Chemistry - Chemical Kinetics Question with Solution | TestHub

ChemistryChemical KineticsFirst Order ReactionsMedium2 minQB

ChemistryMediumsingle choice

Passage / Comprehension

For the following reaction, $2 A (g) + B (g) \to C (g)$ , the rate of reaction is $- \frac{d [ B ]}{d t} = k [A]$ . In an initial reaction mixture, the partial pressures of A and B are $2 a t m$ and $1 a t m$ respectively at $300 K$ . At $100 sec$ , the total pressure of the reaction mixture becomes $2 a t m$ at $300 K$ . ( $ln 2 = 0.693$ )

The rate constant (k) is

Options:

Answer:

Solution:

$t = 0 t = 100 s t = 200 s 2 A (g) 2 atm 1 atm 0.5 atm + 1 atm 0.5 atm B (g) \to C (g) 0 0.5 atm$

$k_{A} = 2 k = \frac{1}{100} ln \frac{2}{1}$

$k = \frac{l n 2}{200}$

Stream:JEESubject:ChemistryTopic:Chemical KineticsSubtopic:First Order Reactions

⏱ 2mℹ️ Source: QB

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