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IIT JAM Chemistry - MCQ Test 4

60 Questions MCQ Test MOCK Test Series for IIT JAM Chemistry | IIT JAM Chemistry - MCQ Test 4

Description

This mock test of IIT JAM Chemistry - MCQ Test 4 for Chemistry helps you for every Chemistry entrance exam. This contains 60 Multiple Choice Questions for Chemistry IIT JAM Chemistry - MCQ Test 4 (mcq) to study with solutions a complete question bank. The solved questions answers in this IIT JAM Chemistry - MCQ Test 4 quiz give you a good mix of easy questions and tough questions. Chemistry students definitely take this IIT JAM Chemistry - MCQ Test 4 exercise for a better result in the exam. You can find other IIT JAM Chemistry - MCQ Test 4 extra questions, long questions & short questions for Chemistry on EduRev as well by searching above.

QUESTION: 1

Relative lowering of vapor pressure produced by dissolving 71.5g of a substance in 1Kg of water is 0.0073. Molecular weight of substance will be

A.
18
B.
342
C.
60
D.
180

Solution:

QUESTION: 2

Which solution will show maximum vapor pressure at 300K

A.
1M Sucrose
B.
1M Acetic acid
C.
1M Calcium Chloride
D.
1M Sodium Chloride

Solution:

QUESTION: 3

The relationship been Osmotic pressure at 273K when 10g Glucose (P1), 10g Urea (P2), 10g Sucrose (P3) are dissolved in 250 Ml of water

A.
P1>P2>P3
B.
P3>P1>P2
C.
P2>P1>P3
D.
P2>P3>P1

Solution:

QUESTION: 4

Solution A contains 7g/L of MgCl2 and Solution B contains 7g/L of NaCl. At room temp, Osmotic pressure of

A.
A>B
B.
A=B
C.
B>A
D.
Insufficient information

Solution:

QUESTION: 5

When a substance is dissolved in solvent, its vapor pressure is decreased. It brings

A.
Decrease in B.pt
B.
Increase in B.pt
C.
Increase in Fz.pt
D.
Decrease in Fz.pt

Solution:

When a solute dissolves in water, the vapour pressure of solvent decreases and because of this boiling point increases and freezing point decreases.

QUESTION: 6

At a given temperature, total vapor pressure in Torr of a mixture of volatile components A and B is given by

p = 120 – 75X_B

Hence, vapor pressure of pure A and B respectively (in Torr) are:

A.
120, 75
B.
120, 195
C.
120, 45
D.
75, 45

Solution:

QUESTION: 7

The equilibrium constant is 6.0 × 10^–4 for the N₂O₂→ 2NO reaction. If the concentration of nitrogen is 0.10 mol/L and concentration of oxygen is 0.20 mol/L at equilibrium. Then the concentration of nitric oxide at equilibrium is:

A.
10.9 × 10^–3 mol/L
B.
1.09 × 10^–3 mol/L
C.
10.9 × 10^–5 mol/L
D.
1.09 × 10^–5 mol/L

Solution:

QUESTION: 8

Some solid NH₄HS is placed in a flask containing 0.5 atm of NH₃, what would be pressure of NH₃ and H₂S when equilibrium is reached:

NH₄HS_(g)→ NH_3(g) + H₂S_(g), K_P = 0.11

A.
6.65 atm
B.
0.665 atm
C.
0.0665 atm
D.
66.5 atm

Solution:

QUESTION: 9

Ratio of sigma and pi bonds is maximum in

A.
Napthalene
B.
Tetracyano methane
C.
Enolic form of Urea
D.
Equal

Solution:

QUESTION: 10

For the following three reactions (I), (II) and (III) equilibrium constants are given

(I) CO_(g) + H₂O_(g)→ CO_2(g) + H_2(g); K₁
(II) CH_4(g) + H₂O_(g)→ CO_(g) + 3H_2(g); K₂
(III) CH_4(g) + 2H₂O_(g)→ CO_2(g) + 4H_2(g); K₃

Which of the following relations is correct:

A.
K₂K₃ = K₁
B.
K₃ = K₁K₂
C.
D.

Solution:

QUESTION: 11

XY₂ dissociates as XY_2→ XY_(g) + Y_(g) when the initial pressure of XY₂ is 600 mmHg, the total equilibrium pressure is 800mm Hg. Calculate K for the reaction assuming that the volume of the system remain unchanged:

A.
50
B.
100.0
C.
166.6
D.
400.0

Solution:

QUESTION: 12

A 50 mL sample of 0.01M Ba(OH)2 is titrated with 0.01 M HCl. The solution at equivalent point is

A.
3.33 × 10^-3M BaCl₂
B.
5 × 10^-3M BaCl₂
C.
2.5 × 10^-3M BaCl₂
D.
1.00 × 10^-2M BaCl₂

Solution:

QUESTION: 13

Which of the following fluorides is angular:

A.
BeF₂
B.
ZnF₂
C.
SnF₂
D.
XeF₂

Solution:

QUESTION: 14

Based on the following information,

Which of the following chemical species is the strongest reducing agent?

A.
F–(aq)
B.
Mg+(aq)
C.
F2(g)
D.
Mg(s)

Solution:

QUESTION: 15

Which molecule has zero bond order:

A.
H₂⁺
B.
H₂
C.
HeH
D.
He₂

Solution:

QUESTION: 16

Which of the following processes involves increasing in bond order:

A.
N₂ → N₂⁺ +e^–
B.
CO + e^– → CO^–
C.
NO → NO⁺ + e^–
D.
O₂ + e^– → O₂^–

Solution:

QUESTION: 17

At room temperature, HCl is a gas while HF is a liquid because:

A.
Of a strong bond between H and F in HF
B.
HF is less acidic as compared to HCl
C.
Of strong intermolecular H–bonding in HF
D.
HCl is less acidic as compared to HF

Solution:

QUESTION: 18

The bond order and bond type in the C₂ molecule are, respectively:

A.
2; one sigma bond and one pi bond
B.
3; one sigma bond and two pi bond
C.
2; two pi bonds
D.
2; two sigma bonds

Solution:

QUESTION: 19

The major product formed in the following reacting is

Solution:

QUESTION: 20

Predict the condition A and the structure of the major product B in the following sequence.

Solution:

QUESTION: 21

The major product B is:

Solution:

QUESTION: 22

The major product P is:

Solution:

QUESTION: 23

The conditions A-B, required for the following pericyclic are

A.
A = ∆ ; B = ∆
B.
A = hν; B = ∆
C.
A = hν; B = hν
D.
A = ∆ ; B = hν∆

Solution:

QUESTION: 24

The major product P is:

Solution:

QUESTION: 25

Solubility of BaSO₄ in aqueous solution is 1 × 10^–5 M. Hence, solubility in 0.1 M BaCl₂ is:

A.
1 × 10^–10 M
B.
1 × 10^–9 M
C.
1 × 10^–4 M
D.
1 × 10^–5 M

Solution:

BaSO₄ ---------> Ba²⁺ + SO₄²⁻
According to ICE table
BaSO₄ -----------------> Ba²⁺ + SO₄²⁻
I 0.1 M 0
C +s +s
E s + 0.1 s
therefore we can write
ksp = ( s + 0.01) . s
as the value of ksp is very small as compared to silver ions initial concentration
we can use approximation
s + 0.1 ≈ 0.1
Ksp = 0.01 . s
s = 1 X 10⁻⁵ / 0.1
s = 0.0001 mol/ L
s = 1 X 10^⁻4 mol/ L

QUESTION: 26

pH of a mixture of 1 M benzoic acid (pKa = 4.20) and 1 M sodium benzoate is 4.5. In 300 mL buffer, benzoic acid is:

A.
200 mL
B.
150 mL
C.
100 mL
D.
50 mL

Solution:

QUESTION: 27

58.5 g of NaCl and 180g of glucose were separately dissolved in 1L of water. Identify the correct statements regarding the elevation in boiling point of solution.

A.
NaCl solution will have higher boiling point
B.
Glucosesolution will have higher boiling point
C.
Both solutionwill have equal boiling point
D.
No elevation will be observed

Solution:

QUESTION: 28

Elevation in boiling point of solution of 13.44g og CuCl₂ in 1 Kg of water will be (M.wt = 134.4, Kb =0.52Kmolal^-1, assume it is a strong electrolyte)

A.
0.16
B.
0.05
C.
0.1
D.
0.2

Solution:

QUESTION: 29

At 700 K, the equilibrium constant K_p, for the reaction 2 SO₃ (g) ⇌ 2 SO₂ (g) + O₂ Is 1.8 X 10^-3 kPa. What is the numerical value in moles per liter of K_c for the reaction at the same temperature?

A.
3.09 × 10^-7
B.
5.07 × 10^-8
C.
8.18 × 10^-9
D.
9.24 × 10^-10

Solution:

QUESTION: 30

0.1 mol of N₂O₄(g) was sealed in a tube under 1 atmospheric pressure at 25^oC. Calculate the no of mole of NO₂(g) present if equilibrium is reached after sometime (Kp = 0.14)

A.
1.8 × 10²
B.
2.8 × 10²
C.
0.034
D.
2.8 × 10^-2

Solution:

*Multiple options can be correct

QUESTION: 31

The compound pair which shows correct order of angle:

(I) NH₃> PH₃, (II) H₂S < H₂O, (III) NO₂⁺ >NO₂ (IV)

A.
I
B.
II
C.
III
D.
IV

Solution:

*Multiple options can be correct

QUESTION: 32

The correct statement among the following is:

A.
N₂ has higher bond order than N₂⁺ and hence has larger bond length compared to N₂⁺
B.
N₂⁺ has higher bond order than N₂ and hence has larger bond length compared to N₂
C.
N₂ has higher bond order than N₂⁺ and hence has higher dissociation energy compared to N₂⁺
D.
N₂ has lower bond order than N₂⁺ and hence has lower dissociation energy compared to N₂⁺ energy.

Solution:

*Multiple options can be correct

QUESTION: 33

Which of the following solutions are isotonic (R = 0.0821 atmK^-1mol^-1)

A.
0.01 M glucose
B.
0.01 M NaNO₃
C.
500 mL solution containing 0.3g Urea
D.
0.04 N HCl

Solution:

*Multiple options can be correct

QUESTION: 34

Some or more species give belowhave pH less than 7.

A.
10^-8 M HCl
B.
10^-8 M NaOH
C.
10 mL of 10^-6 M HCl diluted to 100 mL
D.
10 mL of 0.01 M CH₃COOH at the end point after addition of 10 mL 0.01 M NaOH

Solution:

The pH of 10^-8M HCl solution is 6.98
The pH of NaoH solution will be 8
The pH of 10 mL of 10^-6 M HCl diluted to 100 mL is 6.99

*Multiple options can be correct

QUESTION: 35

For the chemical equilibrium, CaCO₃(s) → CaO(s) + CO₂(g), DH°_r can be determined from which one of the following plots:

Solution:

*Multiple options can be correct

QUESTION: 36

In I₃^–

A.
I₂ is Lewis Acid and I^– is Lewis Base
B.
I₂ is Lewis Base and I^– is Lewis Acid
C.
I₃^– behaves as amphoteric anion
D.
I₃^– does not exist

Solution:

*Multiple options can be correct

QUESTION: 37

Which of the following molecule is expected to exhibit diamagnetic behavior ?

A.
B₂
B.
N₂
C.
O₂
D.
S₂

Solution:

*Multiple options can be correct

QUESTION: 38

Select correct statements:

A.
A solute will dissolve in water if hydration is greater than lattice energy
B.
If anion is large as compared to the cation, the lattice energy will remain almost constant.
C.
Solubiltiy of IIA hydroxide is in order Be > Mg > Ca > Sr
D.
AgF is water soluble

Solution:

*Multiple options can be correct

QUESTION: 39

Which have a linear structure

A.
BeF₂
B.
Ag[CN]₂^–
C.
CO₂
D.
XeF₂

Solution:

*Multiple options can be correct

QUESTION: 40

According to Le-Chatelier’s principle, the equilibrium constant of a reversible reaction will not shift by:

A.
Increasing the temperature of an exothermic reaction.
B.
Increasing the temperature of an endothermic reaction.
C.
Changing the concentrations of the reactants
D.
The effect of a catalyst.

Solution: