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4 cards from this section. Quick, good the night before a test.
What is activation energy?
Think about the energy barrier needed for a reaction to happen.
Define collision frequency.
Consider how often reactant molecules meet each other.
What does the Collision Theory state about reactions?
Think about what makes a collision 'effective'.
True or False: Higher temperature decreases the reaction rate.
Recall how temperature affects molecular motion.
Given that the collision frequency for a reaction is 3.5 x 10^9 collisions per liter per second, and the activation energy is 50 kJ/mol at a certain temperature, calculate the rate of the reaction if the temperature is raised by 10 K.
Don't forget to convert the activation energy into J/mol and use the appropriate values for R.
Discuss how increasing pressure in a gaseous reaction influences collision frequency and the rate of reaction.
Think about how the volume change relates to pressure and how this impacts molecular interactions.
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