In a one-component second-order reaction,if the concentration of the reactant is reduced to half,the rate

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.

Assertion : In rate law,unlike in the expression for equilibrium constants,the exponents for concentrations do not necessarily match the stoichiometric coefficients.
Reason : It is the mechanism and not the balanced chemical equation for the overall change that governs the reaction rate.

For the reaction $2A + B \rightarrow \text{Product}$,the half-life period remains unchanged when the concentration of $B$ is doubled. However,when the concentration of $A$ is doubled,the rate of the reaction doubles. Determine the unit of the rate constant for this reaction.

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 the reaction: $KClO_3 + 6FeSO_4 + 3H_2SO_4 \to KCl + 3Fe_2(SO_4)_3 + 3H_2O$. Determine if the following statement is True $(T)$ or False $(F)$: The reaction is elementary.