Question # 1

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Favour the formation of N₂O₄

Favour the decomposition of N₂O₄

Not alter the equilibrium

Stop the reaction

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K_p> K_c

K_c> K_p

K_p= K_c

None of these

The ph of 10-3 mole dm-3 of an aqueous solution of H₂SO₄ is :

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3.0

2.7

2.0

1.5

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

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32

64

16

4

ph of the buffer CH₃COOh + CH₃COONa is 3.76. If the mixture contains 1 molar acetic acid and 0.1 molar sodium acetate, then pKa of this buffer is

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3.76

4.76

5.76

6.76

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

K_bvalue of NH₄OH is 1.81 x 10^-5and its conjugate acid has K_a= 5.7 x 10^-10pKb of the base is 4.74, pKa of its conjugate acid is

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-4.74

4.74

10

9.26

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

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2

1

5

0.25

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

In a lime kiln, to get higher yield of CO₂, the measure that can be taken is

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To main high temperature

To pump out CO₂

To remove Cao

To add more CaCO₃

A gas bulb is filled with NO₂gas and immersed in an ice bath at 0°C which becomes colourless after sometimes. This colourless gas will be

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NO₂

N₂O

N₂O₄

N₂O₅

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Moles per dm³

Partial pressures

Number of moles

Mole fractions

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Initial concentration of acetic acid

Initial concentration of ethyl acetate

Equilibrium concentration of acetic acid

Equilibrium concentration of ethyl acetate

The solubility product of AgCl is 2.0 x 10^-3 mol² dm^-6 , The maximum concentration of Ag ion in the solution is :

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2.0 x 10^-10 mol dm^-3

1.41 x 10^-10 mol dm^-3

1.0x 10^-10 mol dm^-3

4.0x 10^-10 mol dm^-3

Base buffer solution can be prepared by mixing

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Weak acid and its salt

Strong acid and its salt with weak base

Weak base and its salt with strong acid

Strong base and its salt with weak acid

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.

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8

4

9

3

The substance which increases rate of reaction but remains unchanged at the end of reaction is called :

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Catalyst.

Indicator.

Promoter.

Activator.

For what value ofK_{c almost forward reaction is complete :}

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K_{c =}10³⁰

K_{c =}10^-30

K_{c =}0

K_{c =}1

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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

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HF is stable and does not decompose even at 2000°C

HF is stable and slowly decomposes at 2000°C

HF is strong acid

HF produces equal moles of hydrogen and fluorine

The ionic product of H⁺ions and OH^-in water is called ionization constant of water Kw. The value of Kw at 25°C is

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0.11 x 10^-14

0.30 x 10^-14

1.0 x 10^-14

3 x 10^-14

Which statement about the following equilibrium in correct?

2SO_{2 (g)}+ O_2(g)---------------2sO_3(g)H= - 188.3 KJ mol-1

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T value of K_{p falls witha rise in temperate.}

The value of K_{p falls withincreasing pressure}

Adding V_2O₅catalyst increase the equilibrium yield of sulfur trioxide

The value of K_{p is equal to}K_p

The pH of 10^-3mole dm^-3of an aqueous solution of H₂SO₄is

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3.0

2.7

2.0

1.5

Hydrogen gas and iodine vapours combine to form Hl at 425°C, the same composition of mixture is present if we start with decomposition of Hl. It suggests

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A static equilibrium

Law of mass action

A dynamic equlibrium

Irreversible reaction

H₂+ L₂----2Hl

In the above equilibrium system, if the concentration of reactants at 25°C is increased, the value K_C will :

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Remains Constant

Increases

Cecreases

Depends upon nature of reactans

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

An excess of aqueous silver nitrate is added to aqueous barium chloride and precipitate is removed by filtration. What are the main ions in the filtrate

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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

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