Two electrons occupying the same orbital are distinguished by ___________

(a)

azimuthal quantum number

(b)

spin quantum number

(c)

magnetic quantum number

(d)

 orbital quantum number

Halogens belong to the _____________

(a)

s-block

(b)

p-block

(c)

d-block

(d)

Zero group of the periodic table

In the modern periodic table, the period indicates the value of____

(a)

atomic number

(b)

mass number

(c)

principal quantum number

(d)

azimuthal quantum number

Various successive ionisation enthalpies (in kJ mol^-1) of an element are given below.

IE1	IE2	IE3	IE4	IE5
577.5	1,810	2,750	11,580	14,820

The element is

(a)

phosphorus

(b)

Sodium

(c)

Aluminium

(d)

Silicon

In which of the following reactions H₂O₂ act as a reducing agent?
(i) H₂O₂ + 2H⁺ + 2e \(\rightarrow\) 2H₂O
(ii) H₂O₂ - 2e \(\rightarrow\) O₂ + 2H⁺
(iii) H₂O₂ + 2e \(\rightarrow\) 2OH^-
(iv) H₂O₂ + 2OH^- - 2e \(\rightarrow\) O₂ + 2H₂O

(a)

(ii) and (iv)

(b)

(i) and (ii)

(c)

(iii) and (iv)

(d)

(i) and (iii)

In case of alkali metal halides, the ionic character increases in the order ____________

(a)

MF < MCI < MBr < MI

(b)

MI < MBr < MCI < MF

(c)

MI < MBr

(d)

none of these

__________ is a group 2 element which shows diagonal relationship with aluminium

(a)

Be

(b)

Mg

(c)

Ca

(d)

Ba

The colour produced by potassium when burnt in Bunsen flame is ________

(a)

red

(b)

blue

(c)

green

(d)

lilac

Four gases P, Q, R and S have almost same values of 'b' but their 'a' values (a, b are Vander Waals Constants) are in the order Q < R < S < P. At a particular temperature, among the four gases the most easily liquefiable one is __________

(a)

P

(b)

Q

(c)

R

(d)

S

The unit of pressure is _____________

(a)

Pascal

(b)

Torr

(c)

Bar

(d)

all the above

Which of the following is a diatomic gas in nature?

(a)

Oxygen

(b)

Ozone

(c)

Helium

(d)

Radon

ΔG⁰ of reversible reaction at its equilibrium is ____________

(a)

Positive

(b)

Negative

(c)

Always zero

(d)

Both (a) & (b)

When a liquid boils, there is ___________

(a)

increase in entropy

(b)

a decrease in entropy

(c)

increase in heat of vaporization

(d)

an increase in free energy

Which of the following is a state function?

(a)

q

(b)

\(\Delta\)q

(c)

w

(d)

\(\Delta\)S

Which one of the following is equal to 1 Joule?

(a)

Nm^-1

(b)

Nm^-2

(c)

Nm

(d)

kg ms^-2

Match the List-I and List-II using the correct code given below the list.

List-I	List-II
A. Cyclic process	1. ΔU=q-PΔV
B. Adiabatic process	2. ΔU=qv
C. Isobaric process	3. q=-w
D. Isochoric process	4. ΔU=w

(a)

A	B	C	D
4	2	3	1

(b)

A	B	C	D
3	4	1	2

(c)

A	B	C	D
2	1	4	3

(d)

A	B	C	D
1	3	2	4

The heat of neutralization of a strong acid and strong base is around _____

(a)

+57.32 kJ

(b)

-57.32 kJ

(c)

-3227 kJ mol^-1

(d)

+3227 kJ mol^-1

Mathematically, the third law of thermodynamics is expressed as _______

(a)

\(\overset{\lim}{T\rightarrow 0}{ S=0 } \)

(b)

\(\overset{\lim}{T\rightarrow \infty} {S=1 } \).

(c)

ΔU = q + w

(d)

G = H - TS

Hydrogen (a moles) and iodine (b moles) react to give 2x moles of the HI at equilibrium. The total number of moles at equilibrium is _____________

(a)

a + b + 2x

(b)

(a - b) + (6  - 2x)

(c)

(a + b)

(d)

a + b - x

Two moles of N₂ and two moles of H₂ are taken in a closed vessel of 5 litre capacity and suitable conditions are provided for the reaction. When the equilibrium is reached, it is found that a half mole of N₂ is used up. The equilibrium concentration of NH₃ is

(a)

0.2

(b)

0.4

(c)

0.3.

(d)

0.1

If K_l is the equilibrium constant at temperature T₁ and is the equilibrium constant at temperature T₂ and if T₂ > T₁and reaction is endothermic then ___________

(a)

K₂>K₁

(b)

K₂1

(c)

K₂=K₁

(d)

All of these

Equilibrium constant Kp for following reaction
\(MgCO_{ 3\left( s \right) }\rightleftharpoons Mg{ O }_{ \left( s \right) }+{ CO }_{ 2\left( g \right) }\)

(a)

K_p = P_co2

(b)

\({ K }_{ p }=\cfrac { { p }_{ { CO }_{ 2 } }\times { p }_{ CO_{ 2 } }\times { p }_{ Mgo } }{ { P }_{ MrCO } } \)

(c)

\({ K }_{ p }=\cfrac { { P }_{ MG }{ CO }_{ 3 } }{ { P }_{ CO\bullet }p_{ mgO } } \)

(d)

\({ K }_{ p }=\cfrac { { P }_{ MG }{ CO }_{ 3 } }{ { P }_{ CO\bullet }p_{ mgO } } \)

Which of the following is an example of homogeneous equilibrium?

(a)

H₂O(l) ⇌ H₂O(g)

(b)

CaCO₃(s) ⇌ CaO(s) + CO(g)

(c)

H₂(g) + I₂(g) ⇌ 2HI(g)

(d)

2CO(g) ⇌ CO₂(g) + C(s)

Consider the following equilibrium reaction and relate their equilibrium constants ________.
(i) N₂ + O₂ ⇌ 2NO; K₁
(ii) 2NO + O₂ ⇌ 2NO₂; K₂
(iii) N₂ + 2O₂ ⇌ 2NO₂; K₃

(a)

K₃xK₂ = K₁

(b)

K₁xK₃ = K₂

(c)

K₁xK₂ = K₃

(d)

\(\frac{K_1}{K_2}=K_3\)

Statement I. In Haber's process, NH₃ is liquefied and removed.
Statement II. In manufacture of NH₃, liquefied and removal of NH₃, keeps the reaction moving in forward direction.

(a)

Statement I and II are correct and II is the correct explanation of I.

(b)

Statement I and II are correct but II is not the correct explanation of I.

(c)

Statement I is wrong but statement II is correct.

(d)

Statement I is correct but statement II is wrong.