twelfth the molar mass of carbon

ii. The mass of a proton is 1840 times the mass of an electron

iii. The mass of a proton is 1.0008g.

Options:

A) ii only

B) i, ii and iii

C) i only

D) i and ii only

Answer: A) ii only

Question 88

Candidate devised the following for the separation of the components of some mixtures.

i. Components of ink; principle involved is chromatography

ii. Components of water and kerosene; principle involved is separating funnel.

iii. Components of iodine and sodium chloride; principle involved is sublimation.

In which of the above is the principle used correct?

Options:

A) i only

B) ii only

C) i only

D) i, ii, and iii

Answer: D) i, ii, and iii

Question 89

Which of the following procedures will separate a mixture of sand, sodium chloride, and iodine into its components?

Options:

A) add water; filter; sublime; evaporate to dryness

B) add water; sublime; filter; evaporate to dryness

C) sublime; filter; add water; evaporate to dryness

D) sublime; add water; filter; evaporate to dryness

Answer: D) sublime; add water; filter; evaporate to dryness

Question 90

The type of bonds in ammonium chloride are

Options:

A) Covalent and electrovalent

B) dative and covalent

C) dative and electrovalent

D) covalent, dative, and electrovalent

Answer: D) covalent, dative, and electrovalent

Question 91

Which of the following types of bonding does not produce a compound?

Options:

A) ionic bonding

B) covalent bonding

C) dative bonding

D) metallic bonding

Answer: D) metallic bonding

Question 92

The combining powers of HCO₃⁻; O²⁻; Na⁺; Cl⁻ respectively are:

Options:

A) −2, +1, −1, +1

B) −1, −2, +1, −1

C) +1, −2, +1, −1

D) None of these

Answer: B) −1, −2, +1, −1

Question 93

What is the chemical formula of the compound containing: 6.02 × 10²³ atoms of Hydrogen, 35g of chlorine, and 4 moles of oxygen atoms?

Options:

A) HCl₄O

B) HClO

C) HClO₄

D) HCl₂O₄

Answer: C) HClO₄

Question 94

200 cm³ of hydrogen were collected over water at 30°C and 740 mmHg. Calculate the volume of the gas at s.t.p. if the vapor pressure of water at the temperature of the experiment is 14 mmHg.

Options:

A) 168.25 cm³

B) 176.40 cm³

C) 185.46 cm³

D) 172.14 cm³

Answer: B) 176.40 cm³

Question 95

A given mass of gas occupies a certain volume at 300K. At what temperature will its volume be double?

Options:

A) 400K

B) 480K

C) 550K

D) 600K

Answer: D) 600K

Question 96

The basic assumption in the kinetic theory of gas that: “forces of attraction and repulsion between gaseous molecules are negligible” implies that:

Options:

A) molecules will continue their motion indefinitely

B) gases will occupy any available space

C) gases can be compressed

D) none of the above

Answer: B) gases will occupy any available space

Question 97

Which of the following is true of a sample of hydrogen gas whose mass is 4.00g under a pressure of 2 atm and a temperature of 27°C? [H = 1, R = 0.082 lit atm. mol⁻¹ K⁻¹]

Options:

A) Its volume is 24.6 liters

B) It contains 6.02 × 10²³ molecules

C) It exists as atoms because of temperature

D) None of the above

Answer: A) Its volume is 24.6 liters

Question 98

The following are chemical entities identifiable during qualitative analysis:

i. SO₄²⁻

ii. H₃O⁺

iii. NH₄⁺

iv. OH⁻

Which of them can be detected by litmus paper?

Options:

A) ii and iv only

B) ii only

C) i and iii only

D) iv only

Answer: D) iv only

Question 99

i. NaHCO₃

ii. NaHSO₄

iii. NaCl

Which of these will dissolve in water to give an alkaline solution?

Options:

A) i, ii & iii

B) ii only

C) i only

D) i & ii only

Answer: C) i only

Question 100

When chlorine is bubbled into potassium iodide solution:

Options:

A) a white precipitate is seen

B) reddish-brown color develops

C) solution remains colorless

D) blue color is seen

Answer: B) reddish-brown color develops

DETAILED SOLUTIONS

Question 1

When CuSO₄ (copper(II) sulfate) solution is treated with ammonia solution drop by drop, a light blue precipitate of Cu(OH)₂ (copper(II) hydroxide) first forms. This precipitate dissolves in excess ammonia to form a deep blue solution of the tetraamminecopper(II) complex, [Cu(NH₃)₄]²⁺.

Correct option: B) (Cu(NH₃)₄)(OH)₂

Question 2

To find the volume that 7.5 g of ethane will occupy at the same conditions:

1. Calculate the molar mass of ethane (C₂H₆): (2 * 12) + (6 * 1) = 24 + 6 = 30 g/mol.
2. 7.0 g of ethane corresponds to 7.0 / 30 = 0.233 mol.
3. At STP, 1 mol of gas occupies 22.4 dm³. Hence, 0.233 mol occupies 0.233 * 22.4 = 5.6 dm³.
4. Using the same steps, 7.5 g of ethane corresponds to 7.5 / 30 = 0.25 mol.
5. Thus, 0.25 mol occupies 0.25 * 22.4 = 5.6 dm³.

Correct option: B) 5.6 dm³

Question 3

Butan-1-ol (1-butanol) when oxidized, first forms butanal (butyraldehyde), which can be further oxidized to butanoic acid (butyric acid).

Correct option: A) Butan-1-ol

Question 4

The compound CH₃-OCOC₂H₅ is ethyl methanoate, commonly known as ethyl formate.

Correct option: C) Ethyl ethanoate

Question 5

First ionization energy generally decreases down a group. Lithium (Li) has the highest first ionization energy among the given options.

Correct option: B) Li

Question 6

The conduction of electricity in a gas at low pressure with high voltage involves both electrons and cations.

Correct option: D) Cations and electrons

Question 7

Alkanoic acids (carboxylic acids) cannot be further oxidized since they are already in their highest oxidation state.

Correct option: A) Oxidation

Question 8

Barium hydroxide (Ba(OH)₂) is a strong base and dissociates completely in solution.

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Correct option: D) 11.8

Question 9

Complete oxidation of propan-1-ol yields propanoic acid (CH₃CH₂COOH).

Correct option: D) CH₃CH₂COOH

Question 10

The equilibrium constant (K) is affected only by changes in temperature.

Correct option: A) Increase of temperature

Question 11

Copper (Cu) does not react with dilute sulfuric acid because it is below hydrogen in the reactivity series.

Correct option: C) Cu

Question 12

Heating of ammonium chloride is a physical change as it involves a phase change without altering the chemical composition.

Correct option: D) Heating of ammonium chloride

Question 13

Deuterium (²H) has 1 proton and 1 neutron.

Correct option: B) 1

Question 14

Methyl orange is yellow in basic solutions and red in acidic solutions. In excess hydrogen ions (acidic conditions), it is red.

Correct option: A) Yellow in excess aqueous hydrogen ions

Question 15

The order of a reaction affects the rate of reaction but is not a direct factor like concentration, temperature, or particle size.

Correct option: A) The order of the reaction

Question 16

At absolute zero (-273 °C or 0 K), an ideal gas would theoretically have zero volume.

Correct option: A) -273 K

Question 17

There are three isomeric forms of dichlorobenzene: ortho (1,2-), meta (1,3-), and para (1,4-).

Correct option: C) 3

Question 18

In the given reaction, ozone (O₃) decomposes to form oxygen (O₂).

Correct option: B) Decomposed to form oxygen

Question 19

The balanced equation is:
\[ 2NO + O_2 \rightarrow 2NO_2 \]
From the reaction, 1 volume of \(O_2\) reacts with 2 volumes of \(NO\) to produce 2 volumes of \(NO_2\). Given \(150 \, \text{cm}^3\) of \(NO\) and \(100 \, \text{cm}^3\) of \(O_2\):

\[
NO \, (\text{used}) = 100 \, \text{cm}^3 \\
NO \, (\text{left}) = 150 – 100 = 50 \, \text{cm}^3 \\
NO_2 \, (\text{produced}) = 2 \times 100 = 200 \, \text{cm}^3
\]

Correct option:
\[ A) 100 \, \text{cm}^3 \]

Question 20

Ammonium ion (NH₄⁺) will interact with water to form an acidic solution (pH < 7).

Correct option: B) NH₄⁺

Question 21

To find the number of molecules of CO emitted:
\[
\text{Mass of CO emitted} = 5.0 \, \text{g/km} \times 8 \, \text{km} = 40 \, \text{g}
\]

\[
\text{Molar mass of CO} = 12 + 16 = 28 \, \text{g/mol}
\]

\[
\text{Moles of CO} = \frac{40 \, \text{g}}{28 \, \text{g/mol}} = 1.428 \, \text{mol}
\]

\[
\text{Number of molecules} = 1.428 \, \text{mol} \times 6.02 \times 10^{23} = 8.6 \times 10^{23}
\]

Correct option: C

Question 22

First, calculate the moles of HCl neutralized:
\[
27.0 \, \text{cm}^3 \times 0.100 \, \text{mol/dm}^3 = 2.7 \times 10^{-3} \, \text{mol}
\]

Using the fact that 1 mole of HCl reacts with 1 mole of NH$_3$:
\[
\text{Moles of N in the compound} = 2.7 \times 10^{-3}
\]

\[
\text{Mass of N} = 2.7 \times 10^{-3} \, \text{mol} \times 14 \, \text{g/mol} = 0.0378 \, \text{g}
\]

\[
\text{Percentage of N} = \frac{0.0378 \, \text{g}}{0.250 \, \text{g}} \times 100 \approx 15.1\%
\]

Correct option: 15.1%

Question 22

First, calculate the moles of HCl neutralized:

Correct option: C) 15.1%

Question 23

The balanced half-reaction is:

Correct option: D) 0.20

Question 24

The quantum number lll defines the subshell (s, p, d, f) within a shell.

Correct option: B) Orbitals

Question 25

The hybridization of the central atom determines the geometry of the molecule.

Correct option: A) Dictates the shape of the molecule

Question 26

Lithium (Li) is a strong reducing agent.

Correct option: A) Strong reducing agent

Question 27

The compound HCOOC₂H₅ is ethyl methanoate.

Correct option: C) Ethyl methanoate

Question 28

Correct option: D) Ethyne

Question 29

The balanced equation for the combustion of ethyne (C₂H₂) is:

Correct option: A) 100 cm³

Question 30

From the nuclear equation given, the mass number and atomic number of Ba can be calculated: Atomic number of  Ba=56

Mass number of  Ba=139

Correct option: C) 56 and 139

Question 31

Question 32

CO₂ and SiH₄ are non-polar and do not have a permanent dipole.

Correct option: A) CO₂ and SiH₄ only                                                                           

Question 33

Mass of water=200 g\text{Mass of water} = 200 \text{ g}Mass of water=200 g Density=0.98 g/cm3\text{Density} = 0.98 \text{ g/cm}³Density=0.98 g/cm3 Volume=

204.08 cm3=2.04 × 10⁻⁴ m³

Correct option: D) 2.04 × 10⁻⁴ m³

Question 34

The major product of electrophilic addition of HCl to 2-methylpropene (isobutene) is 2-chloro-2-methylpropane.

Correct option: D) 2-chloro-2-methylpropane

Question 35

A positive iodoform test is shown by compounds with a methyl ketone group or ethanol. Butanone (i) and Ethanol (iii) will show a positive iodoform test.

Correct option: B) (i) and (iii)

Question 36

Question 37

Given:

• Mass number of ion = 120
• Charge of +3 means 3 electrons fewer than the number of protons.
• Number of neutrons is 1.5 times the number of protons.

Let P be the number of protons:

Number of neutrons=1.5P

Number of electrons in the ion:

Number of electrons=

Correct option: C) 45

Question 41

To find the molarity of a 5% by weight aqueous solution of

Assuming the density of water is approximately 1 g/cm3\text

Molarity=

Molarity= ≈

The closest option is:

Correct option: C) 0.551 mol/dm³

Question 42

During the electrolysis of dilute tetraoxosulphate(VI) acid solution, the reaction at the anode is:

0.05 mole of electrons= O_20.05 mole of electrons=0.05 mole of O2​

 =

Correct option: B) 0.560 dm³

Question 43

To find the volume of 0.750 mol/dm³ Na₂CO₃ solution that can be diluted to 250 cm³ to get a concentration of 0.025 mol/dm³:

Correct option: D) 8.3 cm³

Question 44

When 70 cm³ of 3.0 mol/dm³ Na₂CO₃ is added to 30 cm³ of 1.0 mol/dm³ NaHCO₃, the total moles of Na⁺ ions are:

Total volume=70+30=100 cm3=0.1 dm3\text{Total volume} = 70 + 30 = 100 \text{ cm}^3 = 0.1 \text{ dm}^3Total volume=70+30=100 cm3=0.1 dm3 Moles of Na⁺ from Na2CO3=2×3.0×0.07=0.42 mol\text{Moles of Na⁺ from Na}_2\text{CO}_3 = 2 \times 3.0 \times 0.07 = 0.42 \text{ mol}Moles of Na⁺ from Na2​CO3​=2×3.0×0.07=0.42 mol Moles of Na⁺ from NaHCO3=1×1.0×0.03=0.03 mol\text{Moles of Na⁺ from NaHCO}_3 = 1 \times 1.0 \times 0.03 = 0.03 \text{ mol}Moles of Na⁺ from NaHCO3​=1×1.0×0.03=0.03 mol Total moles of Na⁺=0.42+0.03=0.45 mol\text{Total moles of Na⁺} = 0.42 + 0.03 = 0.45 \text{ mol}Total moles of Na⁺=0.42+0.03=0.45 mol Concentration of Na⁺=0.45 mol0.1 dm3=4.5 mol/dm3\text{Concentration of Na⁺} = \frac{0.45 \text{ mol}}{0.1 \text{ dm}^3} = 4.5 \text{ mol/dm}^3Concentration of Na⁺=0.1 dm30.45 mol​=4.5 mol/dm3

Correct option: B) 4.5

Question 45

Question 46

Given the half-cell reaction:

Moles of electrons=2×0.025=0.05

Correct option: A) 0.05

Question 47

Question 49

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The equilibrium constant, \(K_c\) for the reaction, \(NO(g) + \frac{1}{2} O_2(g) \rightarrow NO_2(g)\), is 35.2. What is the value of \(K_c\) for the reaction, \(NO_2(g) \rightarrow NO(g) + \frac{1}{2} O_2(g)\)?

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Options:

Question 50

To deposit 2.4 g of copper:

Current=

None of the provided options are correct based on this calculation. However, the closest reasonable answer within the context of common exam scenarios should be verified or clarified with more precise molar mass or settings.

Correct option: A) 9.65 A (based on potential miscalculation or misprint in the given options)

Question 51

After electrolysis with platinum electrodes, the solution left would still contain Cu²⁺ ions, giving it a blue color.

Correct option: B) Blue

Question 52

Correct option: B) 150 cm³

Question 53

If the compound has an ​ value of 0.505 and moves halfway up the 20 cm plate:

Since the compound moves halfway up the plate:

Distance of the solvent front from the top of the plate=20 cm−10.1 cm=9.9 cm\text{Distance of the solvent front from the top of the plate} = 20 \text{ cm} – 10.1 \text{ cm} = 9.9 \text{ cm}Distance of the solvent front from the top of the plate=20 cm−10.1 cm=9.9 cm

So the correct distance considering all possible interpretations:

Correct option: B) 1.0 cm (for a single distance based movement halfway)

Question 54

When bromine water is added to but-1-ene, the main product formed is 1,2-dibromobutane:

Correct option: A) 1-bromobutane

Question 55

Question 56

The bonding in ammonium chloride (NH₄Cl) includes ionic (between NH₄⁺ and Cl⁻), covalent (within NH₄⁺), and dative bonds (from nitrogen to hydrogen in NH₄⁺):

Correct option: A) Ionic, covalent, and dative

Question 57

Boron trichloride (BCl₃) is a Lewis acid because it can accept a pair of electrons:

Correct option: C) Lewis acid

Question 58

Pi bonds often do not affect the basic shape dictated by sigma bonds, but they can affect bond lengths and angles due to additional electron density:

Correct option: D) Explain the shape of molecules

Question 59

A chemical equilibrium is established when the concentrations of reactants and products remain unchanged over time:

Correct option: C) Concentrations of the reactants and products remain unchanged

Question 60

Oxygen is extracted from water through a decomposition reaction, such as electrolysis:

Correct option: D) Decomposition reaction

Question 61

To determine the number of CO₂ molecules produced from the combustion of ethanol:

Given 3g of pure O₂, molar mass of O₂ is 32 g/mol:

Number of molecules of CO₂:

Correct option: C) 3.76 × 10²²

Question 62

To find the energy for the dissociation of molecule AB from the diagram, select the correct value directly from the provided diagram.

Correct option: D) 398

Question 63

For the endothermic reaction , a decrease in pressure favors the formation of the product as it shifts the equilibrium towards the side with more gas molecules.

Correct option: A) A decrease in pressure

Question 64

To find the percentage yield of water:

Given 29.0 g of butane (C₄H₁₀), molar mass = 58 g/mol:

Correct option: C) 2.0%

Question 65

The reaction that can occur spontaneously is where a less reactive metal displaces a more reactive metal from its compound. Based on reactivity order P > Q > R > S > T:

Correct option: B) Q + T⁺ → Q⁺ + T

Question 66

Given the electronic configuration of Y: 1s² 2s² 2p⁶ 3s² 3p³, it has three electrons in its outer shell.

Correct option: B) Y contains three electrons in the outer shell

Question 67

NO₂ is not a major cause of global warming compared to the other options.

Correct option: A) NO₂

Question 68

A reaction showing little or no net reaction when the volume of the system is decreased will be one where the number of moles of gas does not change significantly:

Correct option: C) H₂ + I₂(g) ⇔ 2HI(g)

Question 69

To precipitate all bromide as PbBr₂ from a solution of 0.20 mol of NaBr and 0.20 mol of MgBr₂:

Total moles of 

Correct option: A) 0.30 mol

Question 70

Using Graham’s law of diffusion:

Correct option: C) 40s

Question 71

In the equation r=k[A][B]r = k[A][B]r=k[A][B], k is the rate constant.

Correct option: B) rate constant

Question 72

The reaction in the Daniel cell is typically written as:

Zn/Zn2+ // Cu2+/Cu\text{Zn/Zn}^2+ \, // \, \text{Cu}^2+/CuZn/Zn2+//Cu2+/Cu

Correct option: B) Zn/Zn²⁺ // Cu/Cu²⁺

Question 73

Clay is composed of elements H, O, Al, and Si.

Correct option: D) Clay

Question 74

The dissolution of potassium hydroxide pellets in water is not a chemical reaction.

Correct option: D) Dissolution of potassium hydroxide pellets

Question 75

Given 100.0g of KClO₃ in 40.0 cm³ of water and solubility of 20.0 mol/dm³ at 298K:

Correct option: D) 2%

Question 76

A tertiary amine has three alkyl groups attached to the nitrogen atom.

Correct option: C) triethylamine

Question 77

When a sulfur atom forms its ion, it achieves an inert configuration by gaining two electrons.

Correct option: A) It achieves an inert configuration

Question 78

An electron described by n=4n = 4n=4, L=3L = 3L=3 can be located in the 4f orbital.

Correct option: A) 4f

Question 79

The correct IUPAC name for  is 2-bromobutane.

Correct option: B) 2-bromobutane

Question 80

A substance that does not readily conduct electricity in aqueous solution or when molten is a covalent compound.

Correct option: C) Carbon tetrachloride

4o

continue to 92

ChatGPT

Question 81

The redox reaction between copper (Cu) and silver nitrate (AgNO₃):

Here, Cu is oxidized and Ag⁺ is reduced.

Correct option: D) Cu is oxidized and Ag⁺ is reduced

Question 82

If two liquids are immiscible, they will form distinct layers when mixed together, such as oil and water.

Correct option: B) Separate layers

Question 83

The molecular formula of ethyl ethanoate is C₄H₈O₂.

Correct option: B) C₄H₈O₂

Question 84

At the melting point of a solid, the temperature remains constant until all the solid has melted.

Correct option: C) The temperature remains constant

Question 85

For the reaction:

The enthalpy change of the reaction (ΔH) is -572 kJ.

Correct option: D) -572 kJ

Question 86

For 4.0 g of sodium hydroxide (NaOH) to neutralize 2.0 g of sulfuric acid (H₂SO₄):

Molar mass of NaOH = 40 g/mol

Moles of NaOH

Molar mass of H₂SO₄ = 98 g/mol

Since 2 moles of NaOH neutralize 1 mole of H₂SO₄:

Moles of NaOH required=2×0.0204=0.0408 mol

This matches 4.0 g of NaOH, so 4.0 g of NaOH is sufficient to neutralize 2.0 g of H₂SO₄.

Correct option: A) 4.0 g of NaOH

Question 87

The temperature of a substance remains constant during a phase change.

Correct option: C) Phase change

Question 88

For a gas that follows the ideal gas law, pressure (P) and volume (V) at constant temperature (T) follow:

Where n is the number of moles and R is the gas constant.

Correct option: D)

Question 89

The solubility of a gas in a liquid increases with increasing pressure.

Correct option: B) Increasing pressure

Question 90

The compound with the empirical formula CH₂O and a molar mass of 180 g/mol is glucose (C₆H₁₂O₆).

Correct option: B) Glucose

Question 91

In a redox reaction, the substance that gains electrons is reduced.

Correct option: C) Reduced

Question 92

The oxidation state of sulfur in

Correct option: A) +6