Decomposition of $X$ exhibits a rate constant of $0.05 \ \mu g/year$. How many years are required for the decomposition of $5 \ \mu g$ of $X$ into $2.5 \ \mu g$?

For the reaction $A \longrightarrow 3 B$,the rate is given by $rate = k[A]^0$. Based on the data provided in the table,what is the concentration of the product $B$ (in $mol \ L^{-1}$) after $20 \ s$?

Time $(s)$	Concentration of the reactant $(mol \ L^{-1})$
$0$	$0.1$
$15$	$0.05$
$20$	$0.1 - x$

The half-life of a zero-order reaction is $1 \text{ hour}$. If the initial concentration of the reactant is $2.0 \text{ mol L}^{-1}$, find the time required to decrease the concentration from $0.50 \text{ mol L}^{-1}$ to $0.25 \text{ mol L}^{-1}$. (in $\text{ hour}$)

What is the formula to find the value of $t_{1/2}$ for a Zero Order Reaction?

For a general reaction $A \to B$,a plot of the concentration of $A$ versus time is given in the figure. Answer the following questions based on this graph:
$(i)$ What is the order of the reaction?
$(ii)$ What is the slope of the curve?
$(iii)$ What are the units of the rate constant?

The rate constant for a zero order reaction is $2 \times 10^{-2} \ mol \ L^{-1} s^{-1}$. If the concentration of the reactant after $25 \ s$ is $0.5 \ M$,the initial concentration must have been $:-$ (in $M$)