OCO AP Chemistry 1 Class 13 (Mod 5).pptx

Kinetics

1. AP Chemistry – Semester 1 Class 13 – Ki netics

2. Questions from Previous Work

3. Energy Diagrams

4. Activation Energy

5. Factors that Affect Reaction Rate

6. Catalysts

7. Rate Law shows relationship of the reaction rate to the concentrations of each reactant A + B --> C R = k [A] n   [B] m R: reaction rate [A] and [B]: concentrations of A and B k: specific rate constant n and m: orders of reaction in with respect to A and B

8. Determining the Rate Law from Experimental Data 2ICl + H 2 --> I 2 + 2HCl Trial Concentration of ICl (M) Concentration of H 2 (M) Instantaneous Reaction Rate (M/s) 1 0.25 0.25 0.0102 2 0.25 0.50 0.0204 3 0.50 0.50 0.0408

9. Determining the Rate Law from Experimental Data 2ICl + H 2 --> I 2 + 2HCl Trial Concentration of ICl (M) Concentration of H 2 (M) Instantaneous Reaction Rate (M/s) 1 0.25 0.25 0.0102 2 0.25 0.50 0.0204 3 0.50 0.50 0.0408 R = k [ ICl ] n [H 2 ] m R = k [ ICl ] 1 [H 2 ] 1

10. Determining the Rate Law from Experimental Data 2ICl + H 2 --> I 2 + 2HCl R = k [ ICl ] n [H 2 ] m Solve for k using data from any 1 trial k = R /([ ICl ] n • [H 2 ] m k = 0.0102 /([0.25] 1 • [0.25] 1 = 0.16 1/M•s Trial Concentration of ICl (M) Concentration of H 2 (M) Instantaneous Reaction Rate (M/s) 1 0.25 0.25 0.0102 2 0.25 0.50 0.0204 3 0.50 0.50 0.0408 R = k [ ICl ] n [H 2 ] m R = k [ ICl ] 1 [H 2 ] 1

11. AP Chemistry – Semester 1 Class 13 – Kinetics