(B) The general rate law is given by: $\text{Rate} = K[A]^x[B]^y$. When the concentration of $A$ is doubled,the rate increases by $4$ times $(2^2 = 4)

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(B) The general rate law is given by: $\text{Rate} = K[A]^x[B]^y$. When the concentration of $A$ is doubled,the rate increases by $4$ times $(2^2 = 4)$,which implies the order with respect to $A$ is $x = 2$. When the concentration of $B$ is doubled,the rate remains unchanged,which implies the order with respect to $B$ is $y = 0$. Substituting these values into the rate law: $\text{Rate} = K[A]^2[B]^0 = K[A]^2$.

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

Medium

For the reaction $A + B \rightarrow$ products,doubling the concentration of $A$ increases the reaction rate by four times,but doubling the concentration of $B$ has no effect on the reaction rate. What is the rate law?

A
Rate $= K[A][B]$
B
Rate $= K[A]^2$
C
Rate $= K[A]^2[B]$
D
Rate $= K[A]^2[B]^2$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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For the reaction $A + B \rightarrow$ products,doubling the concentration of $A$ increases the reaction rate by four times,but doubling the concentration of $B$ has no effect on the reaction rate. What is the rate law?

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For the following reaction: $NO_{2(g)} + CO_{(g)} \to NO_{(g)} + CO_{2(g)}$,the rate law is: $\text{Rate} = k [NO_2]^2$. If $0.1 \ mol$ of gaseous carbon monoxide is added at constant temperature to the reaction mixture,which of the following statements is true?

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