$A \rightarrow B$
The above reaction is of zero order. The half-life of this reaction is $50 \ min$. The time taken for the concentration of $A$ to reduce to one-fourth of its initial value is $........... \ min$ (Nearest integer).

$5$ milli-moles of a solid $A$ was dissolved in $5$ moles of $H_2O$. On adding to the solvent,$A$ starts polymerising into another insoluble solid following zero order kinetics. On adding $6$ milli-moles of another solid solute $C$ (after $20$ minutes) the polymerisation completely stops. The insoluble solid polymer is removed and the resulting solution was cooled to a temperature less than $-0.186\,^{\circ}C$ (melting point of solution) to cause solidification of some liquid water. Calculate the value of $'X'$ if rate constant for polymerisation reaction is represented as $10^{-X}\,moles/minute$. $[K_f(H_2O) = 1.86\, K\, Kg\,mol^{-1}]$

What is a zero order reaction? Determine the integrated rate equation for a zero order reaction $R \to P$.

For a zero-order reaction,the rate constant $K = 2 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$. If the concentration of the reactant after $25 \ s$ is $0.5 \ M$,then its initial concentration must be ...... $M$.

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

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: