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)

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:

The rate of a certain reaction depends on concentration according to the equation $-dc/dt = (K_1 C) / (1 + K_2 C)$. What is the order when concentration $(C)$ is very high?

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

The time for the half-life period of a certain reaction $A \rightarrow \text{Products}$ is $1 \ hr$. When the initial concentration of the reactant $A$ is $2.0 \ mol \ L^{-1}$,how many hours does it take for its concentration to decrease from $0.50 \ mol \ L^{-1}$ to $0.25 \ mol \ L^{-1}$ if it is a zero-order 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 $\%$)