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self evaluation test on chemical equilibrium with answers., Exercises of Chemistry

14 multiple-choice questions related to chemical equilibrium, including equations and calculations. The questions cover topics such as equilibrium constants, reaction quotients, and active mass. The questions are suitable for advanced high school or undergraduate students studying chemistry.

Typology: Exercises

2021/2022

Available from 05/24/2022

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338 Chemical Equilibrium
1. One mole of
3
SO
was placed in a litre reaction vessel at a
certain temperature. The following equilibrium was established
3
2SO
22
2OSO
At equilibrium 0.6 moles of
2
SO
were formed. The
equilibrium constant of the reaction will be [MP PMT 1991]
(a) 0.36 (b) 0.45
(c) 0.54 (d) 0.675
2. For the following homogeneous gas reaction
23 54 ONH
OHNO 2
64
, the equilibrium constant
c
K
has the
dimension of [CPMT 1990; MP PET/PMT 1998 ]
(a)
(b)
1
Conc
(c)
1
Conc
(d) It is dimensionless
3. Consider the imaginary equilibrium
4A + 5B 4X + 6Y
The equilibrium constant
c
K
has the unit [RPMT 2000]
(a) Mole2 litre-2 (b) Litre mole-1
(c) Mole litre-1 (d) Litre2 mole-2
4. For the reaction
)(2)( 2gHgCO
)(
3gOHCH
, true
condition is
(a)
cp KK
(b)
cp KK
(c)
cp KK
(d)
0
c
K
but
0
p
K
5. For the reaction
)(
2
1
)( 2gOgCO
)(
2gCO
;
c
p
K
K
is
equivalent to [M P PET/PMT 1998; AIEEE 2002]
(a) 1 (b)
RT
(c)
RT
1
(d)
2/1
)(RT
6.
)( 2
)( 2
)( 52 42 ggg
ONOON
what is the ratio of the rate of
decomposition of
52ON
to rate of formation of
2
NO
[DCE 2003]
(a)
2:1
(b)
1:2
(c)
4:1
(d)
1:4
7. The reaction quotient (Q) for the reaction
)(2 g
N
)(2
3g
H
)(3
2g
NH
is given by
3
22
2
3]][[
][
HN
NH
Q
. The reaction will proceed from
right to left is [CBSE PMT 2003]
(a) Q = 0 (b) Q =
c
K
(c) Q <
c
K
(d) Q >
c
K
Where
c
K
is the equilibrium constant
8. In the thermal dissociation of
5
PCl
, the partial pressure in the
gaseous equilibrium mixture is 1.0 atmosphere when half of
5
PCl
is found to dissociate. The equilibrium constant of the
reaction
)( p
K
in atmosphere is [JIPMER 2002]
(a) 0.25 (b) 0.50
(c) 1.00 (d) 0.3
9.
HI
was heated in a closed tube at
C
o
440
till equilibrium is
obtained. At this temperature 22% of
HI
was dissociated. The
equilibrium constant for this dissociation will be
[MP PET 1988, 92; MNR 1987 ; UPSEAT 2000]
(a) 0.282 (b) 0.0796
(c) 0.0199 (d) 1.99
10. The following equilibrium exists in aqueous solution
COOHCH3
HCOOCH 3
. If dilute
HCl
is added
without a change in temperature, then the [MNR 1987]
(a) Concentration of
COOCH 3
will increase
(b) Concentration of
COOCH 3
will decrease
(c) Equilibrium constant will increase
(d) Equilibrium constant will decrease
11. Which of the following is not favourable for
3
SO
formation
)()(2 22 gOgSO
kcalHgSO 0.45);(2 3
[IIT 1984; MP PET 1997]
(a) High pressure
(b) High temperature
(c) Decreasing
3
SO
concentration
(d) Increasing reactant concentration
12.
gm120
of urea are present in
litre5
solution, the active mass
of urea is [MP PMT 1994]
(a) 0.2 (b) 0.06
(c) 0.4 (d) 0.08
13. For the system
)()(2 gBgA
)(3 gC
, the expression for
equilibrium constant K is [NCERT 1973; DCE 1999]
(a)
]3[
][]2[
C
BA
(b)
3
2
][
][][
C
BA
(c)
][]2[
]3[
BA
C
(d)
][][
][
2
3
BA
C
14. If concentration of reactants is increased by
''x
, then
K
becomes [AFMC 1997]
(a) ln (
xK/
) (b)
xK/
(c)
xK
(d)
K
(SET -8)
pf2

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338 Chemical Equilibrium

1. One mole of SO 3 was placed in a litre reaction vessel at a

certain temperature. The following equilibrium was established

2 SO 3 ⇌ 2 SO (^) 2  O 2

At equilibrium 0.6 moles of (^) SO 2 were formed. The

equilibrium constant of the reaction will be [MP PMT 1991]

(a) 0.36 (b) 0.

(c) 0.54 (d) 0.

2. For the following homogeneous gas reaction 4 NH (^) 3  5 O 2 ⇌

4 NO  6 H 2 O^ ,^ the^ equilibrium^ constant^ Kc has^ the

dimension of [CPMT 1990; MP PET/PMT 1998]

(a)

 10 Conc (b)

 1 Conc

(c)

 1 Conc (d) It is dimensionless

3. Consider the imaginary equilibrium

4 A + 5 B ⇌ 4 X + 6 Y

The equilibrium constant Kc has the unit [RPMT 2000]

(a) Mole^2 litre -^2 (b) Litre mole-^1

(c) Mole litre -^1 (d) Litre^2 mole-^2

4. For the reaction CO ( g ) 2 H 2 ( g ) ⇌ CH 3 OH ( g ), true

condition is

(a) K (^) pKc (b) K (^) pKc

(c) K (^) pKc (d) (^) Kc  0 but Kp  0

5. For the reaction () 2

1 CO ( g ) O 2 gCO 2 ( g ); c

p

K

K is

equivalent to [MP PET/PMT 1998; AIEEE 2002]

(a) 1 (b) RT

(c) RT

(d) ( RT )^1 /^2

( )

2 ( )

2 ( )

g g g

N ONOO what is the ratio of the rate of

decomposition of N 2 O 5 to rate of formation of NO 2

[DCE 2003]

(a) 1 : 2 (b) 2 : 1

(c) 1 : 4 (d) 4 : 1

7. The reaction quotient ( Q ) for the reaction

N 2 ( g ) 3 H 2 ( g ) ⇌ 2 NH 3 ( g )

is given by 3 2 2

2 3 [ ][ ]

[ ]

N H

NH

Q . The reaction will proceed from

right to left is [CBSE PMT 2003]

(a) Q = 0 (b) Q = Kc

(c) Q < Kc (d) Q > Kc

Where Kc is the equilibrium constant

8. In the thermal dissociation of PCl 5 , the partial pressure in the

gaseous equilibrium mixture is 1.0 atmosphere when half of

PCl 5 is found to dissociate. The equilibrium constant of the

reaction ( Kp )in atmosphere is [JIPMER 2002]

(a) 0.25 (b) 0.

(c) 1.00 (d) 0.

9. HI was heated in a closed tube at C

o 440 till equilibrium is

obtained. At this temperature 22% of (^) HI was dissociated. The

equilibrium constant for this dissociation will be

[MP PET 1988, 92; MNR 1987; UPSEAT 2000]

(a) 0.282 (b) 0.

(c) 0.0199 (d) 1.

10. The following equilibrium exists in aqueous solution

CH 3 COOHCH COO ^  H

  1. If dilute HCl is added

without a change in temperature, then the [MNR 1987]

(a) Concentration of

CH (^) 3 COO will increase

(b) Concentration of

CH (^) 3 COO will decrease

(c) Equilibrium constant will increase

(d) Equilibrium constant will decrease

11. Which of the following is not favourable for SO 3 formation

2 SO (^) 2 ( g ) O 2 ( g ) ⇌ 2 SO (^) 3 ( g ); H  45. 0 kcal

[IIT 1984; MP PET 1997]

(a) High pressure

(b) High temperature

(c) Decreasing SO 3 concentration

(d) Increasing reactant concentration

12. 120 gm of urea are present in 5 litre solution, the active mass

of urea is [MP PMT 1994]

(a) 0.2 (b) 0.

(c) 0.4 (d) 0.

13. For the system 2 A ( g ) B ( g )⇌ 3 C ( g ), the expression for

equilibrium constant K is [NCERT 1973; DCE 1999]

(a) [ 3 ]

[ 2 ] []

C

A  B

(b) 3

2

[ ]

[] []

C

A  B

(c) [ 2 ] []

[ 3 ]

A B

C

(d) [] []

[ ]

2

3

A B

C

14. If concentration of reactants is increased by ' x ', then K becomes [AFMC 1997]

(a) ln ( K / x ) (b) K / x

(c) Kx (d) K

(SET - 8)

Chemical Equilibrium 339

1. (d) ( 10. 6 )

SO ⇌

( 0. 3 )

2 ( 0. 6 )

2 SO 2  O

[ ]

[ ][ ]

3

2

2 (^2)  

SO

SO O

Kc.

2. (b) K has the units of (^) (conc. ) n , where n  10  9  1 3. (c) Unit of (^) Kc (unit of concentration)n

= ( mole litre –^1 )n

n = 10 – 9 = 1

Kcmol Litre –^1.

4. (c) When nrnp then K (^) pKc

where nr = no. of moles of reactant

np = no. of moles of product.

5. (c) For 2 2

CO  O ⇌ CO 2

2

111 ( )

K (^) pKcRT^2

1

( )

  KcRT^ ; K RT

K

c

p^1 

6. (b) 2 N 2 O 5  HNO 2  O 2

Rate of decomposition of N 2 O 5

dt

K [ NO ] . 2

(^1 )  

Rate of formation of dt

dNO NO

[ ] . 4

(^1 ) 2 

 Ratio = 2 : 1

7. (d) If QKc reaction will proceed right to left to decrease

concentration of product.

8. (d) PCl 5 ⇌ PCl 3 (^)  Cl 2

Initial conc. 1 0 0

At equilibrium 0.5 0.5 0.

  1. 3 3

1

  1. 75

  2. 5 0. 5

[ 1 ( 0. 5 )]

1 0. 5 0. 5

( 1 )

2 2

2  

  

   

x

Px Kp

9. (c) 2 HIH 2 (^)  I 2

Initial conc. 2 moles 0 0

at equilibrium 2 100

[ 1. 56 ]

[ ]

[ ][ ]

2 2

2 2 

HI

H I

K^.

10. (b) When adding HCl in CH 3 COOH solution the

concentration of H  is increased. So reaction is proceed

in reverse direction and the concentration of

CH (^) 3 COO

is decreased.

11. (b) The reaction is exothermic so high temperature will favour backward reaction. 12. (c) Active mass litre

moles

in

wt.in /molecularwt.     V litre

gm

13. (d) [ ][]

[]

2

3

A B

C

K .

14. (d) There is no effect of change in concentration on equilibrium constant.