Question # 1

Which of the following in an example of reversible reaction

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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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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

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High temperature and low pressure

Low temperature and high pressure

Low temperature and low pressure

High temperature and high pressure

strength of an acid can be determined by

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P^ka

P^kp

P^oH

P^kw

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4 mole per dm³

2 mole per dm³

0.33 mole per dm³

0.67 mole per dm³

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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Low pressure

High pressure

High temperature

High concentration of SO₂

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

A large value of K_cmeans that at equilibrium :

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Less reactant and more products.

Reactants and product in same amounts.

More reactants and less products.

None of above.

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

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.

Law of mass action was given by :

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Guldberg and Waage.

Berkeley and Hartly.

Ramsay and Reyleigh.

Berthelot.

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1

10

5

0.33

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0.60

1.67

0.66

2.6

Which statement about the following equilibrium in correct?

2SO_{2 (g)}+ O_2(g)---------------2sO_3(g)H= - 188.3 KJ mol-1

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T value of K_{p falls witha rise in temperate.}

The value of K_{p falls withincreasing pressure}

Adding V_2O₅catalyst increase the equilibrium yield of sulfur trioxide

The value of K_{p is equal to}K_p

According to Le-Chatelier's principal, adding heat to a solid and liquid in equilibrium will cause the

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Amount of solid to decrease

Amount of liquid to decrease

Temperature to rise

Temperature to fall

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

For which system does the equilibrium constant, KC has units of concentration

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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

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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Increase in concentration of 1

Decrease in concentration of I₂

Increase in temperature

Increase in total pressure

K_bvalue of NH₄OH is 1.81 x 10^-5and its conjugate acid has K_a= 5.7 x 10^-10pKb of the base is 4.74, pKa of its conjugate acid is

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-4.74

4.74

10

9.26

pH of 0.1 molar HCl solution is

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1

zero

13

14

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

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12

14

zero

10

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

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

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Shift reaction toward forward direction

Shift reaction backward

Lower the value of K_c

No change in reaction

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[A] = [B]

[A] < [B]

[B] = [C]

[A] > [B]

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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

A buffer of a 0.09 molar acetic acid and 0.11 molar sodium acetate has pH = 4.83. If 0.01 mole NaOH in 1 dm³of the buffer solution is added, then pH of the buffer becomes

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4.74

4.92

5.0

4.0

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