(D) The rate of formation of $B$ is given by the expression:$\frac{d[B]}{dt} = K_1[A] - K_2[B]$According to the steady-state approximation,the rate of

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(D) The rate of formation of $B$ is given by the expression:$\frac{d[B]}{dt} = K_1[A] - K_2[B]$According to the steady-state approximation,the rate of formation of $B$ is set to zero:$0 = K_1[A] - K_2[B]$Rearranging the equation to solve for $[B]$:$K_2[B] = K_1[A]$$[B] = \frac{K_1}{K_2}[A]$

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

Medium

For a reaction $A$ $\xrightarrow{K_1} B$ $\xrightarrow{K_2} C$. If the rate of formation of $B$ is set to be zero,then the concentration of $B$ is given by:

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A
$K_1 K_2[A]$
B
$(K_1 - K_2)[A]$
C
$(K_1 + K_2)[A]$
D
$(K_1 / K_2)[A]$

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Class 12

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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For a reaction $A$ $\xrightarrow{K_1} B$ $\xrightarrow{K_2} C$. If the rate of formation of $B$ is set to be zero,then the concentration of $B$ is given by:

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