For a certain reaction $R \to \text{Product}$, the plot of concentration $[R]$ vs time has a negative slope as shown. The order of reaction is:

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 $A$ $(mol \ L^{-1})$ |
| :--- | :--- |
| $0$ | $0.1$ |
| $15$ | $0.05$ |
| $20$ | $0.1 - x$ |

For a reaction,doubling the concentration of the reactant doubles the half-life period. What is the order of the reaction?

The half-life period of a zero order reaction is:

The half-life period for a certain zero-order reaction is $10 \text{ min}$. How much time is required for this reaction to complete $100\%$ (in $\text{ min}$)?

The concentration of $R$ in the reaction $R \rightarrow P$ was measured as a function of time and the following data is obtained:

$[R] \text{ (molar)}$	$1.0$	$0.75$	$0.40$	$0.10$
$t \text{ (min.)}$	$0.0$	$0.05$	$0.12$	$0.18$

The order of the reaction is: