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

The reaction $2X \to B$ is a zeroth order reaction. If the initial concentration of $X$ is $0.2 \ M$,the half-life is $6 \ h$. When the initial concentration of $X$ is $0.5 \ M$,the time required to reach its final concentration of $0.2 \ M$ will be ........ $hr$.

Consider the data given below for the hypothetical reaction $A \to X$:

$Time \ (s)$	$Rate \ (mol \ L^{-1} s^{-1})$
$0$	$1.60 \times 10^{-2}$
$10$	$1.60 \times 10^{-2}$
$20$	$1.60 \times 10^{-2}$
$30$	$1.60 \times 10^{-2}$

From the above data,the order of the reaction is:

For a reaction $A \rightarrow$ products,the half-life period is $1 \ h$. The initial concentration of reactant $A$ is $2 \ M$. If this reaction is of zero order,how many hours will it take for the concentration of the reactant to decrease from $0.5 \ M$ to $0.25 \ M$?

When the initial concentration of the reactant is doubled,the half-life period of a zero order reaction:

In the following reaction $A \to B + C,$ the rate constant is $0.001 \ M \ s^{-1}.$ If we start with $1 \ M$ of $A,$ then the concentrations of $A$ and $B$ after $10 \ minutes$ are respectively: