For the given reaction 2 N 2 O 5 → 4 N O 2 + O 2 , the rate of reaction and rate constant values are 1.02 × 1 0 - 4 and 3.4 × 1 0 - 5 se c - 1 respectively. Then calculate the concentration of N 2 O 5 at that time

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ChemistryChemical KineticsMiscellaneous/MixedEasy2 minPYQ_2020

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For the given reaction $2 N_{2} O_{5} \to 4 N O_{2} + O_{2}$ , the rate of reaction and rate constant values are $1.02 \times 1 0^{- 4}$ and $3.4 \times 1 0^{- 5} se c^{- 1}$ respectively. Then calculate the concentration of $N_{2} O_{5}$ at that time

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Answer:

Solution:

The unit of rate constant suggest that it is a first order reaction. Hence the given rate law is $R = K [A]$ , $1.02 \times 1 0^{- 4} = 3.4 \times 1 0^{- 5} \times [N_{2} O_{5}]$

or $(N_{2} O_{5}) = \frac{1.02 \times 1 0^{- 4}}{3.4 \times 1 0^{- 5}} = 3$

Stream:NTA_ABHYASSubject:ChemistryTopic:Chemical KineticsSubtopic:Miscellaneous/Mixed

⏱ 2mℹ️ Source: PYQ_2020

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