Consider the kinetic data given in the following table for the reaction A+B+C→ productThe Rate of the reaction for A=0.15 mol/dm3 .B=0.23 mol/dm3 and C=0.15 mol/dm3 is found to be y×10−5mol/dm−3s−1 the value of y is ____________

rate=KAxBxCzFrom 182 y=0From 183 z=1From 184 x=16×10−5=K×0.2×0.1K=3×10−13Rate=3×10−3×0.15×1×0.15=6.75×10−5

Consider the kinetic data given in the following table for the reaction A+B+C→ productThe Rate of the reaction for A=0.15 mol/dm3 .B=0.23 mol/dm3 and C=0.15 mol/dm3 is found to be y×10−5mol/dm−3s−1 the value of y is ____________

rate=KAxBxCzFrom 182 y=0From 183 z=1From 184 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 $A + B + C \overset{}{\to} p r o d u c t$

The Rate of the reaction for $[A] = 0.15 m o l / d m^{3}$ . $[B] = 0.23 m o l / d m^{3}$ and $[C] = 0.15 m o l / d m^{3}$ 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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7.75

6.75

8.75

7.85

answer is B.

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Detailed Solution

$r a t e = K {[A]}^{x} {[B]}^{x} {[C]}^{z}$
$\begin{array}{l} F r o m 182 y = 0 \\ F r o m 183 z = 1 \\ F r o m 184 x = 1 \\ 6 \times 10^{- 5} = K \times 0.2 \times 0.1 \\ K = 3 \times 10^{- 13} \\ R a t e = 3 \times 10^{- 3} \times 0.15 \times 1 \times 0.15 \\ = 6.75 \times 10^{- 5} \end{array}$