A substance undergoes first order decomposition involving two parallel first order reactions as :

$k_{1} = 1.25 \times 10^{- 4} s^{- 1}$

$k_{2} = 3.80 \times 10^{- 5} s^{- 1}$

The mole percentage of $B$ in the products is :

Question

A substance undergoes first order decomposition involving two parallel first order reactions as : k 1 = 1.25 × 10 - 4 s - 1 k 2 = 3.80 × 10 - 5 s - 1 The mole percentage of B in the products is :

TestHub · Accepted Answer

mole % o f B = 12.5 × 1 0 - 5 12.5 + 3.8 × 1 0 - 5 × 100 = 12.5 16.3 × 100 = 76.68 %

Chemistry - Chemical Kinetics Question with Solution | TestHub

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