Half-lives of a first-order and a zero-order reaction are the same. Assume that the initial concentration of the reactant is the same for both reactions,then the ratio of the initial rates of the first-order reaction to that of the zero-order reaction is:

For the following parallel chain reaction,what will be the value of the overall half-life of $A$ in minutes?
Given that $\frac{[B]_t}{[C]_t} = \frac{16}{9}$
$A \xrightarrow{k_1 = 2 \times 10^{-3} \ s^{-1}} 4B$
$A \xrightarrow{k_2} C$

If the half-life periods of a first-order reaction and a zero-order reaction are equal,then the ratio of the initial rates of the reactions will be .............

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 $256 \, min$?

At $100\,^\circ C,$ the gaseous reaction $A_{(g)} \rightarrow 2B_{(g)} + C_{(g)}$ is found to be first order. Starting with pure $A,$ if at the end of $10\,\min$,the total pressure of the system is $160\,mm$ and after a long time,when dissociation of $A$ was complete,it was $300\,mm.$ The partial pressure of $A$ at the end of $10\,\min$ is .......... $mm$

Which of the following relations is correct for the given reaction orders?