The unit of the specific reaction rate constant for a first-order reaction (if the concentration is expressed in molarity) is:

Time required to decompose $SO_2Cl_2$ to half of its initial amount is $40 \ minutes$. If the decomposition is a first order reaction,what will be the rate constant of the reaction?

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

$A$ first order reaction has a specific reaction rate of $10^{-2} \ sec^{-1}.$ How much time will it take for $20 \ g$ of the reactant to reduce to $5 \ g?$ ........ $sec$

Consider a certain reaction $A \rightarrow \text{Products}$ with $k = 2.0 \times 10^{-2} \ s^{-1}$. Calculate the concentration of $A$ remaining after $100 \ s$ if the initial concentration of $A$ is $1.0 \ mol \ L^{-1}$.

The first order rate constant for the decomposition of $N_2O_5$ is $6.2 \times 10^{-4} \ s^{-1}$. The half-life period for this decomposition in seconds is: