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  • Stuck here, help me understand: - Chemical Kinetics and Surface Chemistry - BITSAT

For a reaction mA\rightarrow \: product. Rate equation can be written as rate = k[A]^{^{m}}. If concn is changed from 0.1M to 0.15M then rate becomes double, what will be the value of m?

  • Option 1)

    0

  • Option 2)

    1

  • Option 3)

    1.7

  • Option 4)

    2

 

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

 

 rate= k[A]^{m} given

r_1=k[A]^{m}= k(0.1)^{m}

and  r_2= k(0.5)^{m}

Given that r_2= 2r_1

We have, (0.15)^{m}= 2(0.1)^{m}

(1.5)^{m}=2

m\ln (1.5)= \ln(2)

m= \frac{0.693}{\ln(1.5)}=1.7


Option 1)

0

Incorrect option

Option 2)

1

Incorrect option

Option 3)

1.7

Correct option

Option 4)

2

Incorrect option

Posted by

Aadil

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