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(D) The rate law for the reaction $aG + bH ightarrow$ Products is given by: $	ext{Rate} = k[G]^x[H]^y$. From the given information: $1)$ When both

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$3$

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(D) The rate law for the reaction $aG + bH ightarrow$ Products is given by: $	ext{Rate} = k[G]^x[H]^y$. From the given information: $1)$ When both concentrations are doubled: $(2)^x(2)^y = 8$,which implies $2^{(x+y)} = 2^3$,so $x + y = 3$. $2)$ When only $[G]$ is doubled: $(2)^x(1)^y = 2$,which implies $2^x = 2^1$,so $x = 1$. Substituting $x = 1$ into the equation $x + y = 3$,we get $1 + y = 3$,which gives $y = 2$. The overall order of the reaction is $x + y = 1 + 2 = 3$. Therefore,the correct option is $(D)$.

Consider a reaction $aG + bH \rightarrow$ Products. When the concentration of both reactants $G$ and $H$ is doubled,the rate increases by $8$ times. However,when the concentration of $G$ is doubled keeping the concentration of $H$ fixed,the rate is doubled. The overall order of the reaction is:

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