According to the collision theory of chemical reactions:

  • A
    $A$ chemical reaction occurs with every molecular collision.
  • B
    Rate is directly proportional to the number of collisions per second.
  • C
    Reactions in the gas phase are always of zero order.
  • D
    Reaction rates are of the order of molecular speeds.

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The rate constant of a reaction is $2 \times 10^{-3} \ min^{-1}$ at $300 \ K$. When the temperature is increased by $20 \ K$,the rate constant becomes three times its initial value. Calculate the activation energy $(E_a)$ of the reaction. Also,determine the rate constant at $310 \ K$.

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For an endothermic reaction $X \rightarrow Y$,the activation energies for the forward and backward reactions are $E_f$ and $E_b$ respectively. Then,in general:

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