At high pressure the following reaction is zero order

2NH₃(g) KN₂(g) + 3H₂(g)

Which of the following options are correct for this reaction?

A. Rate of reaction = Rate constant

B. Rate of the reaction depends on concentration of ammonia.

C. Rate of decomposition of ammonia will remain constant until ammonia disappears completely.

D. Further increase in pressure will change the rate of reaction.

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.