For a chemical reaction....can never be a fraction

In a reaction, $A + B \rightarrow$ product, rate is doubled when the concentration of $B$ is doubled, and rate increases by a factor of $8$ when the concentration of both the reactants $(A$ and $B)$ are doubled, rate law for the reaction can be written as

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.

The rate equation for the reaction $2A + B \to C$ is found to be : rate $ = k[A][B]$. The correct statement in relation to this reaction is that the

For a certain reaction $A \to P$ , the half life for different initial concentration of $A$ is mentioned below 

$[A_0]$  $||$  $0.1$  $||$  $0.025$

$t_{1/2}(s)$  $||$ $100$  $||$  $50$

Which of the following option $(s)$ is / are correct

What is the order of reaction' for $A + B \to C$