For the reaction A + B $\to$ C + D, doubling the concentration of both the reactants increases the reaction rate by 8 times and doubling the initial concentration of the only B simply doubles the reaction rate. The rate law for the reaction is:

r = k [A] [B]^{2}

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r = k [A] [B]

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r = k [A]^{1 / 2} [B]

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r = k [A]^{2} [B]

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Solution

The correct option is D $r = k [A]^{2} [B]$
A + B $\to$ C + D
as doubling the initial concentration of only B simply doubles the reaction rate so it is first order wrt to B.
and similarly it is second order w.r.t A.
so $r = k [A]^{2} [B]$ .

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For the reaction A + B → C + D, doubling the concentration of both the reactants increases the reaction rate by 8 times and doubling the initial concentration of the only B simply doubles the reaction rate. The rate law for the reaction is:

The correct option is D r=k[A]2[B]A + B → C + Das doubling the initial concentration of only B simply doubles the reaction rate so it is first order wrt to B.and similarly it is second order w.r.t A.so r=k[A]2[B].

For the reaction A + B $\to$ C + D, doubling the concentration of both the reactants increases the reaction rate by 8 times and doubling the initial concentration of the only B simply doubles the reaction rate. The rate law for the reaction is:

The correct option is D $r = k [A]^{2} [B]$
A + B $\to$ C + D
as doubling the initial concentration of only B simply doubles the reaction rate so it is first order wrt to B.
and similarly it is second order w.r.t A.
so $r = k [A]^{2} [B]$ .