For 2A+B+C →Products , rate law is given by rate=k[A][B]2 & rate constant (k) is 2×10−6M−2s−1 . Then rate of the reaction become 2×10−9M−2s−1 only when [A] [B] [C]

rate = K[A][B]2 [A][B]2=rateK=2×10−92×10−6 =10−3 ∴ if [A]=0.1,[B]=0.1 then [A][B]2=0.001

For 2A+B+C →Products , rate law is given by rate=k[A][B]2 & rate constant (k) is 2×10−6M−2s−1 . Then rate of the reaction become 2×10−9M−2s−1 only when [A] [B] [C]

rate = K[A][B]2 [A][B]2=rateK=2×10−92×10−6 =10−3 ∴ if [A]=0.1,[B]=0.1 then [A][B]2=0.001

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For $2 A + B + C \to Products$ , rate law is given by $r a t e = k [A] {[B]}^{2}$ & rate constant $(k)$ is $2 \times 10^{- 6} M^{- 2} s^{- 1}$ . Then rate of the reaction become $2 \times 10^{- 9} M^{- 2} s^{- 1}$ only when
[A] [B] [C]

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0.1 M 0.1M 0.2 M

0.2 M 0.1 M 0.2 M

0.1 M 0.1 M any value

0.2 M 0.2 M 0.1 M

answer is C.

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$r a t e = K [A] {[B]}^{2}$

$[A] {[B]}^{2} = \frac{r a t e}{K} = \frac{2 \times 10^{- 9}}{2 \times 10^{- 6}}$

$= 10^{- 3}$

$∴$ if $[A] = 0.1, [B] = 0.1$ then

$[A] {[B]}^{2} = 0.001$

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For 2A+B+C →Products , rate law is given by rate=k[A][B]2 & rate constant (k) is 2×10−6M−2s−1 . Then rate of the reaction become 2×10−9M−2s−1 only when [A] [B] [C]

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For $2 A + B + C \to Products$ , rate law is given by $r a t e = k [A] {[B]}^{2}$ & rate constant $(k)$ is $2 \times 10^{- 6} M^{- 2} s^{- 1}$ . Then rate of the reaction become $2 \times 10^{- 9} M^{- 2} s^{- 1}$ only when
[A] [B] [C]