Derive an expression to calculate the time required for the completion of a zero order reaction.
(N/A) For a zero order reaction,the integrated rate equation is $k = \frac{[R]_0 - [R]}{t}$.
For the completion of the reaction,the concentration of the reactant $[R]$ becomes $0$.
Substituting $[R] = 0$ in the equation:
$k = \frac{[R]_0 - 0}{t} = \frac{[R]_0}{t}$.
Therefore,the time required for completion is $t = \frac{[R]_0}{k}$.
For the completion of the reaction,the concentration of the reactant $[R]$ becomes $0$.
Substituting $[R] = 0$ in the equation:
$k = \frac{[R]_0 - 0}{t} = \frac{[R]_0}{t}$.
Therefore,the time required for completion is $t = \frac{[R]_0}{k}$.
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The rates of a certain reaction $(dc/dt)$ at different times are as follows:
Time $(sec)$ Rate $(mole \ litre^{-1} \ sec^{-1})$ $0$ $2.8 \times 10^{-2}$ $10$ $2.78 \times 10^{-2}$ $20$ $2.81 \times 10^{-2}$ $30$ $2.79 \times 10^{-2}$
The reaction is:
| Time $(sec)$ | Rate $(mole \ litre^{-1} \ sec^{-1})$ |
|---|---|
| $0$ | $2.8 \times 10^{-2}$ |
| $10$ | $2.78 \times 10^{-2}$ |
| $20$ | $2.81 \times 10^{-2}$ |
| $30$ | $2.79 \times 10^{-2}$ |
The reaction is:
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