For a reaction $A + B \to C$ , the rate law is written as $r = k [A]^{2} [B]$ . Doubling the concentration of both of $A$ and $B$ increases the rate of reaction by:

2 times

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4 times

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8 times

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16 times

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Solution

The correct option is D 8 times
The reaction is 2 $^{n d}$ order with respect to A, and 1st order with respect to B. Therefore doubling the concentration of $A$ & $B$ increases the rate by 4 times and 2 times respectively. Thus the total rate increases by $2 \times 4$ = 8 times.

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For a reaction A+B→C, the rate law is written as r=k[A]2[B]. Doubling the concentration of both of A and B increases the rate of reaction by:

The correct option is D 8 timesThe reaction is 2nd order with respect to A, and 1st order with respect to B. Therefore doubling the concentration of A & B increases the rate by 4 times and 2 times respectively. Thus the total rate increases by 2×4 = 8 times.

For a reaction $A + B \to C$ , the rate law is written as $r = k [A]^{2} [B]$ . Doubling the concentration of both of $A$ and $B$ increases the rate of reaction by:

The correct option is D 8 times
The reaction is 2 $^{n d}$ order with respect to A, and 1st order with respect to B. Therefore doubling the concentration of $A$ & $B$ increases the rate by 4 times and 2 times respectively. Thus the total rate increases by $2 \times 4$ = 8 times.