In the collision model it is assumed that reactions occur as a result of collisions between molecules with the correct kinetic energy and orientation. The minimum energy required for a reaction to occur when molecules collide is called the activation energy, Ea. The number of collisions that are favorably oriented for a reaction is described by the frequency factor, A. The Arrhenius equation relates both of these factors to the rate constant, k: k=A⋅e−Ea/(R⋅T)
where R=8.314 J/(mol⋅K) and T is the temperature in kelvins.
Based on the activation energies and frequency factors, rank the following reactions from fastest to slowest reaction rate, assuming they are all at the same temperature and that each starts with the same initial concentration.
Rank from fastest to slowest reaction rate. To rank items as equivalent, overlap them.
i. Ea=50 kJ/mol
A=1.5×10−7 s−1
ii. Ea=350 kJ/mol
A=1.5×10−7 s−1
iii. Ea=50 kJ/mol
A=1.9×10−7 s−1
Slowest
Fastest