A substance undergoes first order decomposition. The decomposition follows the parallel first order reaction as. The percentage distribution of B and C is

76.83, 23.17

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24.9, 75.1

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60, 40

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50, 50

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Solution

The correct option is C $76.83, 23.17$
At any time t
Rate of formation of $B \Rightarrow C_{B} = k_{1} C_{A}$
Rate of formation of $C \Rightarrow C_{C} = k_{2} C_{A}$
$∴ \frac{C_{B}}{C_{C}} = \frac{k_{1}}{k_{2}} = \frac{1.26 \times 10^{- 4}}{3.8 \times 10^{- 5}}$
% $C_{B} = \frac{C_{B}}{C_{B} + C_{C}} \times 100 = \frac{1.26 \times 10^{- 4}}{(1.26 \times 10^{- 4} + 3.8 \times 10^{- 5}) \times 100} = 76.83$
% $C_{C} = 100 - C_{B} = 100 - 76.83 = 23.17$

Suggest Corrections

Similar questions

K_{1} = 1.26 \times 10^{- 4} s e c^{- 1}

K_{2} = 3.8 \times 10^{- 5} s e c^{- 1}

K_{1} : K_{2} = 1 : 2

B

C

A

k_{1} = 1.28 \times 10^{- 4} {s e c}^{- 1}

k_{2} = 3.2 \times 10^{- 5} {s e c}^{- 1}

B

C

A substance undergoes first order decomposition. The decomposition follows two parallel first order reactions as:

The percentage distribution of B and C are:

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