For an n^{th} order reaction,the rate law is | vedclass

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(C) The rate law is $\frac{dx}{dt} = K[A]^n$. Taking the logarithm on both sides: $\log \left( \frac{dx}{dt} \right) = n \log [A] + \log K$. This equa

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Both order of reaction and $K$ (Rate constant)

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(C) The rate law is $\frac{dx}{dt} = K[A]^n$. Taking the logarithm on both sides: $\log \left( \frac{dx}{dt} \right) = n \log [A] + \log K$. This equation is in the form of a straight line $y = mx + c$,where $y = \log \left( \frac{dx}{dt} \right)$,$x = \log [A]$,slope $m = n$,and intercept $c = \log K$. Thus,by plotting $\log \left( \frac{dx}{dt} \right)$ versus $\log [A]$,the slope gives the order of reaction $(n)$ and the intercept gives the logarithm of the rate constant $(\log K)$. Therefore,both the order of reaction and the rate constant can be determined.

For an $n^{th}$ order reaction,the rate law is given by $\frac{dx}{dt} = K[A]^n$. Which parameter can be determined from the logarithmic plot?

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