E. exothermic F. endothermic G. Activation energy Be able to determine 2. What is necessary for a chemical reaction to proceed (collision theory)
3. 5 ways to change the rate of a reaction
4. Given an energy diagram, be able to determine: How much energy a reaction, or the reverse reaction, needs to proceed 5. Where the transition state is 6.How exothermic or endothermic a reaction is
7. Rate of reaction given reaction time and concentration change • Example: • [HCl] at time = 0: 0.22 M • Start reaction • [HCl] after four seconds 0.32 M • What is the reaction rate? 8. In the energy unit we learned how to predict if a reaction will take place spontaneously. In this unit we determined how to measure how fast a reaction is. What is the relationship, if any, between reaction rate and spontaneity? To consider this, answer each question with a brief explanation - are fast reactions always spontaneous? - if the free energy of a reaction is highly positive, is it a slow reaction? -Are fast or spontaneous reactions dangerous -Are fast reactions exothermic? 22