For the reaction $2 A + B + C \to 2 D$ . The observed rate law is Rate= $K [A] {[B]}^{2}$ . Correct statements are
a) An increase of cone .of C does not affect the rate
b)Doubling the conc of A doubles the rate
c)Tripling the conc of B increases the rate by 9 times
d)Doubling the conc of C, doubling the rate

a,b,c

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b,c,d

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c,d

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Solution

The correct option is A a,b,c
Given rate is $k [A] {[B]}^{2}$
It is overall $3^{r d}$ order reaction with a following first order and B following second order.
(a) True C is not affecting the rate of reaction.
(b) True $r a t e_{1} = k [A] {[B]}^{2} r a t e_{2} = k [2 A] {[B]}^{2} = 2 k [A] {[B]}^{2} = 2 \times r a t e_{1}$
(c) True $r a t e_{1} = k [A] {[B]}^{2} r a t e_{3} = k [A] {[3 B]}^{2} = 9 K k [A] {[B]}^{2} = 9 \times r a t e_{1}$
(d)False C does not affected the rate in any manner.

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For the reaction 2A+B+C→2D. The observed rate law is Rate=K[A][B]2. Correct statements area) An increase of cone .of C does not affect the rateb)Doubling the conc of A doubles the ratec)Tripling the conc of B increases the rate by 9 timesd)Doubling the conc of C, doubling the rate