The reaction $A \xrightarrow{K} \text{Product}$ is zero order while the reaction $B \xrightarrow{K} \text{Product}$ is first order. For what initial concentration of $A$,the half-lives of the two reactions will be equal?

Which of the following graphs is incorrect for a first-order reaction? $A \rightarrow B$

The rate constant for the first order decomposition of $H_{2}O_{2}$ is given by the following equation:
$\log k = 14.34 - 1.25 \times 10^{4} \, K / T$
Calculate $E_{a}$ for this reaction and at what temperature will its half-period be $256 \, min$?

Select the incorrect statement.

Determine whether the following statements are True or False:
$(a)$ The rate of reaction can be decreased by decreasing the concentration of reactant.
$(b)$ Graphite quickly changes to Diamond.
$(c)$ The rate of corrosion of iron is fast.
$(d)$ The meaning of kinesis in Greek is movement.

Fill in the blanks:
$(1)$ The time required to complete $99.9\%$ of a first-order reaction is ............ times the ${t_{1/2}}$.
$(2)$ The reaction in which the rate is given by $-\frac{d[R]}{dt} = k$ has an order of reaction equal to ........
$(3)$ For the reaction $[R] = [R]_0 e^{-kt}$,the order is .......