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ChemistryChemical KineticsRate of Reactions/Rate LawMedium2 minPYQ_2023

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The rate for reaction $A + B \to$ product, is $1.8 \times 1 0^{- 2} mol dm^{- 3} s^{- 1}$ . Calculate the rate constant if the reaction is second order in $A$ and first order in $B . ([A] = 0.2 M; [B] = 0.1 M)$

Options:

Answer:

Solution:

Rate $= k [A]^{2} [B]$ $∴ k k = \frac{rate}{[ A ] ^{2} [ B ]} = \frac{1.8 \times 1 0 ^{- 2} moldm ^{- 5} s ^{- 1}}{( 0.2 moldm ^{- 3} ) ^{2} \times 0.1 moldm ^{- 3}} = 4.5 mol^{- 2} dm^{6} s^{- 1}$

Stream:MHT_CETSubject:ChemistryTopic:Chemical KineticsSubtopic:Rate of Reactions/Rate Law

⏱ 2mℹ️ Source: PYQ_2023

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