In the reaction,$A + B \to C + D$,the rate $\left( \frac{dx}{dt} \right)$ when plotted against time $t$ gives a straight line parallel to the time axis. The order and rate of reaction will be

Which of the following is correct with respect to the graph given?
$[R] = \text{Concentration at time } 't'$
$[R]_0 = \text{Initial concentration}$

Which among the following reactions is an example of a zero-order reaction?

Which of the following is a zero order reaction?

For the reaction $A \rightarrow \text{products}$,the graph of $t_{1/2}$ versus $[A]_0$ is given below. The concentration of $A$ at $10 \ \text{minutes}$ is $.......... \times 10^{-3} \ \text{mol L}^{-1}$ $(nearest \ integer)$. The reaction was started with $2.5 \ \text{mol L}^{-1}$ of $A$.

If doubling the initial concentration of reactant doubles $t_{1/2}$ of reaction,the order of reaction is