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For the reaction , 2A + B \rightarrow products , when the concentrations of A and B both were doubled , the rate of the reaction increased from 0.3\: mol\: L^{-1}s^{-1}\: to\:2.4 \: mol\: L^{-1}s^{-1} . When the concentration of A alone is doubled , the rate increased from 0.3\: mol\: L^{-1}s^{-1}\: to\:0.6 \: mol\: L^{-1}s^{-1}.

Which one of the following statement is correct ?

 

  • Option 1)

    Order of the reaction with respect to B is 1 

  • Option 2)

    Order of reaction with respect to A is 2

  • Option 3)

    Total order of the reaction is 4

  • Option 4)

    Order of the reaction with respect to B is 2

Answers (1)

best_answer

 

Zero Order Reaction -

Zero order reaction means that the rate of the reaction is proportional to zeroth power of the concentration of reactants

 

- wherein

R\rightarrow P

Rate=\frac{-d(R)}{dt}=K[R]^{0}=K

t_\frac {1}{2}= time required for half completion of reaction=\frac{a}{2k}

 

 

nth order reaction -

The rates of the reaction is proportional to nth power of reactant

- wherein

Differential rate law

=\frac{dx}{dt}=k(a-x)^{n}

Integrated rate laws,

=\frac{1}{n-1}[(a-x)^{1-n} -a^{(1-n)}]=k_nt

a= initial, concentration of reactant at t=0 sec

x= concentration of product formed at t= tsec

t_\frac{1}{2}=\frac{1}{(n-1)(a^{n-1})(k_n)}[2^{n-1}-1]

Formulae for all the order except n=1

The formula 

\mu =K\left [ A \right ]^{X}\left [ B \right ]^{Y}

8 =2^{3}=2^{x+y}\Rightarrow x+y=3

2=2^{x}\Rightarrow x=1\: then\: y=2

Order w.nt. A= 1

Order w.n2 B=2

 

 


Option 1)

Order of the reaction with respect to B is 1 

Option 2)

Order of reaction with respect to A is 2

Option 3)

Total order of the reaction is 4

Option 4)

Order of the reaction with respect to B is 2

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