Question # 1

2SO₂ + O₂ ⇌ 2SO₂H= 188KJ mole^-1

Which statement about following equilibrium is correct :

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The value ofK_pfalls with arise in temperature.

The value ofK_pis equal tok_c.

The value ofK_pfalls with the increase pressure.

Adding V₂O₅ catalyst increase the equilibrium yield of Sulphur trioxide.

At certain temperature, 50% of HI is dissociated into H₂and I₂the equilibrium constant is

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1.0

3.0

0.5

0.25

In a reversible chemical reaction having two reactants in equilibrium, if the concentration of the reactants are doubled then the equilibrium constant will

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Also be doubled

Be halved

Becomes one fourth

Remains the same

Which of the following is a characteristic of a reversible reaction?

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It never proceeds to completion

It can be influenced by a catalyst

It proceeds only in the forward direction

Number of moles of reactants and products are equal

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Introduction of an inert gas at constant volume

Introduction of PCl₃(g) at constant

Introduction of PCl₅(g) at constant volume

Introduction of Cl₂at constant volume

The solubility product of AgCl is 2.0 x 10^-10mol²dm^-6The maximum concentration of Ag⁺ions in the solution is

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2.0 x 10^-10mol dm^-3

1.41 x 10^-5mol dm^-3

1.0 x 10^-10mol dm^-3

4.0 x 10^-20mol dm^-3

pKb value of NH₄OH is 4.74. If the concentration of NH₄OH is 1 molar containing 0.1 molar NH₄Cl, then pH of this buffer will be

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3.74

10.26

4.74

9.26

The concentration of reactants is increased by x, then equilibrium constant K becomes

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ln K/x

K/x

K + x

K

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Increase in concentration of 1

Decrease in concentration of I₂

Increase in temperature

Increase in total pressure

Which one of the following is not a buffer

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H₂CO₃+ NaHCO₃solution

H₃PO₄+ NaH₂PO₄solution

Hl + Nal solution

NH₄OH + NH₄CI solution

The optimum conditions of temperature and pressure to get maximum NH₃form N₂and H₂gases is

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2000°C and 10 atmosphere

0°C and 1 atmosphere

400°C and 200-300 atmosphere

200°C and 100 atmosphere

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Pressure change

Temperature change

Concentration change

Catalyst

The equilibrium constant in a reversible chemical reaction at a given temperature

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Depends on the initial concentration of the reactants

Depends on the concentration of one of the products at equilibrium

Does not depend on the initial concentration of rectants

It is characteristic of the reaction

The avtive mass of 64 g of HI in a two litre flask would be

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2

1

5

0.25

The solubility product of Ca(OH)₂is 6.5 x 10^-6. The concentration of OH^-ions is

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1.175 x 10^-2

2.35 x 10^-2

3.25 x 10^-3

3.25 x 10^-4

N₂+3H₂⇌ 2NH_{3 + Heat for above equation, themaximum product will be obtained at :}

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Low temperature at high pressure.

High temperature and low pressure.

High temperature and high pressure.

Low temperature at low pressure.

When rate of forward reaction is equal to rate of backward reaction, then the equilibrium established is called

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Chemical equilibrium

Static equilibrium

Dynamic equilibrium

None of these

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Increases

Decreases

Remains same

Cannot be predicted

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Forward reaction is favoured

Backward reaction is favoured

No effect

None of the above

Which of the following favours the reverse reaction in chemical equilibrium?

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Increasing the concentration of the reactant

Removal of the least one of the products at regular intervals

Increasing the concentration of one or more of the products

None of these

For which system does the equilibrium constant, kc has units of (concentration) ?

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N₂+3H_2-------2NH₃

H₂+L₂---------2HL

2NO₂----------N₂O₄

2HF--------H2+F₂

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The value of K_pfalls with a rise in temperature

The value of K_pfalls with increasing pressure

Adding V₂O₅catalyst increase the equilibrium yield of sulphur trioxide equilibrium yield of sulphur trioxide

The value of K_pis equal to K_c

Extent to H₂ + L₂à2Hl can be increased by :

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Increasing temperature.

Increasing product.

Increasing pressure.

Adding a catalyst.

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[A] = [B]

[A] < [B]

[B] = [C]

[A] > [B]

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

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Increase in concentration of one of the reactants

Increase in concentration of one of the products

Removal of one of the products regularly

None of these

The solubility product of AgCl is 2.0 x 10^-10mole ²dm^-6. The maximum concentration of Ag⁺ions in the solution is

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2.0 x 10^-10mole dm^-3

1.41 x 10^-5mole dm^-3

1.0 x 10^-10

4.0 x 10^-20mole dm^-3

Buffers having pH less than 7 are made

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Mixture of weak acid + salt of it with strong base

Mixture of weak acid + salt of it with weak base

Mixture of weak base + salt of it with strong acid

Mixture of weak base + salt of it with weak base

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Forward

Backward

Already in equilibrium

K_cis never less

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High temperature and low pressure

Low temperature and low pressure

Low temperature and high pressure

High temperature and high pressure

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Low pressure

High pressure

High temperature

High concentration of SO₂

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