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(D) For the elementary reaction $A_2 \underset{k_{-1}}{\overset{k_1}{\longleftrightarrow}} 2A$,the rate of reaction can be expressed in terms of the c

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$2k_1[A_2] - 2k_{-1}[A]^2$

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(D) For the elementary reaction $A_2 \underset{k_{-1}}{\overset{k_1}{\longleftrightarrow}} 2A$,the rate of reaction can be expressed in terms of the change in concentration of reactants and products.The rate of disappearance of $A_2$ is $-\frac{d[A_2]}{dt} = k_1[A_2] - k_{-1}[A]^2$.The rate of appearance of $A$ is $\frac{1}{2} \frac{d[A]}{dt} = k_1[A_2] - k_{-1}[A]^2$.Multiplying both sides by $2$,we get $\frac{d[A]}{dt} = 2k_1[A_2] - 2k_{-1}[A]^2$.

For an elementary chemical reaction,$A_2 \underset{k_{-1}}{\overset{k_1}{\longleftrightarrow}} 2A$,the expression for $\frac{d[A]}{dt}$ is

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