Question # 1

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4 mole per dm³

2 mole per dm³

0.33 mole per dm³

0.67 mole per dm³

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Total pressure

Amount of A₂and B₂

Temperature

Catalyst

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0.12

0.50

0.25

4.00

A reaction is reversible because :

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Products are stable.

Reactants are reactive.

Products are reactive.

Reactants re stable.

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450°C

250°C

850°C

1000°C

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Increase in concentration of 1

Decrease in concentration of I₂

Increase in temperature

Increase in total pressure

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

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Shift reaction toward forward direction

Shift reaction backward

Lower the value of K_c

No change in reaction

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.

In 1000 molecules of 0.001 M acetic acid the number of H⁺ions is 12.6, then its percentage of ionization is

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1.33%

1.26%

12.6

1%

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 one of the following is a buffer

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HCI + NaCI solution

CH₃COOH + CH₃COONH₄solution

H₂SO₄+ CaSO₄solution

CH₃COOH + CH₃COONa

pH of water is 7, if 0.01 M NaOH is added, than its pH is

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12

14

zero

10

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

I a chemical reaction equilibrium is said to have been established when :

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Rate of opposing reactions are equal.

Rate constants of opposing reactions are equal.

Opposing reactions stop.

Concentration of reactants and products are equal

Extent to H₂ + L₂à2Hl can be increased by :

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Increasing temperature.

Increasing product.

Increasing pressure.

Adding a catalyst.

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

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3.0

2.7

2.0

1.5

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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 rate of forward reaction is two times that of the reverse reaction at a given temperature and identical concentration, K equilibrium is

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0.5

1.5

2.5

2.0

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-

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Reversible reaction

Irreversible reaction

Spontaneous reaction

None of these

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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Equal volumes of N₂and H₂are reacting

Equal masses of N₂and H₂are reacting

The reaction has stopped

The same amount of ammonia is formed as is decomposed into N₂and H₂

A solution has pH = 0, its H⁺ion concentration is

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1 x 10^-14

1 x 10¹⁴

1 x 10¹

1

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

In which of the following cases, the reaction goes farthest to completion

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K = 10³

K = 10^-2

K = 10

K = 10⁰

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Low pressure

High pressure

High temperature

High concentration of SO₂

Units of Kw are

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Mole dm^-3

Mole²dm^-3

Mole²dm^-6

Mole²dm^-3

The state of equilibrium refers to

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State of rest

Dynamic state

Stationary state

State of inertness

pH and pKa of the buffer are related by Henderson equation which is

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