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

Units of Kw are

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Mole dm^-3

Mole²dm^-3

Mole²dm^-6

Mole²dm^-3

pH of 1 molar NaOH is

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7

zero

14

10

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0.073

0.147

0.05

0.026

The equilibrium constant in a reversible chemical reaction at a given temperature

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Depends on the initial concentration of the reactants

Depends on the concentration of one of the products at equilibrium

Does not depend on the initial concentration of rectants

It is characteristic of the reaction

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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Temperature is increased

Pressure is increased

HCl is added

HCl is removed

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The value of K_pfalls with rise in temperature

The value of K_pfalls with increasing pressure

Addition of V₂O₅catalyst increase the concentration of SO₃

The value of K_pis equal to K_c

For which system does the equilibrium constant. K_chas units of

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pH of 0.1 molar HCl solution is

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1

zero

13

14

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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8

4

9

3

Addition of solid NaHCO₃in water causes ionization of NaCHO₃its K_a= 4.7 x 10^-1. Then this solution has character

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Acidic

Very weakly basic

Alkaline

Neutral

The avtive mass of 64 g of HI in a two litre flask would be

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2

1

5

0.25

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

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Shift reaction toward forward direction

Shift reaction backward

Lower the value of K_c

No change in reaction

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

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Remains unchanged.

Product side.

Reactant side.

None of above.

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

The relation between Kc and Kp is

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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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Initial concentration of acetic acid

Initial concentration of ethyl acetate

Equilibrium concentration of acetic acid

Equilibrium concentration of ethyl acetate

1.1 mol of A is mixed with 2.2 mol of B and the mixture is kept in on litre flask till the equilibrium is reached. At equilibrium, 0.2 mol of C is formed. If the equilibrium reaction is A+2B 2C+D, the value of equilibrium constant is

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0.002

0.004

0.001

0.003

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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

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Forward reaction is favoured

Backward reaction is favoured

No effect

None of the above

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Reaction occurs at STP

Reaction is exothermic

Reaction is endothermic

Number of moles of production and reactant are same

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

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

On passing HCI gas through a saturated solution of commercial sodium chloride, pure crystals of NaCI are precipitated due to

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Increase in pH of the solution

Decrease in pH of the solution

Common ion effect

Increase in ionization of NaCl

For what value ofK_{c almost forward reaction is complete :}

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K_{c =}10³⁰

K_{c =}10^-30

K_{c =}0

K_{c =}1

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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Increases

Decreases

Remains same

Cannot be predicted

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