For a reaction,$A \rightarrow B$,the rate equation is $r = K[A]^0$. If the initial concentration of the reactant is $a \ mol \ dm^{-3}$,find the half-life time of the reaction.

For a zero order reaction,the plot of concentration of reactant $vs$ time is (Hint: Consider the intercept on the concentration axis)

What is the unit of $K$ for a zero-order reaction?

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

Half life of zero order reaction $A \rightarrow \text{product}$ is $1 \ \text{hour}$,when initial concentration of reactant is $2.0 \ \text{mol L}^{-1}$. The time required to decrease concentration of $A$ from $0.50$ to $0.25 \ \text{mol L}^{-1}$ is:

$5$ 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 $10^{-X}\,moles/minute$. $[K_f(H_2O) = 1.86\, K\, Kg\,mol^{-1}]$