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 V₂O₅catalyst increase the equilibrium yield of Sulphur trioxide.

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Reversible reaction

Irreversible reaction

Spontaneous reaction

None of these

A solution having pH = 4 its OH^-ion concentration in mole dm^-3is

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1.0 x 10^-4

1.0 x 10^-10

1.0 x 10^-14

1 x 10⁰

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Le-chatlier's principle

Only adding catalyst

Decreasing pressure

Decreasing temperature

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Forward

Backward

Already in equilibrium

K_cis never less

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

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Low pressure

High pressure

High temperature

High concentration of SO₂

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[A] = [B]

[A] < [B]

[B] = [C]

[A] > [B]

A large value of K_cmeans that at equilibrium :

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Less reactant and more products.

Reactants and product in same amounts.

More reactants and less products.

None of above.

K_spvalue for PbSO₄= 1.8 x 10^-8mole²dm^-6. The maximum concentration of Pb⁺⁺ions is

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1.34 x 10^-4mole dm^-3

1.8 x 10^-4

3.6 x 10^-16mole dm^-3

1.0 x 10^-8mole dm^-3

When a weak acid is dissolved in water or a weak base dissolved in water, then in both cases the conjugate acid base pair is produced. The ionization constants K_aand K_bof a pair are related with each other as

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K_a= K_b

K_a. K_b= K_w

K_a. K_w= K_b

K_b. K_w= K_a

If pH of buffer of 1 mole dm^-3of HCOOH + 0.1 mole dm^-3HCOONa having pKa = 3.78 is

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1.78

2.78

3.78

4.78

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Increase in concentration of 1

Decrease in concentration of I₂

Increase in temperature

Increase in total pressure

What happens when reaction is at equilibrium and more reactant is added :

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Forward reaction rate is increased.

Forward reaction rate is decreased.

Backward reaction rate is increased.

Equilibrium remains unchanged.

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

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Ag⁺ and NO_3- only

Ag⁺ and Ba² and NO^-3

Ba² and NO^-3

Ba² and NO^-3and Cl-

In exothermic reversible reaction increase in temperature shift the equilibrium to :

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Remains unchanged.

Product side.

Reactant side.

None of above.

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

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3.0

2.7

2.0

1.5

K_avalue of HF acid is 6.7 x 10^-15the acid is a

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Weak acid

Moderately strong acid

Strong acid

Very weak acid

A reaction is reversible because :

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Products are stable.

Reactants are reactive.

Products are reactive.

Reactants re stable.

Product of concentration of ions raised to the power equal to the co-efficient of ions in balanced equation for saturated solution of a salt is called

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Ionic product

Equilibrium constant K_c

K_w

Solubility product (K_sp)

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0.02

0.2

50

25

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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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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

The value of K_pis greater than K_cfor a gaseous reaction when

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Number of molecules of products is greater than the reactants

Number of molecules of reactants is greater than those of products

Number of molecules of reactants and products equal

Catalyst is added

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.

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KC = KP

Kp = KcRT

Kp = kc(RT)^-2

Kp = Kc(RT)^-1

The rate of a chemical reaction is directly;y proportional to product of molar concentration of reaction substance it is called :

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Low of conservation of energy.

Law of mass action.

Rate law .

Active mass rule.

Under what condition of temperature and pressure the formation of atomic hydrogen from molecular hydrogen will be favourd

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High temperature and high pressure

Low temperature and low pressure

High temperature and low pressure

:Low temperature and high pressure

Units of Kw are

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Mole dm^-3

Mole²dm^-3

Mole²dm^-6

Mole²dm^-3

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4 mole per dm³

2 mole per dm³

0.33 mole per dm³

0.67 mole per dm³

For which system does the equilibrium constant. K_chas units of

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