Question # 1

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

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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

Extent to H₂ + L₂à2Hl can be increased by :

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Increasing temperature.

Increasing product.

Increasing pressure.

Adding a catalyst.

Reactions that proceed on both sides and never go to completion are called

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Irreversible reactions

Reversible reactions

Opposing reactions

Spontaneous reactions

For the above reaction the relationship b/w k_c and k_p will be :

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K_p = K_cRT

Kp = K_c(RT)_-1

K_p = K_c(RT)_-2

K_c = K_p

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Forward

Backward

Already in equilibrium

K_cis never less

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

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0.02

0.2

50

25

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Initial concentration of acetic acid

Initial concentration of ethyl acetate

Equilibrium concentration of acetic acid

Equilibrium concentration of ethyl acetate

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)

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

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0.12

0.50

0.25

4.00

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Increases

Decreases

Remains same

Cannot be predicted

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

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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The solubility of PbF₂is 2.6 x 10^-3mole dm^-3then its solubility product is

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2.6 x 10^-3

6.76 x 10^-6

5.2 x 10^-6

7.0 x 10^-8

Ammonium carbonate when heated to 200°C gives a mixture of NH₃and CO₂vapour with a density of 13.0. What is the degree of dissociation of ammonia carbonate?

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3/2

1/2

2

1

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Forward reaction is favoured

Backward reaction is favoured

No effect

None of the above

Which one of the following is a buffer

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HCI + NaCI solution

CH₃COOH + CH₃COONH₄solution

H₂SO₄+ CaSO₄solution

CH₃COOH + CH₃COONa

N₂O₄⇌ 2NO₂

For the above reaction, which of the Following expression of K_c correct :

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Kc = [ N₂O₄]/[ NO₂]²

Kc = [ N₂O₄]/ [NO₂]

Kc = [ N₂O]²/[ N₂O₄]

Kc = [ N₂O₄]/[ N O₂]

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Total pressure

Amount of A₂and B₂

Temperature

Catalyst

When H₂and I₂are mixed and equilibrium is attained, then

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Amount of HI formed is equal to the amount of H₂dissociated

HI dissociation stops

The reaction stops completely

None of these

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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Chemical equilibrium involving reactants and products in more than one phase is called

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Static

Dynamic

Homogeneous

Heterogeneous

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4 mole per dm³

2 mole per dm³

0.33 mole per dm³

0.67 mole per dm³

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.

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 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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KC = KP

Kp = KcRT

Kp = kc(RT)^-2

Kp = Kc(RT)^-1

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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