Consider the kinetic data given in the following table for the reaction $A + B + C \rightarrow$ Product.
Experiment No.
$\begin{array}{c}{[ A ]} \\ \left( mol dm ^{-3}\right)\end{array}$
$\begin{array}{c}{[ B ]} \\ \left( mol dm ^{-3}\right)\end{array}$
$\begin{array}{c}{[ C]} \\ \left( mol dm ^{-3}\right)\end{array}$
Rate of reaction $\left( mol dm ^{-3} s ^{-1}\right)$
$1$
$0.2$
$0.1$
$0.1$
$6.0 \times 10^{-5}$
$2$
$0.2$
$0.2$
$0.1$
$6.0 \times 10^{-5}$
$3$
$0.2$
$0.1$
$0.2$
$1.2 \times 10^{-4}$
$4$
$0.3$
$0.1$
$0.1$
$9.0 \times 10^{-5}$
The rate of the reaction for $[ A ]=0.15 mol dm ^{-3},[ B ]=0.25 mol dm ^{-3}$ and $[ C ]=0.15 mol dm ^{-3}$ is found to be $Y \times 10^{-5} mol dm d ^{-3} s ^{-1}$. The value of $Y$ i. . . . . . .
Consider the kinetic data given in the following table for the reaction $A + B + C \rightarrow$ Product.
| Experiment No. | $\begin{array}{c}{[ A ]} \\ \left( mol dm ^{-3}\right)\end{array}$ | $\begin{array}{c}{[ B ]} \\ \left( mol dm ^{-3}\right)\end{array}$ | $\begin{array}{c}{[ C]} \\ \left( mol dm ^{-3}\right)\end{array}$ | Rate of reaction $\left( mol dm ^{-3} s ^{-1}\right)$ |
| $1$ | $0.2$ | $0.1$ | $0.1$ | $6.0 \times 10^{-5}$ |
| $2$ | $0.2$ | $0.2$ | $0.1$ | $6.0 \times 10^{-5}$ |
| $3$ | $0.2$ | $0.1$ | $0.2$ | $1.2 \times 10^{-4}$ |
| $4$ | $0.3$ | $0.1$ | $0.1$ | $9.0 \times 10^{-5}$ |
The rate of the reaction for $[ A ]=0.15 mol dm ^{-3},[ B ]=0.25 mol dm ^{-3}$ and $[ C ]=0.15 mol dm ^{-3}$ is found to be $Y \times 10^{-5} mol dm d ^{-3} s ^{-1}$. The value of $Y$ i. . . . . . .
- [IIT 2019]
- A
$6.75$
- B
$6.80$
- C
$6.85$
- D
$6.90$
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