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For the reaction A+B\rightarrow products, it is observed that:

  1. On doubling the initial concentration of A only, the rate of reaction is also doubled and
  2. On doubling the initial concentrations of both A and B, there is a change by a factor of 8 in the rate of the reaction.

The rate of this reaction is given by:

  • Option 1)

    rate =k [A] [B]2

  • Option 2)

    rate =k [A]2 [B]2

  • Option 3)

    rate =k [A] [B]

  • Option 4)

    rate =k [A]2 [B]

 

Answers (1)

best_answer

As we learned in concept

Rate of Law = Dependence of Rate on Concentration -

The representation of rate of a reaction in terms of concentration of the reactants is known as Rate Law

or

The Rate Law is the expression in which reaction rate is given in terms of molar concentration of reactants with each term raised to some power, which may/maynot be equal to stoichiometric of the reacting species in a balanced chemical equation 

- wherein

Formula: aA+bB\rightarrow cC+dD

              Rate=\frac{dR}{dT}

              =\alpha [A]^{x}.[B]^{y}

             =k[A]^{x}.[B]^{y}

 K= rate constant

 

Let R = \left [ A \right ]^{x}\left [ B \right ]^{y}\\ then,2R=k\left [ 2A \right ]^{x}\left [ B \right ]^{y}\\ x=1\\ also\: 8R=k\left [ 2A \right ]^{x}\left [ 2B \right ]^{y}\\ y=2\\ \therefore R=k\left [ A \right ]\left [ B \right ]^{2}


Option 1)

rate =k [A] [B]2

This solution is correct 

Option 2)

rate =k [A]2 [B]2

This solution is incorrect 

Option 3)

rate =k [A] [B]

This solution is incorrect 

Option 4)

rate =k [A]2 [B]

This solution is incorrect 

Posted by

divya.saini

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