Jee 2014 Booklet3 Hwt Chemical Equilibrium

August 28, 2017 | Author: varunkohliin | Category: Chemical Equilibrium, Chemical Reactions, Ammonia, Chemistry, Dissociation (Chemistry)
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Jee 2014 Booklet3 Hwt Chemical Equilibrium...

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Vidyamandir Classes

DATE :

  MARKS :    10 

IITJEE :

NAME :

TIME : 25 MINUTES

TEST CODE : CM-EQ [1]

ROLL NO.

START TIME :

END TIME :

STUDENT’S SIGNATURE :

TIME TAKEN:

PARENT’S SIGNATURE :

 This test contains a total of 10 Objective Type Questions.  Each question carries 1 mark. There is NO NEGATIVE marking. Choose the correct alternative. Only one choice is correct. 1.

A vessel at 1000 K contains CO2 with a pressure of 0.5 atm. Some of the CO2 is converted into CO on the addition of graphite. If the total pressure at equilibrium is 0.8 atm, the value of Kp is : (A) 1.8 atm (B) 3 atm (C) 0.3 atm (D) 0.18 atm

2.

Four moles of PCl5 are heated in a closed 4 dm3 container to reach equilibrium at 400 K. At equilibrium 50% of PCl5 is dissociated. What is the value of Kc for the dissociation of PCl5 into PCl3 and Cl2 at 400 K? (A) 0.50 (B) 1.00 (C) 1.15 (D) 0.05 (E) 0.25

3.

Consider the following gaseous equilibria with equilibrium constant K1 and K2 respectively. SO 2  g  

1  SO3  g  ; O 2  g   2

 2SO 2  g   O 2  g  2SO3  g  

The equilibrium constant are related as : (A) 4.

2K1  K 22

(B)

K12 

1 K2

(C)

K 22 

1 K1

(D)

K2 

2 K12

  For the reaction N 2 O4 (g)   2NO2 (g) the relation connecting the degree of dissociation ( ) of N 2 O4 (g) with the equilibrium constant Kp is : (A)

5.

4  Kp / p

(B)



Kp 4  Kp

1/ 2

(C)

 Kp / p     4  Kp / p   

(D)

 Kp   4  Kp 

1/ 2

   

  In the system AB(s)   A(g)  B(g) doubling the equilibrium concentration of A will cause the equilibrium concentration of B to : (A) (C)

6.



Kp / p

change to two times its original value remain constant

(B) (D)

change to one-half its original value change to a new value which cannot be predicted

 NH3  g   H 2S  g  NH 4HS  s   In the above reaction, if the pressure at equilibrium and at 300 K is 100 atm then what will be the equilibrium constant K p? (A) 2500 atm2 (B) 50 atm2 (C) 100 atm2 (D) 200 atm2

7.

3 moles of A and 4 moles of B are mixed together and allowed to come into equilibrium according to the following reaction.

 2C  g   3D  g  3A  g   4B  g   When equilibrium is reached, there is 1 mole of C. The equilibrium constant of the reaction is : (A)

8.

1 4

(B)

1 3

(C)

1 2

Which of the following is a wrong statement about equilibrium state ? (A) Rate of forward reaction = Rate of backward reaction (B) (C) Catalysts increase value of equilibrium constant (D)

VMC/Chemical Equilibrium

1

(D)

1

Equilibrium is dynamic Free energy change is zero

HWT/Chemistry

Vidyamandir Classes 9.

 C  D A  B  Initially moles of A and B are equal. At equilibrium, moles of C are three times of A. The equilibrium constant of the reaction will be : (A) 1 (B) 2 (C) 4 (D) 9

10.

Which of the following is not a physical equilibrium ? (A)

 Water Ice 

VMC/Chemical Equilibrium

(B)

 I2 (g) (C) I 2 (s) 

2

 S(g) S(l ) 

(D)

 2O3 3O 2 

HWT/Chemistry

Vidyamandir Classes

DATE :

  MARKS :    10 

IITJEE :

NAME :

TIME : 25 MINUTES

TEST CODE : CM-EQ [2]

ROLL NO.

START TIME :

END TIME :

STUDENT’S SIGNATURE :

TIME TAKEN:

PARENT’S SIGNATURE :

 This test contains a total of 10 Objective Type Questions.  Each question carries 1 mark. There is NO NEGATIVE marking. Choose the correct alternative. Only one choice is correct. 1.

5 moles of SO2 and 5 moles of O2 are allowed to react. At equilibrium, it was found that 60% of SO2 is used up. If the partial pressure of the equilibrium mixture is one atmosphere, the partial pressure of O2 is : (A) 0.82 atm (B) 0.52 atm (C) 0.21 atm (D) 0.41 atm

2.

 H 2 (g)  I 2 (g) 2HI(g)  The equilibrium constant of the above reaction is 6.4 at 300 K. If 0.25 mole each of H2 and I2 are added to the system, the equilibrium constant will be : (A) 6.4 (B) 0.8 (C) 3.2 (D) 1.6

3.

  For PCl5 g    PCl3 g   Cl2 g  , initial concentration of each reactant and product is 1 M. If keq = 0.41 then : (A)

more PCl3 will form (B)

more Cl2 will form (C)

more PCl5 will form (D)

4.

For a reaction and equilibrium which of the following is correct ? (A) Concentration of reactant = concentration of product (B) Concentration of reactant is always greater than product (C) Rate forward reaction = rate of backward reaction (D) Qc = k

5.

For the following three reaction I, II, and III, equilibrium constant are given I.

 CO 2  g   H 2  g  ; K1 CO  g   H 2O  g  

III.

 CO 2  g   4H 2  g  ; K 3 CH 4  g   2H 2O  g  

no change

 CO  g   3H 2  g  ; K 2 CH 4  g   H 2O  g  

II.

Which of the following relations is correct ? (A) 6.

K1 K 2  K 3

(B)

K 2K 3  K1

(C)

K3 = K1K2

(D)

K 3K 32  K12

 2Y and Z   P  Q , respectively are in the ratio of 1 : 9. If the The equilibrium constant K p1 and K p2 for the reaction X  degree of dissociation of X and Z be equal, then the ratio of total pressure at these equilibria is : (All gaseous) (A) 1 : 36 (B) 1:1 (C) 1:3 (D) 1:9

7.

 Y  g   Z  g  At 600 C, K p for the following reaction is 1 atm. X  g   At equilibrium, 50% of X (g) is dissociated. The total pressure of the equilibrium system is p atm. What is the partial pressure (in atm) of X (g) at equilibrium? (A) 1 (B) 4 (C) 2 (D) 0.5

8.

In a 500 mL flask, the degree of dissociation of PCl5 at equilibrium is 40 % and the initial amount is 5 moles. The value of equilibrium constant in mol L1 for decomposition of PCl5 is : (A) 2.33 (B) 2.66 (C)

VMC/Chemical Equilibrium

3

5.32

(D)

4.66

HWT/Chemistry

Vidyamandir Classes 9.

For the following reaction in gaseous phase CO(g)  (A)

10.

(RT)1/2

(B)

(RT) 1/ 2

1   O2 (g)   CO2 (g) K p / K c is : 2

(C)

(RT)

(D)

(RT) 1

Three moles of PCl5, three moles of PCl3 and two moles of Cl2 are taken in a closed vessel. If at equilibrium the vessel has 1.5 moles of PCl5, the number of moles of PCl3 present in it is : (A) 5 (B) 3 (C) 6 (D) 4.5

VMC/Chemical Equilibrium

4

HWT/Chemistry

Vidyamandir Classes

DATE :

IITJEE :

NAME :

  MARKS :    10 

TIME : 25 MINUTES

TEST CODE : CM-EQ [3]

ROLL NO.

START TIME :

STUDENT’S SIGNATURE :

END TIME :

TIME TAKEN:

PARENT’S SIGNATURE :

 This test contains a total of 10 Objective Type Questions.  Each question carries 1 mark. There is NO NEGATIVE marking. Choose the correct alternative. Only one choice is correct. 1.

For the reaction,

 H 2  g   I 2  g   Q kJ , 2HI(g)  the equilibrium constant depends upon : (A) temperature only (B) pressure

(C)

catalyst

(D)

volume

2.

1.6 moles of PCl5 (g) is placed in 4 dm3 closed vessel. When the temperature is raised to 500 K, it decomposes and at equilibrium 1.2 moles of PCl5 (g) remains. What is the Kc value of for the decomposition of PCl5(g) to PCl3 (g) and Cl2 at 500 K (A) 0.013 (B) 0.050 (C) 0.033 (D) 0.067 (E) 0.045

3.

Ammonium carbonate decomposes as :

 2NH3  g   CO 2  g  NH 2COONH 4  s   For the reaction, K p  2.9  105 atm3 . If we start with 1 mole of the compound, the total pressure at equilibrium would be : (A)

0.766 atm

(B)

0.0582 atm

(C)

0.0388

(D)

0.0194 atm

4.

1 mole of H2 and 2 moles of I2 are taken initially in a 0.2 L container. Then, the number of H2 at equilibrium is 0.2. Then, the number of moles of I2 and HI at equilibrium are : (A) 1.2, 1.6 (B) 1.8, 1.0 (C) 0.4, 2.4 (D) 0.8, 2.0

5.

On doubling p and V with constant temperature, the equilibrium constant will : (A) remain constant (B) become double (C) become one-fourth (D)

6.

None of these

    The equilibrium constant Kp1 and Kp2 for the reactions X   2Y and Z   P  Q , respectively, are in the ratio of 1 : 9. If the degree of dissociation of X and Z be equal then the ratio of total pressures at these equilibrium is : (A) 1:9 (B) 1 : 36 (C) 1:1 (D) 1:3

7.

4 moles each of SO2 and O2 gases are allowed to react to form SO3 in a closed vessel. At equilibrium 25% of O2 is used up. The total number of moles of all the gases at equilibrium is : (A) 6.5 (B) 7.0 (C) 8.0 (D) 2.0

8.

Formaldehyde polymerizes to form glucose according to the reaction,

 C6H12O6 6 HCHO  The theoretically computed equilibrium constant for this reaction is found to be 6 × 10 22. If 1 M solution of glucose dissociates according to the above equilibrium, the concentration of formaldehyde in the solution will be : (A)

1.6  102 M

VMC/Chemical Equilibrium

(B)

1.6  104 M

(C)

5

1.6  106 M

(D)

1.6  108 M

HWT/Chemistry

Vidyamandir Classes 9.

In chemical equilibrium, the value of n (number of molecules), is negative, then the relationship between Kp and Kc will be : (A)

10.

Kp  Kc  0

(B)

K p  K c   RT 

n

(C)

K p  K c   RT 

n

(D)

Kp 

1 Kc

 1 N 2  O 2 , K1 ; N 2O 4   2NO 2 , K 2 Consider the reaction, NO 2  2 Give the equilibrium constant for the formation of N2O4 from N2 and O2.

(A)

1 K12



1 K2

VMC/Chemical Equilibrium

(B)

1 K1K 2

(C)

6

1 K1 K 2

(D)

K2 K1

HWT/Chemistry

Vidyamandir Classes

DATE :

IITJEE :

NAME :

  MARKS :    10 

TIME : 25 MINUTES

TEST CODE : CM-EQ [4]

ROLL NO.

START TIME :

STUDENT’S SIGNATURE :

END TIME :

TIME TAKEN:

PARENT’S SIGNATURE :

 This test contains a total of 10 Objective Type Questions.  Each question carries 1 mark. There is NO NEGATIVE marking. Choose the correct alternative. Only one choice is correct. 1.

  For the reaction CO (g)  0.5O 2 (g)   CO 2 (g) Kp/Kc is equal to : 1 (A) (B) RT RT

(C) 2.

3.

1

(D)

7.

RT2

The equilibrium constant (Kc) of the reaction

Equivalent amounts of H2 and I2 are heated in a closed vessel till equilibrium is obtained. If 80 % of the hydrogen can be converted to H, the Kc at this temperature is : (A) 64 (B) 16 (C) 0.25 (D) 4

6.08 × 106

(C)

6.08  109

(D)

None of these

Phosphorus pentachloride dissociates as follows, in a closed reaction vessel,

 3   Ag   NH 3   [Ag(NH 3 )] ; K1  2.5  10    [Ag(NH 3 )]  NH 3   [Ag(NH 3 ) 2 ] ;

(A)

 x   p  x  1

(B)

 2x   p 1  x 

(C)

 x   p  x  1

(D)

 x   p 1  x 

8.

1 mole of N2O4 (g) at 300 K is kept in a closed container under 1 atm. It is heated to 600 K when 20 % by mass of N2O4(g) decomposes to NO2(g). The resultant pressure is : (A) 1.2 atm (B) 2.4 atm (C) 2.0 atm (D) 1.0 atm

9.

The chemical equilibrium of a reversible reaction is not influenced by : (A) pressure (B) catalyst (C) concentration of the reactants (D) temperature

10.

56 g of nitrogen and 8 g of hydrogen gas are heated in a closed vessel. At equilibrium 34 g of ammonia are present. The equilibrium number of moles of nitrogen, hydrogen and ammonia are respectively (A) 1, 2, 2 (B) 2, 2, 1 (C) 1, 1, 2 (D) 2, 1, 2

  A  B   C  D . If initially the concentration of

A and B are both equal but at equilibrium, concentration of D will be twice of that of A, then what will be the equilibrium constant of reaction ? (A) 4/9 (B) 9/4 (C) 1/9 (D) 4 6.

(B)

If total pressure at equilibrium of the reaction mixture is p and degree of dissociation of PCl5 is x, the partial pressure of PCl3 will be :

is 50. If 1 mol of A2 and 2 mol of B2 are mixed, the amount of AB at equilibrium would be : (A) 0.934 mol (B) 0.467 mol (C) 1.866 mol (D) 1.401 mol

5.

6.08  106

 PCl3  g   Cl2  g  PCl5  g  

A liquid is in equilibrium with its vapour at it’s boiling point. On the average, the molecules in two phases have equal : (A) inter-molecular forces (B) potential energy (C) kinetic energy (D) total energy

  A 2 (g)  B2 (g)   2AB(g)

4.

(A)

K 2  1.7  103 then the formation constant of [Ag(NH3)2]+ is :

VMC/Chemical Equilibrium

7

HWT/Chemistry

Vidyamandir Classes

DATE :

  MARKS :    10 

IITJEE :

NAME :

TIME : 25 MINUTES

TEST CODE : CM-EQ [5]

ROLL NO.

START TIME :

END TIME :

STUDENT’S SIGNATURE :

TIME TAKEN:

PARENT’S SIGNATURE :

 This test contains a total of 10 Objective Type Questions.  Each question carries 1 mark. There is NO NEGATIVE marking. Choose the correct alternative. Only one choice is correct. 1.

2.

Which of the following is not a characteristic property of chemical equilibrium? (A) Rate of forward reaction is equal to rate of backward reaction at equilibrium (B) After reaching the chemical equilibrium, the concentrations of reactants and products remain unchanged with time (C)

 B  g  , K c is 102 . If this reaction is carried out in the presence of catalyst, the value of Kc decreases For A  g  

(D)

After reaching the equilibrium, both forward and backward reactions continue to take place

Which of the following is correct for the reaction ?

 2NH3  g  N 2  g   3H 2  g   (A) (D) 3.

Kp = Kc (B) Kp < Kc Pressure is required to predict the correlation

(C)

Kp > Kc

Consider the following equilibrium in a closed container,

 2NO 2  g  N 2O 4  g   At a fixed temperature, the volume of the reaction container is halved. For this change of the following statement holds true regarding the equilibrium constant (Kp) and degree of dissociation () ? (A) (C)

Neither Kp nor  changes Kp changes but  does not

(B) (D)

Both Kp and  changes Kp does not change but  changes

4.

The equilibrium constant of a reaction is 300. If the volume of reaction flask is tripled, the equilibrium constant is : (A) 300 (B) 600 (C) 900 (D) 100

5.

The equilibrium reaction that is not influenced by volume change at constant temperature is :

6.

7.

(A)

 2HI  g  H 2  g   I 2  g  

(B)

 2NH3  g  N 2  g   3H 2  g  

(C)

 2NO 2  g  N 2O 4  g  

(D)

 2NO 2  g  2NO  g   O 2 

An amount of solid NH4HS is placed in a flask already containing ammonia gas at a certain temperature and 0.50 atm pressure. Ammonium hydrogen sulphide decomposes to yield NH3 and H2S gases in the flask when the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 0.84atm. The equilibrium constant for NH4 decomposition at this temperature is: (A) 0.11 (B) 0.17 (C) 0.18 (D) 0.30

 4Ag  s   O 2  g  is : Partial pressure of O2 in the reaction 2Ag 2O  s   (A)

KP

VMC/Chemical Equilibrium

(B)

Kp

(C)

8

3 Kp

(D)

2KP

HWT/Chemistry

Vidyamandir Classes 8.

9.

The change in pressure will not affect the equilibrium constant for : (A)

  N 2  3H 2   2NH 3

(B)

  PCl5   PCl3  Cl 2

(C)

  H 2  I 2   2HI

(D)

All of these

For the reaction :    N 2 (g)  O 2 (g)   2NO(g) , the value of Kc at 800 C is. 0.1. When the equilibrium concentration of both the reactants is 0.5 mole, what is the value of Kp at the same temperature ? (A) 0.5 (B) 0.1 (C) 0.01 (D) 0.025

10.

  A(g)  3B(g)   4C(g) . Initially concentration of A is equal to that of B. The equilibrium concentrations of A and C are equal. Kc is. 1 (A) 0.08 (B) 8 (C) 80 (D) 8

VMC/Chemical Equilibrium

9

HWT/Chemistry

Vidyamandir Classes

DATE :

IITJEE :

NAME :

  MARKS :    10 

TIME : 25 MINUTES

TEST CODE : CM-EQ [6]

ROLL NO.

START TIME :

STUDENT’S SIGNATURE :

END TIME :

TIME TAKEN:

PARENT’S SIGNATURE :

 This test contains a total of 10 Objective Type Questions.  Each question carries 1 mark. There is NO NEGATIVE marking. Choose the correct alternative. Only one choice is correct. 1.

2.

Two moles of PCl5 is heated in a closed vessel of 2 L capacity. When the equilibrium is attained 40 % of it has been found to be dissociated. What is the Kc in mol/dm3 ? (A) 0.532 (B) 0.266 (C) 0.133 (D) 0.174 (E) 0.25 At 550 K, the Kc for the following reaction is 104 mol1 L

  X(g)  Y(g)   Z(g)





1 1 At equilibrium, it was observed that [X]  [Y]  [Z] . What is the value of [Z] in mol L1 at equilibrium ? 2 2

(A) 3.

2  104

(B)

104

(C)

2  104

(D)

104

For the reaction,

  H 2  g   CO2  g    CO  g   H 2 O  g  , if the initial concentration of [H2] = [CO2] and x mol/L of hydrogen is consumed at equilibrium, the correct expression of Kp is : (A)

4.

5.

x2

1  x 2

(B)

1  x 2 1  x 2

(C)

For a reaction if Kp > Kc the forward reaction is favoured by : (A) low pressure (B) high pressure (C)

x2

 2  x 2

(D)

high temperature

(D)

7.

low temperature

(D)

0.25

In which of the following reactions, the concentration of product is higher than the concentration of reactant at equilibrium? (K = equilibrium constant) (A)

  A   B; K  0.001

(B)

  M   N ; K  10

(C)

  X   Y ; K  0.005

(D)

  R   P ; K  0.01 

Calculate the partial pressure of carbon monoxide from the following data’s CaCO3 (s)  CaO  s   CO2 (g) K p  8  102 CO2  g   C  s    2CO  g  ; K p  2 (A) 0.2 (B) 0.4

8.

1  x2

  The compounds A and B are mixed in equimolar proportion to form the products, A  B   C  D . At equilibrium, one thirt

of A and B are consumed. The equilibrium constant for the reaction is : (A) 0.5 (B) 4.0 (C) 2.5 6.

x2

(C)

1.6

(D)

4

 4PCl3  g  attained by mixing equal moles of P 4 and Cl2 in a evacuated vessel. Then at The equilibrium, P4  s   6Cl2  g   equilibrium. (A) [Cl2] > {PCl3]

VMC/Chemical Equilibrium

(B)

[Cl2] > [P4]

(C)

10

[P4] > [Cl2]

(D)

[PCl3] > [P4]

HWT/Chemistry

Vidyamandir Classes 9.

  Consider the following reaction equilibrium N 2  g   3H 2  g    2NH 3  g  Initially, 1 mole N2 3 moles of H2 are take in a 2 L flask. At equilibrium state if, the number of moles of N2 is 0.6, what is the total number of moles of all gases present in the flask? (A) 0.8 (B) 1.6 (C) 3.2 (D) 6.4

10.

  N 2  g   3H 2  g    2NH 3  g  In the reaction given above, the addition of small amount of an inert gas at constant pressure will shift the equilibrium towards which side? (A) LHS (Left hand side) (B) RHS (Right hand side) (C) Neither side (D) Either side

VMC/Chemical Equilibrium

11

HWT/Chemistry

Vidyamandir Classes

DATE :

  MARKS :    10 

IITJEE :

NAME :

TIME : 25 MINUTES

TEST CODE : CM-EQ [7]

ROLL NO.

START TIME :

END TIME :

STUDENT’S SIGNATURE :

TIME TAKEN:

PARENT’S SIGNATURE :

 This test contains a total of 10 Objective Type Questions.  Each question carries 1 mark. There is NO NEGATIVE marking. Choose the correct alternative. Only one choice is correct 1.

The

reaction

 2SO3  heat . 2SO 2  O 2 

equilibrium reaction proceeds in forward direction by (A) addition of O2 (B) removal of O2 (C) additional of inert gas (D) cannot proceed 2.

  N 2 (g)  3H 2 (g)   2NH 3 (g)  heat . What is the effect of the increase of temperature on the equilibrium of the reaction ? (A) Equilibrium is shifted to the left (B) Equilibrium is shifted to the right (C) Equilibrium is unaltered (D) Reactions rate does not change

3.

Formation of SO3 from SO2 and O2 is favoured by : (A) increase in pressure (B) decrease in pressure (C) increase in temperature (D) decrease in temperature

4.

When hydrogen molecules decomposed into its atoms, which conditions gives maximum yield of H atom? (A) High temperature and low pressure (B) Low temperature and high pressure (C) High temperature and high pressure (D) Low temperature and low pressure

5.

(A) (B) (D)

The

According to Le-Chatelier principle, adding heat to solid and liquid in equilibrium will cause the : (A) amount of solid to decrease (B) amount of liquid to decrease (C) temperature to rise (D) temperature to fall

8.

Given the equilibrium system     NH 4 Cl (s)   NH 4 (aq)  Cl (aq) ( H   3.5 kcal / mol)

What change will shift the equilibrium to the right ? (A) Decreasing the temperature (B) Increasing the temperature (C) Dissolving NaCl crystals in the equilibrium mixture (D) Dissolving NH4NO3 crystals in the equilibrium mixture 9.

10.

  N 2 (g)  3H 2 (g)   2NH 3 (g)

In the manufacture of ammonia by Haber’s process,

 2NH3  g   92.3 kJ N 2  g   3H 2  Which of the following condition is unfavourable? (A) Increasing the temperature (B) Increasing the pressure (C) Reducing the temperature (D) Removing ammonia as it is formed

For the chemical reaction

 X3Y  g  , 3X  g   Y  g   that amount of X3Y at equilibrium is affected by :

VMC/Chemical Equilibrium

For the reaction

H   93.6 kJ mol 1 the formation of NH3 is expected to increase at : (A) high pressure and low temperature (B) low pressure and low temperature (C) high pressure and high temperature (D) low pressure and high temperature

CO 2  g   2H 2O  g    CH 4  g   2O 2  g 

6.

only

7.

According to Le-Chatelier’s principle, the addition of temperature to the following reaction

Will cause it to the right. This reaction is, therefore : (A) exothermic (B) unimolecular (C) endothermic (D) spontaneous

temperature and pressure temperature only (C) pressure temperature, pressure and catalyst

12

HWT/Chemistry

Vidyamandir Classes

DATE :

  MARKS :    10 

IITJEE :

NAME :

TIME : 25 MINUTES

TEST CODE : CM-EQ [8]

ROLL NO.

START TIME :

END TIME :

STUDENT’S SIGNATURE :

TIME TAKEN:

PARENT’S SIGNATURE :

 This test contains a total of 10 Objective Type Questions.  Each question carries 1 mark. There is NO NEGATIVE marking. Choose the correct alternative. Only one choice is correct. 1.

 2ClF3  g  ; H   329 kJ The exothermic formation of ClF3 is represented by the equation Cl2  g   3F2  g   Which of the following will increase the quantity of ClF3 in an equilibrium mixture of Cl2 F2 and ClF3? (A) Adding F2 (B) Increasing the volume of the container (C) Removing Cl2 (D) Increasing the temperature

2.

3.

4.

1   For the gaseous reaction, C2 H 4 (g)  H 2 (g)  carried in a closed vessel, the  C2 H 6 (g), H(g)   130 kJ mol equilibrium concentration of the C2H6 can definitely be increased by. (A) increasing temperature and decreasing pressure (B) decreasing temperature and pressure both (C) increasing temperature and pressure both (D) decreasing temperature and pressure both

   In a lime kiln, to get higher yield of CO2, the measure than can be taken is: CaCO3 (s)   CO 2 (g)  CaO (s)    (A) to remove CaO (B) to add more CaCO3 (C) to add CO2 (D) to pump out CO2   In the given reaction, 2X(g)  Y(g)   2Z(g)  80 kcal , Which combination of pressure and temperature will give the highest yield of Z of equilibrium? (A) 1000 atm and 200C (B) 500 atm and 500C (C) 1000 atm and 100C (D) 500 atm and 100C

(E)

1000 atm and 500C

5.

When pressure is applied to the equilibrium system ice and water. Which of the following phenomenon will happen? (A) More ice will be formed (B) Water will evaporate (C) More water will be formed (D) Equilibrium will not be formed

6.

  For the reaction, PCl3 (g)  Cl 2 (g)   PCl5 (g) the position of equilibrium can shifted to the right by : (A) doubling the volume (B) increasing the temperature (C) addition of equimolar quantities of PCl3 and PCl5 (D) addition of Cl2 at constant volume

7.

A reversible reaction is one which : (A) proceeds in both directions (C) proceeds spontaneously

(B) (D)

proceeds in one directions All the above statements are wrong

8.

In a reaction, the rate of reaction is proportional to its active mass. This statement is known as : (A) law of mass-action (B) Le-Chatelier principle (C) Faraday law of electrolysis (D) law of constant proportion

9.

  In the equilibrium, AB   A  B , if the equilibrium concentration of A is doubled, the equilibrium concentration of B would become : 1 1 th th (A) half (B) twice (C) (D) 4 8 According to law of mass action, for the reaction :

10.

(A)

2A  B   Pr oducts Rate = k[A] [B] (B)

VMC/Chemical Equilibrium

Rate = k[A]2 [B]

(C)

13

Rate = k[A] [B]2

(D)

Rate = k [A]1/2 [B]

HWT/Chemistry

Vidyamandir Classes

DATE :

  MARKS :    10 

IITJEE :

NAME :

TIME : 25 MINUTES

TEST CODE : CM-EQ [9]

ROLL NO.

START TIME :

END TIME :

STUDENT’S SIGNATURE :

TIME TAKEN:

PARENT’S SIGNATURE :

 This test contains a total of 10 Objective Type Questions.  Each question carries 1 mark. There is NO NEGATIVE marking. Choose the correct alternative. Only one choice is correct. 1.

 C , the expression for equilibrium constant is : For the system; 3A  2B  3

(A)

2.

2

A  B C

(B)

C 3

2

A  B

(C)

3A  2B C  

(D)

C 3A   2B

 Z, 2 moles of Z are formed. 5 mole of X are mixed with 3 moles of Y. At equilibrium for the reaction, X  Y  The equilibrium constant for the reaction will be : (A)

2 3

(B)

1 2

(C)

3 2

3.

The equilibrium constant in a reversible reaction at a given temperature (A) does not depend on the initial concentrations (B) depends on the initial concentrations of the reactants (C) depends on the concentration of the products at equilibrium (D) it is not a characteristic of the reaction

4.

 FeS(s) the expression for equilibrium constant is : For the reaction, Fe(s)  S(s)  (A)

5.

6.

[FeS] [Fe][S]

(B)

[Fe][S] [FeS]

(C)

[Fe] [S] [FeS]

(D)

(D)

1 4

None of these

For which of the following reactions, does the equilibrium constant depend on the units of concentration? (A)

 1 N 2 (g)  1 O 2 (g) NO(g)  2 2

(B)

 Cu(s)  Zn 2  (aq) Zn(s)  Cu 2 (aq) 

(C)

 CI(g)  Cl2 (g) COCl2 (g) 

(D)

 CH3COOC 2H5 (l ) C2H5OH(l )  CH3COOH(l ) 

On a given condition, the equilibrium concentration of HI, H2 and I2 are 0.80, 0.10 and 0.10 mol/L. the equilibrium constant for the

 2HI will be : reaction, H 2  I 2  (A) 7.

8

(B)

16

(C)

32

(D)

64

For the decomposition reaction : 5 3   NH 2 COONH 4 (s)   2NH 3 (g)  CO2 (g) the K 2  2.9  10 atm .

The total pressure of gases at equilibrium when 1.0 mol of NH2COONH4(s) was taken to start with, would be : (A) 0.0194 (B) 0.0388 atm (C) 0.0582 atm (D) 0.0776 atm 8.

 C , would be : The unit of equilibrium constant, K for the reaction, A  B  (A)

mol L1

VMC/Chemical Equilibrium

(B)

mol L

(C)

14

L mol1

(D)

dimensionless

HWT/Chemistry

Vidyamandir Classes 9.

 2C , if 2 moles of A, 3.0 moles of B and 2.0 moles of C are placed in a 2 L flask and the equilibrium In the reaction, A  2B  concentration of C is 0.5 mol/L, the equilibrium constant (Kc) for the reaction is : (A) 0.21 (B) 0.50 (C) 0.75

10.

(D)

0.05

 2NO 2  g  , the concentrations of N2O4 and NO2 at equilibrium are For the reaction equilibrium, N 2O 4  g  

4.8  102 and 1.2  102 mol / L respectively. The value of Kc for the reaction is : (A)

3  103 mol / L

VMC/Chemical Equilibrium

(B)

3.3  103 mol / L (C)

15

3  101 mol / L

(D)

3.3  101 mol / L

HWT/Chemistry

Vidyamandir Classes

DATE :

  MARKS :    10 

IITJEE :

NAME :

TIME : 25 MINUTES

TEST CODE : CM-EQ [10]

ROLL NO.

START TIME :

STUDENT’S SIGNATURE :

END TIME :

TIME TAKEN:

PARENT’S SIGNATURE :

 This test contains a total of 10 Objective Type Questions.  Each question carries 1 mark. There is NO NEGATIVE marking. Choose the correct alternative. Only one choice is correct. 1.

4   The equilibrium constant for the reaction N 2 (g)  O 2 (g)   2NO(g) at temperature T is 4  10 . The value of Kc for the

  reaction NO(g)  

(A)

2.

25

Kc 

7.

(B)

K c  [O 2 ]5

Kc 

(C)

[P4O10 ] 5[P4 ][O 2 ]

(D)

Kc 

(D)

1.0

[P4O10 ] [P4 ][O 2 ]5

(B)

RT

(C)

RT

   For the reaction C2 H 4 (g)  H 2 (g)   C2 H 6 (g) , which of the following expressions between Kp and Kc is true at 27 C ?

Kp > Kc

(B)

Kp < Kc

(C)

Kp = Kc

(D)

cannot be predicted

   For the reaction, PCl3  g   Cl 2 (g)   PCl5 (g) , the value of Kc at 250 C is 26. The value of Kp at this temperature will be :

(A) 6.

1 [O 2 ]5

1/RT

(A)

5.

100

  For the reaction, CO(g)  Cl 2 (g)   COCl 2 (g) , the Kp/Kc is equal to :

(A) 4.

(D)

  What is the equilibrium expression for the reaction, P4 (s)  5O2 (g)   P4 O10 (s) ?

(A)

3.

1 1 N 2 (g)  O 2 (g) at the same temperature is. 2 2 (B) 50 (C) 75

0.41

(B)

0.51

(C)

0.61

(D)

0.71

In which one of the following gaseous equilibrium, Kp is less than Kc? (A)

 2NO 2  g  N 2O 4  g  

(B)

 2SO3  g  2SO 2  g   O 2  g  

(C)

 H 2  g   I 2  g  2HI  g  

(D)

 2NO  g  N 2  g   O 2  g  

 2NH3  g  is K then the equilibrium constant for the equilibrium, The equilibrium constant for the reaction N 2  g   3H 2  g    1 N 2  g   3 H 2  g  is : NH3  g   2 2 1 K

(A)

8.

For

the

NO(g) 

(A)

(B)

K

(C)

1 K

2

6    reaction, 2NO 2 (g)   2NO(g)  O 2 (g), K c  1.8  10 at 185 C ,

1  NO 2 (g) is : O 2 (g)  2 0.9 × 106 (B)

VMC/Chemical Equilibrium

1.9 × 106

(C)

16

7.5 × 102

1 K

(D)

the

(D)

value

of

Kc

for

the

reaction

5.7 × 102

HWT/Chemistry

Vidyamandir Classes 9.

Of the following which change will shift the reaction towards the product ?

 2I(g), I 2 (g)  (A) (C) 10.

Hr  298 K    150 kJ

Increase in temperature Increase in concentration of I

(B) (D)

Increase in total pressure Decrease in concentration of I2

In the following reversible reaction,

 2SO3  g   Q cal 2SO 2  g   O 2  g   Most suitable condition for the higher production of SO3 is. (A) low temperature and high pressure (B) (C) high temperature and high pressure (D)

VMC/Chemical Equilibrium

17

low temperature and low pressure high temperature and low pressure

HWT/Chemistry

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