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3 cards from this section. Quick, good the night before a test.
What is concentration and how does it affect reaction rates?
Think about how many particles are present.
Define activation energy.
It's what must be overcome for a reaction to happen.
What happens to reaction rates when the concentration of reactants increases?
Think about how many particles are available to collide.
True or False: Catalysts are consumed in the chemical reactions they facilitate.
Consider what catalysts do versus what happens to them.
Given a reaction with activation energy of 50 kJ/mol, calculate the rate constant at 298K, and analyze how increasing temperature by 20K alters the rate constant using the Arrhenius equation.
Apply k = A exp(-Ea/(RT)) and calculate separately for 298K and 318K to observe the change.
A solid reactant's size changes from large chunks to fine powder. Describe how this alters the reaction rate with an example.
Consider the collisions happening on the surface and how more area contributes to those collisions.
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