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 Multiple Choice QuestionsMultiple Choice Questions

1.

The equilibrium constant at 298 K for a reaction A+B ⇌ C+D is 100. If the initial concentration of all the four species were 1 M each, then equilibrium concentration of D (in mol L−1 ) will be:

  • 0.818

  • 1.818

  • 1.182

  • 1.182

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2.

For the reaction,

SO subscript 2 space left parenthesis straight g right parenthesis space plus space 1 half space straight O subscript 2 space left parenthesis straight g right parenthesis space leftwards harpoon over rightwards harpoon space SO subscript 3 space left parenthesis straight g right parenthesis
if Kp = Kc (RT)x where the symbol has usual meaning then the value of x is (assuming ideality)

  • -1

  • -1/2

  • 1/2

  • 1/2


B.

-1/2

For  the given reaction, ∆ng = np-nR
where np = number of moles of products
nR = number of moles of reactants
Kp = Kc (RT)∆ng

∆ng = -1/2

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3.

The species which can best serve as an initiator for the cationic polymerization is

  • LiAlH4

  • HNO3

  • AlCl3

  • AlCl3

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4.

The equilibrium constant (Kc) for the reaction, N2(g) + O2 (g) → 2NO (g) at temperature T is 4 x 10-4. The value of Kc for the reaction NO space left parenthesis straight g right parenthesis space rightwards arrow 1 half space straight N subscript 2 space left parenthesis straight g right parenthesis space plus 1 half straight O subscript 2 space left parenthesis straight g right parenthesis at the same temperature is

  • 0.02

  • 2.5 x 102

  • 4 x 10-4

  • 4 x 10-4

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5.

The pH of a 0.1 molar solution of the acid HQ is 3. The value of the ionisation constant, Ka of this acid is

  • 3 x 10–1

  • 1 x 10–3

  • 1 x 10—5

  • 1 x 10—5

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6.

Consider the reaction:
Cl2(aq) + H2S(aq) → S (s) + 2H+ (aq) + 2Cl- (aq)
The rate equation for this reaction is
I. Cl2 + H2S → H+ +Cl- + Cl+ +HS-
II. H2S ⇌ H+ + HS- (fast equilibrium)
Cl2 + HS- → 2Cl- + H+ + S (slow)

  • II only

  • Both (I) and (II)

  • Neither (I) nor (II)

  • Neither (I) nor (II)

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7.

Three reactions involving H2PO4- are given below
I. H3PO4 + H2O → H3O+ + H2PO4-
II. H2PO4- + H2O→ HPO42- + H3O+
III. H2PO4- + OH- → H3PO4  + O2-
In which of the above does H2PO4- act  as an acid

  • (II) only

  • (I) and (II)

  • (III) only

  • (III) only

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8.

In aqueous solution the ionization constants for carbonic acid are
K1 = 4.2 x 10-7 and K2 = 4.8 x 10-11.
Select the correct statement for a saturated 0.034 M solution of the carbonic acid.

  • The concentration of CO32- is 0.034 M

  • The concentration of CO32- is greater than that of HCO3-

  • The concentration of H+ and HCO3- are approximately equal

  • The concentration of H+ and HCO3- are approximately equal

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9.

The correct order of increasing basicity of the given conjugate bases (R = CH3) is

  • RCO straight O with minus on top space less than space HC space identical to space straight C with minus on top space less than thin space straight N with minus on top straight H subscript 2 space less than straight R with minus on top
  • RCO straight O with minus on top space less than thin space HC space identical to straight C with minus on top space less than space thin space straight R with minus on top less than space straight N with minus on top straight H subscript 2
  • straight R with minus on top space less than HC space identical to space straight C with minus on top space less than space RCO straight O with minus on top space less than space straight N with minus on top straight H subscript 2
  • straight R with minus on top space less than HC space identical to space straight C with minus on top space less than space RCO straight O with minus on top space less than space straight N with minus on top straight H subscript 2
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10.

At 25°C, the solubility product of Mg(OH)2 is 1.0 × 10–11. At which pH, will Mg2+ ions start precipitating in the form of Mg(OH)2 from a solution of 0.001 M Mg2+ ions?

  • 9

  • 10

  • 11

  • 11

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