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

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 $0.25 \ M$?

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:

For a zero order reaction:

At high pressure,the following reaction is zero order:
$2NH_{3(g)} \xrightarrow[Pt \ \text{catalyst}]{1130 \ K} N_{2(g)} + 3H_{2(g)}$
Choose the option which is not true with respect to the reaction,from the choices given below:

Which of the following is the slope of the graph of $[A]_{t}$ versus time for a zero order reaction?