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

Find the percentage of unreacted reactant for a zero order reaction in $90 \ s$ having a rate constant of $1 \ mol \ dm^{-3} \ s^{-1}$. (in $\%$)

Mention True $(T)$ and False $(F)$ statement of the following for reaction $R \to P$.
Rate $= -\frac{d[R]}{dt} = k[R]^0$
Rate $= -\frac{d[R]}{dt} = k$

The decomposition of $NH_3$ on $Pt$ surface is a zero order reaction. If the value of rate constant is $2 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$,the rates of appearance of $N_2$ and $H_2$ are respectively:

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 $\rightarrow$ P at T K, the half life ($t_{1/2}$) is plotted as a function of initial concentration $[A]_0$ of A as given below. The value of x in the given figure is _______ s (Nearest integer)