From the concentrations of $C_{4}H_{9}Cl$ (butyl chloride) at different times given below,calculate the average rate of the reaction:
$C_{4}H_{9}Cl + H_{2}O \rightarrow C_{4}H_{9}OH + HCl$
during different intervals of time.
$t/s$ $0$ $50$ $100$ $150$ $200$ $300$ $400$ $700$ $800$ $[C_{4}H_{9}Cl]/mol\ L^{-1}$ $0.100$ $0.0905$ $0.0820$ $0.0741$ $0.0671$ $0.0549$ $0.0439$ $0.0210$ $0.017$
$C_{4}H_{9}Cl + H_{2}O \rightarrow C_{4}H_{9}OH + HCl$
during different intervals of time.
| $t/s$ | $0$ | $50$ | $100$ | $150$ | $200$ | $300$ | $400$ | $700$ | $800$ |
| $[C_{4}H_{9}Cl]/mol\ L^{-1}$ | $0.100$ | $0.0905$ | $0.0820$ | $0.0741$ | $0.0671$ | $0.0549$ | $0.0439$ | $0.0210$ | $0.017$ |
(N/A) The average rate of reaction is calculated using the formula: $r_{av} = -\frac{\Delta[R]}{\Delta t} = -\frac{[R]_{2} - [R]_{1}}{t_{2} - t_{1}}$.
| $Time \ Interval \ (s)$ | $Average \ Rate \ (mol \ L^{-1} s^{-1})$ |
| $0-50$ | $1.90 \times 10^{-4}$ |
| $50-100$ | $1.70 \times 10^{-4}$ |
| $100-150$ | $1.58 \times 10^{-4}$ |
| $150-200$ | $1.40 \times 10^{-4}$ |
| $200-300$ | $1.22 \times 10^{-4}$ |
| $300-400$ | $1.10 \times 10^{-4}$ |
| $700-800$ | $0.40 \times 10^{-4}$ |
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