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:

For the reaction,$A \rightarrow$ products,if the graph of $[A]$ vs time gives a straight line,predict the order of the reaction.

Which of the following is a zero order reaction?

For a zero order reaction,the plot of concentration of reactant $vs$ time is (Hint: Consider the intercept on the concentration axis)

For a reaction $A \to$ Products,a plot of $\log\,t_{1/2}$ versus $\log\,a_0$ is shown in the figure. If the initial concentration of $A$ is represented by $a_0,$ the order of the reaction is

$A \rightarrow P$ is a zero order reaction. At $298 \ K$ the rate constant of the reaction is $1 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$. Initial concentration of '$A$' is $0.1 \ mol \ L^{-1}$. What is the concentration of '$A$' after $10 \ s$?