Observe the following reaction, 2 A + B → C The rate of formation of C is 2.2 × 10 - 3 mol L -1 mtextn -1 , then rate of disappearance of A is

2 A + B → C Rate of reaction, = - 1 2 d A d t = - d B d t = d C d t ∴ - d A d t = 2 d [ C ] d t = 2 × 2.2 × 10 - 3 = 4.4 × 10 - 3 m o l L - 1 m i n - 1

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ChemistryChemical KineticsRate of Reactions/Rate LawEasy2 minPYQ_2020

ChemistryEasysingle choice

Observe the following reaction,

$2 A + B \to C$

The rate of formation of C is $2.2 \times 10^{- 3}$ mol L^-1mtextn^-1, then rate of disappearance of A is

Options:

Answer:

Solution:

$2 A + B \to C$

Rate of reaction,

$= - \frac{1}{2} \frac{d [A]}{d t} = - \frac{d [B]}{d t} = \frac{d [C]}{d t}$

$∴ - \frac{d [A]}{d t} = 2 \frac{d [C]}{d t}$

$= 2 \times 2.2 \times 10^{- 3}$

$= 4.4 \times 10^{- 3} m o l L^{- 1} {m i n}^{- 1}$

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

⏱ 2mℹ️ Source: PYQ_2020

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