Question # 1

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

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Favour the formation of N₂O₄

Favour the decomposition of N₂O₄

Not alter the equilibrium

Stop 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

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Moles^-2dm⁺⁶

No units

Mole dm^-3

Mole^-1dm^-3

Extent to H₂ + L₂à2Hl can be increased by :

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Increasing temperature.

Increasing product.

Increasing pressure.

Adding a catalyst.

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

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Almost forward reaction is complete when value of k_{c :}

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Neither larger nor very small.

Very small.

Very large.

Negligible.

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0.5

4.0

2.5

0.25

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Reversible reaction

Irreversible reaction

Spontaneous reaction

None of these

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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

1 mol of N₂O₄ was decomposed according to given equation in 1dm₃ container. At equilibrium x mole of N₂O₄ have dissociated. What is the value of K_C:

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2x/(1-x)²

4x²/(1-x)

4x/(1-x)

2x/(1-x)

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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

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

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

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8

4

9

3

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Complete conversion of A to B has taken place

Conversion of A to B is only 50% complete

Only 10% conversion of A to B has taken place

The rate of transformation of A to B is just equal to rate of transformation of B to A in the system

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%

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

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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Reaction occurs at STP

Reaction is exothermic

Reaction is endothermic

Number of moles of production and reactant are same

The solubility of KCIO₃salt in water is decreased by adding

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NaCIO₃

NaCI

KCIO₄

KCI

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.

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0.073

0.147

0.05

0.026

The ionization constant of an acid is expressed in term of the following constant

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Kw

Kn

Ka

Kb

1 mole of N₂and 2 moles of H₂are allowed to react in a 1 dm³vessel. At equilibrium 0.8 mole of NH₃is formed. The concentration of H₂in the vessel is

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0.6 mole

0.8 mole

0.2 mole

0.4 mole

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

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

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3.0

2.7

2.0

1.5

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

Which one of the following is a buffer

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HCI + NaCI solution

CH₃COOH + CH₃COONH₄solution

H₂SO₄+ CaSO₄solution

CH₃COOH + CH₃COONa

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

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Remains unchanged.

Product side.

Reactant side.

None of above.

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