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Common Ion Effect

The instantan...

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The instantanous rate of Dissaperance MnO4- ion in the following reaction is 4.56 x 10^-3 ms 2 MnO^-4 + 10 I^- + 16H^+ gives 2Mn^+2 + 5 I2 + 8H2O The rate of apperance of I2 is (a) 1.14 x 10^-3 (b) 5.7×10^-3 (c) 4.56x10^-4 (d) 1. 14x10^-2

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Q. The instantaneous rate of disappearance of the

M n O_{4}^{-}

ion in the following reaction is

4.56 \times 10^{- 3} M s^{- 1}

2 M n O_{4}^{-} + 10 I^{-} + 16 H^{+} \to 2 M n^{2 +} + 5 I_{2} + 8 H_{2} O

The rate of appearance of

I_{2}

Q. For the reaction

C l_{2} + 2 I^{-} \to I_{2} + 2 C l^{-}

, the initial concentration of

I^{-}

L^{- 1}

and the concentration after 20 min was 0.18 mol

L^{- 1}

. The rate of formation of l2 in mol

L^{- 1} m i n^{- 1}

Q. In a reaction;

H_{2} + I_{2} \to 2 H I

, the rate of dissappearance of

I_{2}

10^{- 6} m o l l i t r e^{- 1} s e c^{- 1}

. If the corresponding rate of appearance of HI is

x \times 10^{- 6} m o l l i t r e^{- 1} s e c^{- 1}

x

Q. The rate of the reaction

H_{2} + I_{2} ⇌ 2 H I

r a t e = 1.7 \times 10^{- 19} [H_{2}] [I_{2}]

25^{\circ} C

The rate of decomposition of gaseous

H I

H_{2}

I_{2}

r a t e = 2.4 \times 10^{- 21} [H I]^{2}

25^{\circ} C

.
Calculate the equilibrium constant for the formation of

H I

H_{2}

I_{2}

25^{\circ} C

Q. The following data pertains to the reaction between A and B:

S. No	[A]	[B]	Rate
$1$	$1 \times 10^{- 2}$	$2 \times 10^{- 2}$	$2 \times 10^{- 4}$
$2$	$2 \times 10^{- 2}$	$2 \times 10^{- 2}$	$4 \times 10^{- 4}$
$3$	$2 \times 10^{- 2}$	$4 \times 10^{- 2}$	$8 \times 10^{- 4}$

Which of the following inferences can be drawn from the above data?

1.

Rate law of the reaction is

K [A] [B]

.

2.

Rate constant of the reaction is

10^{- 4}

.

3.

Rate of reaction increases four times by doubling the concentration of each reactant.

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