For the reaction 2A + B rightarrow A_2B,if th | vedclass

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(C) The rate law for the reaction $2A + B \rightarrow A_2B$ is given by $Rate = k[A]^x[B]^y$. Assuming the reaction is elementary,the rate law is $Rat

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Increase by $2$ times

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(C) The rate law for the reaction $2A + B \rightarrow A_2B$ is given by $Rate = k[A]^x[B]^y$. Assuming the reaction is elementary,the rate law is $Rate = k[A]^2[B]^1$. Let the initial rate be $R_1 = k[A]^2[B]$. When the concentration of $A$ is doubled $(2[A])$ and $B$ is halved $([B]/2)$,the new rate $R_2$ is: $R_2 = k(2[A])^2([B]/2) = k(4[A]^2)([B]/2) = 2k[A]^2[B]$. Comparing $R_2$ with $R_1$,we get $R_2 = 2R_1$. Therefore,the rate of the reaction increases by $2$ times.

For the reaction $2A + B \rightarrow A_2B$,if the concentration of reactant $A$ is doubled and the concentration of reactant $B$ is halved,the rate of the reaction will:

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