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(D) The rate law is given by $Rate = k[P]^1[Q]^{0.5}[R]^{0.5}$.$1$. The order with respect to $P$ is $1$,which is correct.$2$. The total order of the

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Unit of specific reaction rate is $mol \, L^{-1} s^{-1}$

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(D) The rate law is given by $Rate = k[P]^1[Q]^{0.5}[R]^{0.5}$.$1$. The order with respect to $P$ is $1$,which is correct.$2$. The total order of the reaction is the sum of the exponents: $1 + 0.5 + 0.5 = 2$,which is correct.$3$. The order with respect to $Q$ and $R$ is $0.5$ each,which is correct.$4$. The unit of the rate constant $k$ for a reaction of order $n$ is $(mol \, L^{-1})^{1-n} s^{-1}$. For $n = 2$,the unit is $(mol \, L^{-1})^{1-2} s^{-1} = (mol \, L^{-1})^{-1} s^{-1} = L \, mol^{-1} s^{-1}$. Therefore,the statement in option $D$ is wrong.

The differential form of the rate equation is given by:
$dx/dt = k[P][Q]^{0.5}[R]^{0.5}$
Which statement about the above equation is wrong?

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The differential form of the rate equation is given by:$dx/dt = k[P][Q]^{0.5}[R]^{0.5}$Which statement about the above equation is wrong?