Considering Ellingham diagram, which of the following metals can be used to reduce alumina? 

(a)

Fe

(b)

Cu

(c)

Mg

(d)

Zn

Which of the following is not true with respect to Ellingham diagram?

(a)

Free energy changes follow a straight line. Deviation occurs when there is a phase change.

(b)

The graph for the formation of CO₂ is a straight line almost parallel to free energy axis.

(c)

Negative slope of CO shows that it becomes more stable with increase in temperature.

(d)

Positive slope of metal oxides shows that their stabilities decrease with increase in temperature.

Name the process by which elements such as germanium, silicon and gallium are refined.

(a)

Vapour phase method

(b)

Electrolytic refining

(c)

Zone refining

(d)

Van-Arkel method

Identify the halide ore among the following

(a)

Epsom Salt

(b)

Pyrolusite

(c)

Anglesite

(d)

Rock Salt

Ignition mixture used in aluminothermic process is ________.

(a)

Cr + AI₂O₃

(b)

Mg + BaO₂

(c)

AI + Cr₂O₃

(d)

Ba + MgO

Boric acid is an acid because its molecule________.

(a)

contains replaceable H⁺ ion

(b)

gives up a proton

(c)

combines with proton to form water molecule

(d)

accepts OH^- from water, releasing proton.

Oxidation state of carbon in its hydrides _______.

(a)

+4

(b)

-4

(c)

+3

(d)

+2

Graphite has _______.

(a)

2-d sheet structure

(b)

Vander waals force between successive layers of carbon sheets

(c)

Sp² hybridised carbon linked with other three carbon atoms in hexagonal planar structure

(d)

all the above

Aluminium is used for making alloys because of its _____

(a)

resistance to corrosion

(b)

poor conductivity

(c)

heaviness

(d)

all of these

Group 14 elements have general electronic configuration _______.

(a)

ns²

(b)

ns²np⁴

(c)

ns²np⁶

(d)

ns²np²

P₄O₆ reacts with cold water to give _______.

(a)

H₃PO₃

(b)

H₄P₂O₇

(c)

HPO₃

(d)

H₃PO₄

On oxidation with iodine, sulphite ion is transformed to _______.

(a)

S₄O₆^2-

(b)

S₂O₆^2-

(c)

SO₄^2-

(d)

SO₃^2-

Which is dibasic?

(a)

Orthophosphoric acid

(b)

Pyrophosphoric acid

(c)

Orthophosphorus acid

(d)

Hypophosphorous acid

Oxalic acid on heating with cone H₂SO₄ gives ______.

(a)

CO only

(b)

CO₂ only

(c)

CO₂ + H₂O

(d)

CO + CO₂ + H₂O

Orthophosphorus acid on heating gives______.

(a)

Hypophosphorous

(b)

Orthophosphoric acid

(c)

Phosphine gas

(d)

both (b) and (c)

Among the transition metals of 3d series, the one that has highest negative \(\left( \frac { M^{ 2+ } }{ M } \right) \) standard electrode potential is _______.

(a)

Ti

(b)

Cu

(c)

Mn

(d)

Zn

Which of the following compounds is colourless?

(a)

Fe³⁺

(b)

Ti⁴⁺

(c)

Co²⁺

(d)

Ni²⁺

Ce (Z=58) and Yb (Z=70) exhibits stable +4 and +2 oxidation states respectively. This is because_______.

(a)

Ce⁴⁺ and Yb²⁺acquire f⁷ configuration

(b)

Ce⁴⁺ and Yb²⁺ acquire f⁰ configuration

(c)

Ce⁴⁺ and Yb²⁺acquire f⁷ and f¹⁴ configuration

(d)

Ce⁴⁺and Yb²⁺ acquire f⁰ and f¹⁴ configuration

Which of the following ions will exhibit colour in aqueous solutions?

(a)

SC³⁺(Z=21)

(b)

Ti³⁺(Z =22)

(c)

La³⁺(Z=57)

(d)

Lu³⁺(Z=71)

FeSO₄ on heating gives _______.

(a)

SO₂ and O₂

(b)

SO₂ and SO₃

(c)

SO₂

(d)

SO₃

A complex in which the oxidation number of the metal is zero is_______.

(a)

K₄[Fe(CN)₆]

(b)

[Fe(CN)₃(NH₃)₃]

(c)

[Fe(CO)₅]

(d)

both (b) and (c)

Which of the following is paramagnetic in nature?

(a)

[Zn(NH₃)₄]²⁺

(b)

[Co(NH₃)₆]³⁺

(c)

[Ni(H₂O)₆]²⁺

(d)

[Ni(CN)₄]^2-

Which of the following co-ordination compounds would exhibit optical isomerism?

(a)

Pemtaamminenitrocobalt (III) iodide

(b)

Diamminedichloropaltinum (II)

(c)

Tris-(ethylenediamine) cobalt (III) bromide

(d)

Transdicyanobis( ethylenediamine) chromium (III) chloride

According to IUPAC, No is _________.

(a)

nitro

(b)

nitrosyl

(c)

nitrate

(d)

nitrito

The structure of hexaaquatitanium (III) ion is _______.

(a)

[Ti(H₂O)₆]³⁺

(b)

[Ti(H₂O)₆]^3-

(c)

[Ti(H₂O)₅]H₂O

(d)

[Ti(H₂O)₆]

Assertion: monoclinic sulphur is an example of monoclinic crystal system
Reason: for a monoclinic system, \(a\neq b\neq c\) and \(\alpha =\gamma ={ 90 }^{ 0 },\beta \neq { 90 }^{ 0 }\) 
Codes:
a) Both assertion and reason are true and reason is the correct explanation of assertion
b) Both assertion and reason are true but reason is not the correct explanation of assertion.
c) Assertion is true but reason is false.
d) Both assertion and reason are false.

(a)

Both assertion and reason are true and reason is the correct explanation of assertion

(b)

Both assertion and reason are true but reason is not the correct explanation of assertion.

(c)

Assertion is true but reason is false.

(d)

Both assertion and reason are false.

If ‘a’ stands for the edge length of the cubic system sc, bcc, and fcc. Then the ratio of radii of spheres in these systems will be respectively ________.

(a)

\(\left( \frac { 1 }{ 2 } a;\frac { \sqrt { 3 } }{ 2 } a;\frac { \sqrt { 2 } }{ 2 } a \right) \)

(b)

\(\left( \sqrt { 1a } :\sqrt { 3a } :\sqrt { 2a } \right) \)

(c)

\(\left( \frac { 1 }{ 2 } a:\frac { \sqrt { 3 } }{ 4 } a:\frac { 1 }{ 2\sqrt { 2 } } a \right) \)

(d)

\(\frac { 1 }{ 2 } a:\sqrt { 3 } a:\frac { 1 }{ \sqrt { 2 } } a\)

The mass of unit cell of Na₂O is ______.

(a)

Twice the formula mass of Na₂O

(b)

Four times the formula mass of Na₂O

(c)

Six times the formula mass of Na₂O

(d)

Thrice the formula mass of Na₂O

The number of cesium ion per unit cell in CsCI crystal system is________.

(a)

4

(b)

8

(c)

6

(d)

1

Structure of B₂O₃ is _____.

(a)

trigonal planar

(b)

tetrahedral

(c)

octahedral

(d)

cubic

Consider the following statements:
(i) increase in concentration of the reactant increases the rate of a zero order reaction.
(ii) rate constant k is equal to collision frequency A if E_a = 0
(iii) rate constant k is equal to collision frequency A if E_a = ∞
(iv) a plot of ln (k) vs T is a straight line.
(v) a plot of ln (k) vs \(\left( \frac { 1 }{ T } \right) \) is a straight line with a positive slope.
Correct statements are

(a)

(ii) only

(b)

(ii) and (iv)

(c)

(ii) and (v)

(d)

(i), (ii) and (v)

In a homogeneous reaction A⟶B+C+D, the initial pressure was P₀ and after time t it was P expression for rate constant in terms of P₀, P and t will be _____.

(a)

\(k=\left( \frac { 2.303 }{ t } \right) \log\left( \frac { 2{ P }_{ 0 } }{ { 3P }_{ 0 }-P } \right) \)

(b)

\(k=\left( \frac { 2.303 }{ t } \right) \log\left( \frac { { 2P }_{ 0 } }{ { P }_{ 0 }-P } \right) \)

(c)

\(k=\left( \frac { 2.303 }{ t } \right) \log\left( \frac { 3{ P }_{ 0 }-P }{ 2P_{ 0 } } \right) \)

(d)

\(k=\left( \frac { 2.303 }{ t } \right) \log\left( \frac { 2{ P }_{ 0 } }{ { 3P }_{ 0 }-2P } \right) \)

How much time will be taken for 20 gm to reduce 5 g? [R = 2 x 10^-3s^-1 (I order reaction)]

(a)

693.1 s

(b)

693.1 s^-1

(c)

6.931 s

(d)

6.931 s^-1

During a chemical reaction, the concentration of reaction  _____.

(a)

increases

(b)

decreases

(c)

remains constant

(d)

first increases and then decreases

Activation energy is equal to _______.

(a)

Threshold energy + Energy of colliding molecules

(b)

Threshold energy

(c)

Threshold energy x Energy of colliding molecules

(d)

Threshold energy - Energy of colliding molecules

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

Using Gibb’s free energy change, ∆G^o=57.34 kJ mol^-1, for the reaction, X₂Y_(s)⇌2X⁺+Y^2- (aq), calculate the solubility product of X₂Y in water at 300 K_______. (R = 8.3 J K^-1Mol^-1)

(a)

10^-10

(b)

10^-12

(c)

10^-14

(d)

can not be calculated from the given dat

An aqueous solution with pH value zero is _______.

(a)

acidic

(b)

basic

(c)

amphoteric

(d)

neutral

A drop of hydrochloric acid is added to pure water, its pH _____.

(a)

increases

(b)

decreases

(c)

increases and then decreases

(d)

resist the change in pH and so remains unaltered

The ionic product of water at 25°C is ________.

(a)

1 x 10^-7

(b)

1 x 10⁷

(c)

1 x 10^-14

(d)

1 x 10¹⁴

The molar conductivity of a 0.5 mol dm^-3 solution of AgNO₃ with electrolytic conductivity of 5.76 ×10⁻³ S cm⁻¹at 298 K is______.

(a)

2.88 S cm²mol^-1

(b)

11.52 S cm²mol^-1

(c)

0.086 S cm²mol^-1

(d)

28.8 S cm²mol ^-1

How many faradays of electricity are required for the following reaction to occur MnO₄^-→ Mn²⁺

(a)

5F

(b)

3F

(c)

1F

(d)

7F

Faraday's laws of electrolysis are related to ______.

(a)

atomic number of the cation

(b)

atomic number of the anion

(c)

equivalent weight of the electrolyte

(d)

speed of the cation

The specific conductance of a 0.01 M solution of KCI is 0.0014 ohm^-1 em^-1 at 25°C. Its equivalent conductance is ______.

(a)

14 ohm^-1 cm²eq^-1

(b)

140 ohm^-1 cm²eq^-1

(c)

1.4 ohm^-1 cm²eq^-1

(d)

0.14 ohm^-1 cm²eq^-1

When two half cells of Daniel cell is connected, a spontaneous ________ reaction takes place resulting in the flow of electrons from anode to cathode.

(a)

reduction

(b)

oxidation

(c)

redox

(d)

hydration

Adsorption of a gas on solid metal surface is spontaneous and exothermic, then ______.

(a)

ΔH increases

(b)

ΔS increases

(c)

ΔG increases

(d)

ΔS decreases

Match the following

a	Pure nitrogen	i	Chlorine
b	Haber process	ii	Sulphuric acid
c	Contact process	iii	Ammonia
d	Deacons Process	iv	Sodium azide (or) Barium azide

Which of the following is the correct option?

(a)

A	B	C	D
i	ii	iii	iv

(b)

A	B	C	D
ii	iv	i	iii

(c)

A	B	C	D
iii	iv	ii	i

(d)

A	B	C	D
iv	iii	ii	i

In case of physical adsorption, there is desorption when _______.

(a)

temperature increases

(b)

temperature decreases

(c)

pressure increases

(d)

concentration increases

The combination of the two layers of charges around the sol particle is called _______.

(a)

Brownian movement

(b)

Tyndall effect

(c)

Helmholtz double layer

(d)

None of these

The platinum catalyst used in the oxidation of SO₂ by contact process is poisoned by _______.

(a)

As₂O₃

(b)

V₂O₅

(c)

Fe₂O₃

(d)

CuCl₂

Assertion: Phenol is more reactive than benzene towards electrophilic substitution reaction
Reason: In the case of phenol, the intermediate arenium ion is more stabilized by resonance
Codes:
a) if both assertion and reason are true and reason is the correct explanation of assertion.
b) if both assertion and reason are true but reason is not the correct explanation of assertion.
c) assertion is true but reason is false
d) both assertion and reason are false.

(a)

if both assertion and reason are true and reason is the correct explanation of assertion.

(b)

if both assertion and reason are true but reason is not the correct explanation of assertion.

(c)

assertion is true but reason is false

(d)

both assertion and reason are false.

Which of the following compound can be used as antifreeze in automobile rediators?

(a)

methanol

(b)

ethanol

(c)

Neopentyl alcohol

(d)

ethan -1, 2-diol

Predict the structure of propane-1,2 diol ______.

(a)

CH₂ (OH) - CH₂CH₂OH

(b)

HOCH₂ - CH₂OH

(c)

CH₃CH (OH) CH₂OH

(d)

None of these

The number of secondary alcoholic group in glycerol is _______.

(a)

1

(b)

2

(c)

3

(d)

0

Among the following compounds strongest acid is _______.

(a)

HC≡CH

(b)

C₆H₆

(c)

C₂H₆

(d)

CH₃OH

Benzoic acid \(\overset { i){ NH }_{ 3 } }{ \underset { ii)\Delta }{ \longrightarrow } } A\overset { NaOBr }{ \longrightarrow } B\overset { NaN{ O }_{ 2 }/HCl }{ \longrightarrow } \) C 'C'  is ______.

(a)

anilinium chloride

(b)

O – nitro aniline

(c)

benzene diazonium chloride

(d)

m– nitro benzoic acid

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

(a)

Tollens reagent

(b)

Fehling’s solution

(c)

2,4 – dinitrophenyl hydrazine

(d)

semicarbazide

Reduction of ketone gives _______.

(a)

Primary alcohol

(b)

Secondary alcohol

(c)

Primary amide

(d)

Secondary amide

The test to distinguish HCOOH and CH₃COOH is/are ________.

(a)

Tollens reagent test

(b)

Litmus test

(c)

Sodium bicarbonate test

(d)

Both (b) and (c)

The decarboxylating agent is ___________.

(a)

soda lime

(b)

lime water

(c)

quick lime

(d)

lime of milk

What are the differences between minerals and ores?

Describe a method for refining nickel. (or) Explain the Mond process of refining nickel.

Name the two steps involved in the extraction of crude metal

Why is the froth flotation method selected for the concentration of sulphide ores?

Write a short note on anomalous properties of the first element of p-block.

What is catenation ? describe briefly the catenation property of carbon.

Name the building block of zeolites. Why zeolites have high porosity?

Which one is more soluble in diethyl ether, anhydrous Alcl₃ or hydrated Alcl₃? Explain in terms of bonding.

What is inert pair effect?

Explain why fluorine always exhibit an oxidation state of -1?

There is a huge difference between the melting and boiling points of oxygen and sulphur. Why?

Give reason for the following:
F₂ is more reactive than CIF₃ but CIF₃ is more reactive than Cl₂

What are transition metals? Give four examples.

Explain the oxidation states of 4d series elements.

Arrange the following in increasing order of acidic character?
CrO₃, CrO, Cr₂O₃

A poster suggests the following life style on the part of families / individuals.
(i) Which environmental values are promoted through these life style?
(ii) Suggest one additional life style action for promotion of green chemistry.
(iii) Give reason for the bleaching action of  KMnO₄

Write the IUPAC names for the following complexes.

Calculate the ratio of \(\frac { \left[ { Ag }^{ + } \right] }{ \left[ Ag\left( NH_{ 3 } \right) _{ 2 } \right] ^{ + } } \) in 0.2 M solution of NH_3. If the stability constant for the complex \([Ag(NH_{ 3 })_{ 2 }]^{ + }\) is 1.7 x 10⁷

What are stereoisomers?

Draw the Cis and trans isomer of MA₂B₂ type

Why do solids have a definite volume?

What is point defect in crystals?

Explain the rate determining step with an example.

The rate law for a reaction of A, B and C has been found to be rate = k[A]²[B][L]^3/2 How would the rate of reaction change when
(i) Concentration of [L] is quadrupled
(ii) Concentration of both [A] and [B] are doubled
(iii) Concentration of [A] is halved
(iv) Concentration of [A] is reduced to \(\left(\frac{1}{3}\right)\) and concentration of [L] is quadrupled.

Rate of chemical reaction is not uniform throughout. Justify you answer:

The reaction A + 2B ⟶ C obeys the rate equation. Rate = \(K{ \left[ A \right] }^{ \frac { 1 }{ 2 } }{ \left[ B \right] }^{ \frac { 3 }{ 2 } }\) What is the order of the reaction?

What are Lewis acids and bases? Give two example for each.

Calculate the pH of 0.04 M HNO₃ Solution.

What are the two types of buffer? Give an example for each.

Magnesium is not precipitated from a solution of its salt by a mixture of NH₄OH and NH₄Cl. Explain

Describe the electrolysis of molten NaCl using inert electrodes

State Faraday’s Laws of electrolysis

Explain the function of a salt bridge in an electrochemical cell.

Write the oxidation, reduction and overall redox reaction taking place in the Lithium ion battery.

What are promoters? Give an example.

Adsorption of a gas on the surface of solid is generally accompanied by decrease in entropy. Still it is a spontaneous process. Explain.

What happens when ethylene reacts with alkaline KMnO₄ solution?

Which of the following does not give iodoform reaction?

Write short note on Kolbe's electrolytic reaction.

Give any three uses of benzoic acid.

Using the Ellingham diagram,
(A) Predict the conditions under which
(i) Aluminium might be expected to reduce magnesia.
(ii) Magnesium could reduce alumina.
(B) it is possible to reduce Fe₂O₃ by coke at a temperature around 1200K

How oxides of metals are reduced by hydrogen?

AlCl₃ behaves like a lewis acid. Substantiate this statement.

What happens to boranes at high temperatures?

Give a reason to support that sulphuric acid is a dehydrating agent.

Explain the commercial method of preparation of nitric acid.

What are interstitial compounds?

Write chemical equations for the reactions involved in the manufacture of potassium permanganate from pyrolusite ore.

Classify the following ligands based on the number of donor atoms.
a) NH₃
b) en
c) ox^2-
d) pyridine

Aqueous copper sulphate solution (blue) gives
(i) a green precipitate with aqueous potassium fluoride.
(ii) a bright green solution with aqueous potassium chloride. Explain these experimental results.

State Bragg's law.

A gas phase reaction has energy of activation 200 kJ mol^-1. If the frequency factor of the reaction is 1.6 x 10¹³s^-1. Calculate the rate constant at 600 K.(e^-40.09 = 3.8 x 10^-48)

What is the effect of temperature on the rate constant of a reaction? How can this temperature effect on rate constant be represented quantitatively?

Define pH.

What do you mean by buffer action?

The conductivity of a 0.01M solution of a 1 :1 weak electrolyte at 298K is 1.5\(\times\)10^-4 S cm⁻¹.
i) molar conductivity of the solution
ii) degree of dissociation and the dissociation constant of the weak electrolyte
Given that
\(\lambda^{0}_{cation}=248.2 \ S\) cm² mol^-1
\(\lambda^{0}_{anlon}=51.8 \ S\) cm² mol^-1

Write the cell representation of the galvanic cell in which the following reaction take place
\({ Zn }_{ (s) }+Cu{ SO }_{ 4 }\rightarrow { ZnSO }_{ 4 }+{ Cu }_{ (s) }\)
For the above cell. Identify the anode and cathode half cell.

What are enzymes? Write a brief note on the mechanism of enzyme catalysis.

Name various techniques by which a colloid can be deemulsified.

Write the mechanism of acid catalysed dehydration of ethanol to give ethene.

How do primary, secondary and tertiary alcohols differ in terms of their oxidation?

What is acidity constant? How is it expressed.

List the applications of iron.

How are silicates classified? Give an example for each type of silicate.

Explain the oxidising property of sulphuric acid.

Justify the following statement.
"Elements of the first transition series possess many properties different from those of heavier transition elements".

What are the postulates of valance bond theory? Give its limitations.

An element with molar mass 2.7 x 10^-2 kg mol forms a cubic unit cell with edge length 405 pm. If its density is 2.7 x 10³ kg m^-3, What is the nature of the cubic unit cell?

A first order reaction completes 25% of the reaction in 100 mins. What are the rate constant and half life values of the reaction?

Calculate the pH of 0.02 MHCl.

The emf values of the cell reactions Fe³⁺+ e^- ⇾ Fe²⁺ and Ce²⁺ ⇾ Ce³⁺ e^- are 0.61 V and -0.85 V respectively. Construct the cell such that the free energy of the cell is negative. Calculate the emf of the cell.

Write any five applications of colloids in day - to day life.

What is major product formed when 3,3-dimethyl-2-butanol is heated in the presence of H₂SO₄.

An organic compound (A) C₂H₃OCI on treatment with Pd and BaSO₄ gives (B) C₂H₄O which answers iodoform test. (B) when treated with cone.H₂SO₄ undergoes polymerisation to give (C) a cyclic compound. Identify (A), (B) and (C) and explain the reactions.