Question # 1

N₂ + O₂ ⇌2NO

The unit of K_c for tis reaction will be:

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No unit

mol^-2 dm^-3

mol^-1 dm^-3

mol^-2 dm⁺³

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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450°C

250°C

850°C

1000°C

The best buffer is prepared when molar concentrations of the salt and acid are equal, then its pH and pKa value are related

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pH = pKa

pH < pKa

pH > pKa

pH x pKa = 14

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

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3.0

2.7

2.0

1.5

The state of equilibrium refers to

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State of rest

Dynamic state

Stationary state

State of inertness

The rate of reaction :

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Remain same as reaction proceeds.

May decrease or increase as reaction proceeds .

Increase as reaction proceeds.

Decreases as reaction proceeds.

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

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

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.

The solubility of KCIO₃salt in water is decreased by adding

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NaCIO₃

NaCI

KCIO₄

KCI

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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Whenever a week base is dissolved in water, it give its conjugate acid. similarly a weak acid in water produces its conjugate base. This conjugate acid-base pair concept is stated by

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Law of mass action

Le-charlier's principle

Common ion effect

Lowery Bronsted concept

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KC = KP

Kp = KcRT

Kp = kc(RT)^-2

Kp = Kc(RT)^-1

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

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

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

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Reaction occurs at STP

Reaction is exothermic

Reaction is endothermic

Number of moles of production and reactant are same

The rate of which the reaction proceeds is directly proportional to the product of the active masses of the reactants is according to

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Law of mass action

Le Chateliers principle

Equilibrium law

Law of constant proportion

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Moles per dm³

Partial pressures

Number of moles

Mole fractions

The correct relation b/wK_{c and}K_{p is :}

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K_p = K_c[P/N] ^Δn

K_{c =}K_p(RT) ^Δn

K_{p =}K_c(RT) ^Δn

N₂ + 3H₂ ⇌2NH₃

The unit of K_c for tis reaction will be:

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mol² dm^-6

mol^-2 dm⁺⁶

mol dm^-3

mol^-1 dm⁺³

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0.5

4.0

2.5

0.25

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Total pressure

Amount of A₂and B₂

Temperature

Catalyst

pH of the human blood which is essentially maintained constant due to carbonates, biocarbonates, phosphates etc., is

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7.00

7.25

7.35

7.47

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High temperature and low pressure

Low temperature and low pressure

Low temperature and high pressure

High temperature and high pressure

A buffer solution of 0.1 molar HCOOH and 0.1 molar HCCONa has pH = 3.78 To is 0.01 molar HCl is added, then pH of the buffer solution becomes

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2.78

4.78

3.78

3.70

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

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

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