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(D) The given rate law is $	ext{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

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

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(D) The given rate law is $	ext{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 of the concentration terms: $1 + 0.5 + 0.5 = 2$,which is correct.$3$. The order with respect to $Q$ is $0.5$ and with respect to $R$ is $0.5$,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 $(mol\ L^{-1})^{1-2} s^{-1} = mol^{-1}\ L\ s^{-1}$.Therefore,the statement in option $D$ is incorrect because $mol\ L^{-1}\ s^{-1}$ is the unit for a zero-order reaction.

Differential form of the rate equation is $\frac{dx}{dt} = k[P][Q]^{0.5}[R]^{0.5}$. Which statement about the above equation is wrong?

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