Which of the following equations represents the integrated rate law for a zero order reaction?
- A$k = \frac{[A]_t - [A]_0}{t}$
- B$k = \frac{1}{t} \log_{10} \frac{[A]_0}{[A]_t}$
- C$k = \frac{[A]_0 - [A]_t}{t}$
- D$k = \frac{t}{2.303} \times \log_{10} \frac{[A]_0}{[A]_t}$
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What is the concentration (in $mol \ L^{-1}$) of the product $B$ after $20 \ s$ in the following reaction? Given that $A \longrightarrow 3B$,rate $= k[A]^0$. The data is provided in the table below:
| Time $(s)$ | Concentration of reactant $A$ $(mol \ L^{-1})$ |
| :--- | :--- |
| $0$ | $0.1$ |
| $15$ | $0.05$ |
| $20$ | $0.1 - x$ |
| Time $(s)$ | Concentration of reactant $A$ $(mol \ L^{-1})$ |
| :--- | :--- |
| $0$ | $0.1$ |
| $15$ | $0.05$ |
| $20$ | $0.1 - x$ |
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