Which one of the following statements regarding the order of a reaction is not correct?

  • A
    Order is determined experimentally.
  • B
    Order of reaction is equal to the sum of powers of concentration terms in the experimental rate law.
  • C
    It is not affected by the stoichiometric coefficients of the reactants.
  • D
    Order cannot be fractional.

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Considering the reaction $aG + bH \rightarrow \text{Products}$,when the concentrations of both reactants $G$ and $H$ are doubled,the rate increases by $8$ times. However,when the concentration of $G$ is doubled while the concentration of $H$ remains constant,the rate doubles. What is the overall order of the reaction?

For the reaction,$CH_3Br_{(aq)} + OH_{(aq)}^{-} \rightarrow CH_3OH_{(aq)} + Br_{(aq)}^{-}$,the rate law is $\text{rate} = k[CH_3Br][OH^{-}]$. What is the change in the rate of reaction if the concentration of both reactants is doubled?

The rate law for the reaction between substances $A$ and $B$ is given by $\text{Rate} = k[A]^n[B]^m$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,what is the ratio of the new rate to the initial rate?

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The order of a reaction with rate equals $k[C_A]^{3/2} [C_B]^{-1/2}$ is

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