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Studies reaction rates and mechanisms.
In terms of concentration change over time.
Concentration of A decreases over time.
Change in concentration over time.
Rate at a specific moment, found using a tangent.
Collisions between reactants.
Effective collisions result in product formation.
Minimum energy needed for a reaction to occur.
Higher temperatures increase kinetic energy and collision frequency.
Larger surface area increases contact and reaction speed.
Higher concentration increases the rate due to more collisions.
Lowers activation energy and speeds up the reaction.
Homogeneous reactions occur in one phase; heterogeneous in multiple phases.
Rate increases due to higher concentration of gas particles.