Consider the kinetic data given in the following table for the reaction A+B+C→product.Experiment No.[A](mol dm-3)[B](Mol dm-3)[C](Mol dm-3)Rate of reaction(Mol dm-3)10.20.10.16.0×10-520.20.20.16.0×10-530.20.10.21.2 × 10-440.30.10.19.0×10-5The rate of the reaction for A = 0.15 mol−3, B = 0.25 mol dm−3 and [C] = 0.15 mol dm-3 is found to be Y × 10−5mol dm−3s−1. The value of Y is _____

Rate =KAxByC2 From 1 & 2 Y = 0From 1 & 3 Z = 1From 1 & 4 X = 16×10−5=K×0.2×0.1K=3×10−13Rate = 3×10−3×0.15×1×0.15=6.75×10−5

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Consider the kinetic data given in the following table for the reaction
$A + B + C \to$ product.
Experiment No.
[A]
(mol dm-3)
[B]
(Mol dm-3)
[C]
(Mol dm-3)
Rate of reaction
(Mol dm-3)
1 0.2 0.1 0.1 $6.0 \times 10^{- 5}$
2 0.2 0.2 0.1 $6.0 \times 10^{- 5}$
3 0.2 0.1 0.2 $1.2 \times 10^{- 4}$
4 0.3 0.1 0.1 $9.0 \times 10^{- 5}$
The rate of the reaction for $[A] = 0.15 m o l^{- 3}, [B] = 0.25 m o l d m^{- 3}$ and [C] = 0.15 mol $d m^{- 3}$ is found to be $Y \times 10^{- 5} m o l d m^{- 3} s^{- 1}$ . The value of Y is _____

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Rate = $K {[A]}^{x} {[B]}^{y} {[C]}^{2}$

From 1 & 2 Y = 0

From 1 & 3 Z = 1

From 1 & 4 X = 1

$6 \times 10^{- 5} = K \times 0.2 \times 0.1$

$K = 3 \times 10^{- 13}$

Rate = $3 \times 10^{- 3} \times 0.15 \times 1 \times 0.15 = 6.75 \times 10^{- 5}$

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