(A) The given reaction is $2 \ NOBr_{(g)} \rightarrow 2 \ NO_{(g)} + Br_{2_{(g)}}$.Given: $k = 1.62 \ M^{-1} \ s^{-1}$ and $[NOBr] = 2.00 \times 10^{-

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$6.48 \times 10^{-6} \ M \ s^{-1}$

(A) The given reaction is $2 \ NOBr_{(g)} \rightarrow 2 \ NO_{(g)} + Br_{2_{(g)}}$.Given: $k = 1.62 \ M^{-1} \ s^{-1}$ and $[NOBr] = 2.00 \times 10^{-3} \ M$.The rate law is $r = k[NOBr]^{2}$.Substituting the values:$r = 1.62 \ M^{-1} \ s^{-1} \times (2.00 \times 10^{-3} \ M)^{2}$$r = 1.62 \times 4.00 \times 10^{-6} \ M \ s^{-1}$$r = 6.48 \times 10^{-6} \ M \ s^{-1}$.

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

Medium

For the reaction $2 \ NOBr_{(g)} \rightarrow 2 \ NO_{(g)} + Br_{2_{(g)}}$,the rate law is $r = k[NOBr]^{2}$. If the rate constant is $1.62 \ M^{-1} \ s^{-1}$ and the concentration of $NOBr$ is $2.00 \times 10^{-3} \ M$,what is the rate of reaction?

MHT CET 2020 All MHT CET

A
$6.48 \times 10^{-6} \ M \ s^{-1}$
B
$4.05 \times 10^{-5} \ M \ s^{-1}$
C
$2.46 \times 10^{-6} \ M \ s^{-1}$
D
$5.24 \times 10^{-6} \ M \ s^{-1}$

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Rate law , Rate constant , Order of Reaction and Molecularity

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For the reaction $2 \ NOBr_{(g)} \rightarrow 2 \ NO_{(g)} + Br_{2_{(g)}}$,the rate law is $r = k[NOBr]^{2}$. If the rate constant is $1.62 \ M^{-1} \ s^{-1}$ and the concentration of $NOBr$ is $2.00 \times 10^{-3} \ M$,what is the rate of reaction?

Similar Questions

How can you determine the rate law of the following reaction?$2 \, NO \, (g) + O_2 \, (g) \to 2 \, NO_2 \, (g)$

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How can you determine the rate law of the following reaction?
$2 \, NO \, (g) + O_2 \, (g) \to 2 \, NO_2 \, (g)$

The rate law for the reaction below is given by the expression $Rate = k[A][B]$.
$A + B \to \text{Product}$
If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be: