The half-life period for a certain zero-order reaction is $10 \text{ min}$. How much time is required for this reaction to complete $100\%$ (in $\text{ min}$)?

Write the rate equation for the reaction $2A + B \to C$ if the order of the reaction is zero.

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 $\%$)

The rate constant,$k$ of a zero order reaction $2 NH_{3(g)} \xrightarrow[1130 \ K]{Pt} N_{2(g)} + 3 H_{2(g)}$ is $y \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$. The rate of formation of hydrogen (in $mol \ L^{-1} \ s^{-1}$) is

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 $(mol \ L^{-1})$
$0$	$0.1$
$15$	$0.05$
$20$	$0.1 - x$

Consider the data given below for the hypothetical reaction $A \to X$:

$Time \ (s)$	$Rate \ (mol \ L^{-1} s^{-1})$
$0$	$1.60 \times 10^{-2}$
$10$	$1.60 \times 10^{-2}$
$20$	$1.60 \times 10^{-2}$
$30$	$1.60 \times 10^{-2}$

From the above data,the order of the reaction is: