# Chemical Equilibrium Test 3

Total Questions:50 Total Time: 75 Min

Remaining:

## Questions 1 of 50

Question:Which of the following conditions represents an equilibrium

Freezing of ice in a open vessel, temperature of ice is constant

Few drops of water is present along with air in a balloon, temperature of balloon is constant

Water is boiling in an open vessel over stove, temperature of water is constant

All the statements , and are correct for the equilibrium

## Questions 2 of 50

Question:When rate of forward reaction becomes equal to backward reaction, this state is termed as

Chemical equilibrium

Reversible state

Equilibrium

All of these

## Questions 3 of 50

Question:In chemical reaction $$A$$ $$\Leftrightarrow$$$$B$$, the system will be known in equilibrium when

A completely changes to B

50% of A changes to B

The rate of change of A to B and B to A on both the sides are same

Only 10% of A changes to B

## Questions 4 of 50

Question:In the reaction $${N_2}(g) + 3{H_2}$$ $$\Leftrightarrow$$ $$2N{H_3}(g)$$, the value of the equilibrium constant depends on

Volume of the reaction vessel

Total pressure of the system

The initial concentration of nitrogen and hydrogen

The temperature

## Questions 5 of 50

Question:In which of the following equilibria, the value of $${K_p}$$ is less than $${K_c}$$

$${H_2} + {I_2}$$ $$\Leftrightarrow$$ $$2HI$$

$${N_2} + 3{H_2}$$ $$\Leftrightarrow$$$$2N{H_3}$$

$${N_2} + {O_2}$$ $$\Leftrightarrow$$ $$2NO$$

$$CO + {H_2}O$$ $$\Leftrightarrow$$ $$C{O_2} + {H_2}$$

## Questions 6 of 50

Question:Two gaseous equilibria $$S{O_{2(g)}} + \frac{1}{2}{O_{2(g)}}$$ $$\Leftrightarrow$$ $$S{O_{3(g)}}$$ and $$2S{O_{3(g)}}$$ $$\Leftrightarrow$$$$2S{O_{2(g)}} + {O_{2(g)}}$$ have equilibrium constants $${K_1}$$ and $${K_2}$$ respectively at $$298\,K$$. Which of the following relationships between $${K_1}$$ and $${K_2}$$ is correct

$${K_1} = {K_2}$$$${K_2} = K_1^2$$

$${K_2} = \frac{1}{{K_1^2}}$$

$${K_2} = \frac{1}{{{K_1}}}$$

$${H_2} + {I_2}$$ $$\Leftrightarrow$$$$2HI$$

## Questions 7 of 50

Question:For reaction 2NOCl(g) $$\Leftrightarrow$$ $$2NO(g) + C{l_2}(g)$$, $${K_C}$$at 427°C is $$3 \times {10^{ - 6}}L\;mo{l^{ - 1}}$$. The value of $${K_P}$$ is nearly

$$7.50 \times {10^{ - 5}}$$

$$2.50 \times {10^{ - 5}}$$

$$2.50 \times {10^{ - 4}}$$

$$1.75 \times {10^{ - 4}}$$

## Questions 8 of 50

Question:For which one of the following reactions $${K_p} = {K_c}$$

$${N_2} + 3{H_2}$$ $$\Leftrightarrow$$$$2N{H_3}$$

$${N_2} + {O_2}$$ $$\Leftrightarrow$$$$2NO$$

$$PC{l_5}$$ $$\Leftrightarrow$$$$PC{l_3} + C{l_2}$$

$$2S{O_3}$$ $$\Leftrightarrow$$$$2S{O_2} + {O_2}$$

## Questions 9 of 50

Question:The equilibrium constant for the reversible reaction, $${N_2} + 3{H_2}$$ $$\Leftrightarrow$$ $$2N{H_3}$$ is $$K$$ and for the reaction $$\frac{1}{2}{N_2} + \frac{3}{2}{H_2}$$ $$\Leftrightarrow$$ $$N{H_3}$$ the equilibrium constant is $$K'$$. $$K$$ and $$K'$$ will be related as

$$K = K'$$

$$K' = \sqrt K$$

$$K = \sqrt {K'}$$

$$K \times K' = 1$$

## Questions 10 of 50

Question:If $${K_c}$$ is the equilibrium constant for the formation of $$N{H_3}$$, the dissociation constant of ammonia under the same temperature will be

$${K_c}$$

$$\sqrt {{K_c}}$$

$$K_c^2$$

$$1/{K_c}$$

## Questions 11 of 50

Question:3.2 moles of hydrogen iodide were heated in a scaled bulb at 444°C till the equilibrium was reached. The degree of dissociation of HI at this temperature was found to be 22%. The number of moles of hydrogen iodide present at equilibrium are

1.87

2.496

4

2

## Questions 12 of 50

Question:The $${K_c}$$ for $${H_{2(g)}} + {I_{2(g)}}$$ $$\Leftrightarrow$$$$2H{I_{(g)}}$$ is 64. If the volume of the container is reduced to one-half of its original volume, the value of the equilibrium constant will be

28

64

32

16

## Questions 13 of 50

Question:The chemical equilibrium of a reversible reaction is not influenced by

Pressure

Catalyst

Concentration of the reactants

Temperature

## Questions 14 of 50

Question:Of the following which change will shift the reaction towards the product $${I_2}(g)$$ $$\Leftrightarrow$$$$2I(g),\;\Delta H_r^0(298K) = + 150\;kJ$$

Increase in concentration of l

Decrease in concentration of $${I_2}$$

Increase in temperature

Increase in total pressure

## Questions 15 of 50

Question:For the reaction, $$C{O_{(g)}} + C{l_{2(g)}}$$ $$\Leftrightarrow$$ $$COC{l_{2(g)}}$$ the $${K_p}/{K_c}$$ is equal to

$$\sqrt {RT}$$

$$RT$$

$$1/RT$$

$$1.0$$

## Questions 16 of 50

Question:On a given condition, the equilibrium concentration of $$HI,\,{H_2}$$ and $${I_2}$$ are 0.80, 0.10 and 0.10 mole/litre. The equilibrium constant for the reaction $${H_2} + {I_2}$$ \ [ \Leftrightarrow \) $$2HI$$ will be

64

12

8

0.8

## Questions 17 of 50

Question:In which of the following, the reaction proceeds towards completion

$$K = {10^3}$$

$$K = {10^{ - 2}}$$

$$K = 10$$

$$K = 1$$

## Questions 18 of 50

Question:A reversible chemical reaction having two reactants in equilibrium. If the concentrations of the reactants are doubled, then the equilibrium constant will

Also be doubled

Be halved

Become one-fourth

Remain the same

## Questions 19 of 50

Question:In a chemical equilibrium $$A + B$$ $$\Leftrightarrow$$ $$C + D$$, when one mole each of the two reactants are mixed, 0.6 mole each of the products are formed. The equilibrium constant calculated is

1

0.36

2.25

9-Apr

## Questions 20 of 50

Question:For the reaction $${N_{2(g)}} + 3{H_{2(g)}}$$ $$\Leftrightarrow$$ $$2N{H_{3(g)}}$$, the correct expression of equilibrium constant K is

$$K = \frac{{{{[N{H_3}]}^2}}}{{[{N_2}]{{[{H_2}]}^3}}}$$

$$K = \frac{{[{N_2}]{{[{H_2}]}^3}}}{{{{[N{H_3}]}^2}}}$$

$$K = \frac{{2[N{H_3}]}}{{[{N_2}] \times 3[{H_2}]}}$$

$$K = \frac{{[{N_2}] \times 3[{H_2}]}}{{2[N{H_3}]}}$$

## Questions 21 of 50

Question:The suitable expression for the equilibrium constant of the reaction $$2N{O_{(g)}} + C{l_{2(g)}}$$ $$\Leftrightarrow$$ $$2NOC{l_{(g)}}$$ is

$${K_c} = \frac{{[2NOCl]}}{{[2NO]\,[C{l_2}]}}$$

$${K_c} = \frac{{{{[NOCl]}^2}}}{{{{[NO]}^2}[C{l_2}]}}$$

$${K_c} = \frac{{{{[NOCl]}^2}}}{{[NO]{{[C{l_2}]}^2}}}$$

$${K_c} = \frac{{{{[NOCl]}^2}}}{{{{[NO]}^2}{{[C{l_2}]}^2}}}$$

## Questions 22 of 50

Question:4.5 moles each of hydrogen and iodine heated in a sealed ten litre vessel. At equilibrium, 3 moles of $$HI$$ were found. The equilibrium constant for $${H_2}(g) + {I_2}(g)$$ $$\Leftrightarrow$$$$2HI(g)$$ is

1

10

5

0.33

## Questions 23 of 50

Question:An equilibrium mixture of the reaction $$2{H_2}S(g)$$ $$\Leftrightarrow$$$$2{H_2}(g) + {S_2}(g)$$ had 0.5 mole $${H_2}S$$, 0.10 mole $${H_2}$$ and 0.4 mole $${S_2}$$ in one litre vessel. The value of equilibrium constant $$(K)$$ in mole litre-1 is

0.004

0.008

0.016

0.16

## Questions 24 of 50

Question:At 3000 K the equilibrium pressures of CO2, CO and O2 are 0.6,0.4 and 0.2 atmospheres respectively. $${K_p}$$for the reaction, $$2C{O_2}$$ $$\Leftrightarrow$$$$2CO + {O_2}$$ is

0.089

0.0533

0.133

0.177

## Questions 25 of 50

Question:The equilibrium constant (Kc) for the reaction $${\rm{HA}} + {\rm{B}}$$ $$\Leftrightarrow$$$${\rm{B}}{{\rm{H}}^ + } + {{\rm{A}}^ - }$$ is 100. If the rate constant for the forward reaction is 105, then rate constant for the backward reaction is

$${10^7}$$

$${10^3}$$

$${10^{ - 3}}$$

$${10^{ - 5}}$$

## Questions 26 of 50

Question:9.2 grams of $${N_2}{O_{4(g)}}$$ is taken in a closed one litre vessel and heated till the following equilibrium is reached $${N_2}{O_{4(g)}}$$ $$\Leftrightarrow$$ $$2N{O_{2(g)}}$$. At equilibrium, 50% $${N_2}{O_{4(g)}}$$ is dissociated. What is the equilibrium constant (in mol litre–1) (Molecular weight of $${N_2}{O_4} = 92)$$

0.1

0.4

0.2

2

## Questions 27 of 50

Question:Two moles of $$N{H_3}$$ when put into a previously evacuated vessel (one litre), partially dissociate into $${N_2}$$ and $${H_2}$$. If at equilibrium one mole of NH3 is present, the equilibrium constant is

3/4 $$mo{l^2}\,litr{e^{ - 2}}$$

27/64 $$mo{l^2}\,litr{e^{ - 2}}$$

27/32 $$mo{l^2}\,litr{e^{ - 2}}$$

27/1 $$mo{l^2}\,litr{e^{ - 2}}$$

## Questions 28 of 50

Question:Ammonia carbonate when heated to 200°C gives a mixture of $$N{H_3}$$ and $$C{O_2}$$vapour with a density of 13.0. What is the degree of dissociation of ammonium carbonate

$$3/2$$

$$1/2$$

2

1

$$5/2$$

## Questions 29 of 50

Question:2 mol of $${N_2}$$ is mixed with 6 mol of $${H_2}$$in a closed vessel of one litre capacity. If 50% of $${N_2}$$is converted into $$N{H_3}$$at equilibrium, the value of $${K_c}$$for the reaction $${N_{2(g)}} + 3{H_{2(g)}}$$ $$\Leftrightarrow$$$$2N{H_{3(g)}}$$is

$$4/27$$

$$27/4$$

$$1/27$$

24

9

## Questions 30 of 50

Question:For a reaction $${H_2} + {I_2}$$ $$\Leftrightarrow$$$$2HI$$at 721K, the value of equilibrium constant is 50. If 0.5 mols each of $${H_2}$$and $${I_2}$$is added to the system the value of equilibrium constant will be

40

60

50

30

## Questions 31 of 50

Question:What is the effect of halving the pressure by doubling the volume on the following system at 500$$^\circ$$C $${H_{2(g)}} + {I_{2(g)}}$$ $$\Leftrightarrow$$ $$2H{I_{(g)}}$$

Shift to product side

Shift to product formation

Liquefaction of HI

No effect

## Questions 32 of 50

Question:Chemical equations convey quantitative information on the

Type of atoms/molecules taking part in the reaction

Number of atoms/molecules of the reactants and products involved in the reaction

Relative number of moles of reactants and products involved in the reaction

Quantity of reactant consumed and quantity of product formed

## Questions 33 of 50

Question:In the thermal decomposition of potassium chlorate given as $$2KCl{O_3} \to 2KCl + 3{O_2}$$, law of mass action

Cannot be applied

Can be applied

Can be applied at low temperature

Can be applied at high temp. and pressure

## Questions 34 of 50

Question:When in any system at equilibrium state pressure, temperature and concentration is changed then the equilibria shifted to such a direction which neutralize the effect of change. This is known as

First law of thermodynamics

Le-chatelier's principle

Ostwald's rule

Hess's law of constant heat summation

$${N_2} + {O_2}$$ $$\Leftrightarrow$$ $$2NO - Q\,cals$$

## Questions 35 of 50

Question:In the above reaction which is the essential condition for the higher production of $$NO$$

High temperature

High pressure

Low temperature

Low pressure

## Questions 36 of 50

Question:For the equilibrium $$2N{O_2}(g)$$ $$\Leftrightarrow$$ $${N_2}{O_4}(g)$$ $$+ 14.6\,kcal$$ the increase in temperature would

Favour the formation of $${N_2}{O_4}$$

Favour the decomposition of $${N_2}{O_4}$$

Not alter the equilibrium

Stop the reaction

## Questions 37 of 50

Question:Which of the following factors will favour the reverse reaction in a chemical equilibrium

Increase in the concentration of one of the reactants

Removal of at least one of the product at regular time intervals

Increase in the concentration of one or more products

None of these

## Questions 38 of 50

Question:In the formation of $$S{O_3}$$ by contact process, the conditions used are

Catalyst, optimum temperature and higher concentration of reactants

Catalyst, optimum temperature and lower concentration of reactants

Catalyst, high temperature and higher concentration of reactants

Catalyst, low temperature and lower concentration of reactants

## Questions 39 of 50

Question:Given reaction is $$2{X_{(gas)}} + {Y_{(gas)}}$$ $$\Leftrightarrow$$ $$2{Z_{(gas)}} + 80\,kcal$$ Which combination of pressure and temperature gives the highest yield of Z at equilibrium

1000 atm and $${500^o}C$$

500 atm and $${500^o}C$$

1000 atm and $${100^o}C$$

500 atm and $${100^o}C$$

## Questions 40 of 50

Question:In the reaction $$A(g) + B(g)$$ $$\Leftrightarrow$$ $$C(g)$$, the backward reaction is favoured by

Decrease of pressure

Increase of pressure

Either of the two

None of the two

## Questions 41 of 50

Question:The formation of $$N{O_2}$$ in the reaction $$2NO + {O_2}$$ $$\Leftrightarrow$$$$2N{O_2}$$+ heat is favoured by

Low pressure

High pressure

Low temperature

Reduction in the mass of

## Questions 42 of 50

Question:For the reaction $$PC{l_5}(g)$$ $$\Leftrightarrow$$ $$PC{l_3}(g) + C{l_2}(g)$$, the forward reaction at constant temperature is favoured by

Introducing an inert gas at constant volume

Introducing chlorine gas at constant volume

Introducing an inert gas at constant pressure

Decreasing the volume of the container

## Questions 43 of 50

Question:Which of the following conditions is favourable for the production of ammonia by Haber's process

High concentration of reactants

Low temperature and high pressure

Continuous removal of ammonia

All of these

## Questions 44 of 50

Question:Which of the following equilibria will shift to right side on increasing the temperature

$$C{O_{(g)}} + {H_2}{O_{(g)}}$$ $$\Leftrightarrow$$$$C{O_2}_{(g)} + {H_2}_{(g)}$$

$$2S{O_2}_{(g)} + {O_2}_{(g)}$$ $$\Leftrightarrow$$$$2S{O_3}_{(g)}$$

$${H_2}{O_{(g)}}$$ $$\Leftrightarrow$$$${H_2}_{(g)} + \frac{1}{2}{({O_2})_{(g)}}$$

$$4HC{l_{(g)}} + {O_2}_{(g)}$$ $$\Leftrightarrow$$$$2{H_2}{O_{(g)}} + 2C{l_2}_{(g)}$$

## Questions 45 of 50

Question:Sodium sulphate dissolves in water with evolution of heat. Consider a saturated solution of sodium sulphate. If the temperature is raised, then according to Le-Chatelier principle

More solid will dissolve

Some solid will precipitate out from the solution

The solution will become supersaturated

Solution concentration will remain unchanged

## Questions 46 of 50

Question:Consider the equilibrium $${N_2}(g) + 3{H_2}(g)$$ $$\Leftrightarrow$$$$2N{H_3}(g)$$; $$\Delta$$H = – 93.6 KJ. The maximum yield of ammonia is obtained by

Decrease of temp. and increase of pressure

Increase of temp. and decrease of pressure

Decrease of both the temp. and pressure

Increase of both the temp. and pressure

## Questions 47 of 50

Question:In the equilibrium $$AB$$ $$\Leftrightarrow$$$$A + B$$; if the equilibrium concentration of A is doubled, the equilibrium concentration of B would become:

Twice

Half

1/4th

1/8th

## Questions 48 of 50

Question:The reaction $$2S{O_2} + {O_2}$$ $$\Leftrightarrow$$$$2S{O_3}$$; $$\Delta H$$ = – ve is favoured by

Low temperature, low pressure

Low temperature, high pressure

High temperature, high pressure

High temperature, low pressure

## Questions 49 of 50

Question:Which of the following will favour the reverse reaction in a chemical equilibrium

Increasing the concentration of the reactants

Removal of at least one of the products at regular intervals

Increasing the concentration of one or more of the products

Increasing the pressure

None of these

## Questions 50 of 50

Question:Under what conditions of temperature and pressure the formation of atomic hydrogen from molecular hydrogen will be favoured most