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For the non - stoichiometre reaction    2A+B\rightarrow C+D,, the following kinetic data were  obtained  in  three  separate experiments, all at 298 K.

    

The rate law for the formation of C is :

  • Option 1)

    \frac{dc}{dt}=k\left [ A \right ]\left [ B \right ]\;

  • Option 2)

    \frac{dc}{dt}=k\left [ A \right ]^{2}\left [ B \right ]\;

  • Option 3)

    \frac{dc}{dt}=k\left [ A \right ]\left [ B \right ]^{2}

  • Option 4)

    \frac{dc}{dt}=k\left [ A \right ]

 

Answers (1)

best_answer

As we have learnt,

 

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

 

 From the given values in table 

rate of reaction is of first order in respect to A and of zeroth order in respect to B, so

\frac{\mathrm{d} C}{\mathrm{d} t} = K[A]

 


Option 1)

\frac{dc}{dt}=k\left [ A \right ]\left [ B \right ]\;

Option 2)

\frac{dc}{dt}=k\left [ A \right ]^{2}\left [ B \right ]\;

Option 3)

\frac{dc}{dt}=k\left [ A \right ]\left [ B \right ]^{2}

Option 4)

\frac{dc}{dt}=k\left [ A \right ]

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SudhirSol

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