Assertion: All collision of reactant molecules leads to product formation.

Reason: Only those collisions in which molecules have correct orientation and sufficient kinetic energy lead to compound formation. 

Choose the correct answer out of the following choices.
A. Both assertion and reason are correct, and the reason is correct  of assertion.
B. Both assertion and reason are correct, but reason does not explain assertion.
C. Assertion is correct, but reason is incorrect
D. Both assertion and reason are incorrect.
E. Assertion is incorrect, but reason is correct.

Kindly go through the solution 

$K=A.e^{-Ea/RT}=\left(6.5\times 10^2\right)e^{-26000K/T}$

$\frac{Ea}{8.314}=26000$

Ea = 216.164kJ/mol $\cong$ $$ 216

Reaction rate is used to measure how fast or slow reactions occur per unit time. The rate constant is a proportionality factor that remains constant for every reaction.

Yes, in elementary reactions, order and molecularity can be the same, but this is not always the case because order is an experimental quantity, and molecularity is a theoretical concept.

Reaction Kinetics, also known as chemical kinetics, is the study of the rate of chemical reaction and the factors affecting the reaction rate, such as temperature, concentration, and catalyst.