For the reaction $A + B \to$ Products, it is found that the order of A is 2 and of B is 3 in the rate expression. When the concentration of both is doubled the rate will increase to:

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Solution

The correct option is C 32
The rate law expression is $R = k [A]^{2} [B]^{3}$

The concentration of A and B are doubled.
$R^{'} = k [2 A]^{2} [2 B]^{3} = k 2^{2} [A]^{2} 2^{3} [B]^{3} = 2^{2} 2^{3} R = 32 R$

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For the reaction A+B→ Products, it is found that the order of A is 2 and of B is 3 in the rate expression. When the concentration of both is doubled the rate will increase to:

The correct option is C 32The rate law expression is R=k[A]2[B]3The concentration of A and B are doubled.R′=k[2A]2[2B]3=k22[A]223[B]3=2223R=32R

For the reaction $A + B \to$ Products, it is found that the order of A is 2 and of B is 3 in the rate expression. When the concentration of both is doubled the rate will increase to:

The correct option is C 32
The rate law expression is $R = k [A]^{2} [B]^{3}$

The concentration of A and B are doubled.
$R^{'} = k [2 A]^{2} [2 B]^{3} = k 2^{2} [A]^{2} 2^{3} [B]^{3} = 2^{2} 2^{3} R = 32 R$