The dimension of the rate constant for a second-order reaction involves:

Consider the given graph showing the variation of reactant concentration with time. Three different reactions were started with identical initial concentration of reactants. Which of the following statements is correct?

Rate of reaction is given by the following rate law $-\frac{d[C]}{dt} = \frac{k_1 [C]}{1 + k_2 [C]}$. Determine the order of reaction when the concentration $[C]$ is very high.

For a reaction,$A + 2B \rightarrow$ Products,when the concentration of $B$ alone is increased,the half-life remains the same. If the concentration of $A$ alone is doubled,the rate remains the same. The unit of the rate constant for the reaction is:

The rate of the reaction: $2N_2O_5 \rightarrow 4NO_2 + O_2$ can be written in three ways.
$-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$\frac{d[NO_2]}{dt} = k'[N_2O_5]$ ; $\frac{d[O_2]}{dt} = k''[N_2O_5]$
The relationship between $k$ and $k'$ and between $k$ and $k''$ are:

The mechanism of the reaction $2NO_2 + F_2 \to 2NO_2F$ is given by:
$(i)$ $NO_2 \xrightarrow{slow} NO + O$
$(ii)$ $F_2 + O + NO \xrightarrow{fast} NO_2F + F$
$(iii)$ $F + NO_2 \xrightarrow{fast} NO_2F$
Select the correct statement.