Consider the concentration cell:
a. Label the anode and cathode.
b. Indicate the direction of electron flow.
c. Indicate what happens to the concentration of Pb2+ in each half-cell.
Monday January 11, 2016 1 Important Information: Midterm #1 Wednesday, January 20 Lecture 4: Mechanisms and Catalysts Collision Theory ● molecules generally collide before a reaction can occur ● the more molecules → the more collisions (more opportunities for the reaction to happen) → this is why concentration is related to rates ● however, the collisions must have the correct orientations and energy in order for the reaction to be successful ● increasing the temperature gives the reactant molecules sufficient energy to react in a forward reaction nd a reverse reaction ● at equilibrium, the rate forward = the rate reversed Temperature and Reaction Rate Ea/RT ● k = Ae ○ E = activation energy (stays constant) a ○ R = 8.314 J/molK ○ T = Kelvin ○ = 3/2RT ○ RT = the average energy of the molecules compared to E a ○ A = frequency factor → the frequency of attempts and success rate of collisions ● larger activation energy means smaller k which means slower rate ● larger temperature means bigger k which means faster rate Clicker Question #1 Which reaction would you expect to have the smallest orientation factor a.) H(g) + I(g) → HI(g) b.) H2(g) + 2g) → 2HI c.) HCl (g) + HCl (g) → H 2(g) + C2(g) d.) they would all be the same as long as they’re at