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  • In a reaction between A and B, the initial rate of reaction (r 0) was measured for different initial concentrations of A and B as given below:

In a reaction between A and B, the initial rate of reaction (r0) was measured for different initial concentrations of A and B as given below:

          

          What is the order of the reaction to A and B?

              

Answers (1)

best_answer

we know that 
rate law $\left(r_{0})=k[A]^x[B]^y\right.
As per data 

\begin{aligned} & 5.07 \times 10^{-5}=k[0.2]^x[0.3]^y \\ & 5.07 \times 10^{-5}=k[0.2]^x[0.1]^y \\ & 1.43 \times 10^{-4}=k[0.4]^x[0.05]^y\end{aligned}

these are the equation 1, 2, and 3 respectively

Now, divide eq.1 by equation2, we get
1=(0.3 / 0.1)^y
from here we calculate that y = 0

Again, divide eq. 2 by Eq. 3, we get
Since y =0 also substitute the value of y 
So, \begin{aligned} & \left(\frac{1.43}{0.507}\right)=\left(\frac{0.4}{0.2}\right)^x \\ = & 2.821=2^x\end{aligned}

taking log both sides we get,

x=\frac{\log 2.821}{\log 2}
    = 1.496 
   = approx 1.5
Hence the order of reaction w.r.t A is 1.5 and w.r.t B is 0(zero)

Posted by

manish

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