What is the order of reaction $A + B \to C$?
Observation $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ Rate $(mol \ L^{-1} \ sec^{-1})$
$1$ $0.1$ $0.1$ $2 \times 10^{-3}$
$2$ $0.4$ $0.1$ $3.2 \times 10^{-3}$
$3$ $0.1$ $0.2$ $8 \times 10^{-3}$

  • A
    $1.5$
  • B
    $2.5$
  • C
    $3.0$
  • D
    $2.0$

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Similar Questions

For the decomposition of a compound $AB$ at $600 \ K$,the following data were obtained:
$[AB] \ (mol \ dm^{-3})$Rate of decomposition of $AB \ (mol \ dm^{-3} \ s^{-1})$
$0.20$$2.75 \times 10^{-8}$
$0.40$$11.0 \times 10^{-8}$
$0.60$$24.75 \times 10^{-8}$

The order for the decomposition of $AB$ is:

For the reaction,$2N_2O_5 \to 4NO_2 + O_2$,the rate equation can be expressed in two ways $-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$ and $+\frac{d[NO_2]}{dt} = k'[N_2O_5]$. $k$ and $k'$ are related as:

Units of rate constant of first and zero order reactions in terms of molarity $M$ unit are respectively

The half-life period of a $second$ order reaction is:

Higher order $(> 3)$ reactions are rare due to:

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