Warmup (3 minutes) Na 2 CO 3 (aq) + 2HCl (aq)  2NaCl (aq) + CO 2 (g) + H 2 O (l) 1) In the reaction above, identify the compounds whose concentrations or pressures will increase during the course of the reaction, and the compounds whose amounts will decrease as the reaction progresses. 2) What is the purpose of refrigerating milk?

Reaction Rates Demos: Lightsticks and 1,2,3 Blastoff! Have your packet out.

When a glow stick is snapped and shaken it gives off light! I’ll bet you have some questions about this. I sure do! What’s inside that makes them light up? How do they work?

Hydrogen peroxide oxidizes the phenyl oxalate ester, making phenol and an unstable peroxyacid ester (POE). Ester decomposes, forming a cyclic peroxy compound, which decomposes to CO 2, a process which releases energy to the dye. Electrons in the dye atoms jump to a higher level, then fall back down releasing energy (light). What determines how long they last? Let’s discuss collision theory first…

Collision theory: molecules must hit each other hard and be under favorable conditions to react Molecules are always colliding. Atoms SOMETIMES rearrange to form new products (ex. pool). Changing any condition that forces molecules to collide more frequently will increase reaction rate don’t draw

The amount of time that a lightstick lasts (AKA the rate of a reaction!) depends on: 1. Temperature! Increasing temperature increases KE of particles, which move faster and have more frequent and harder collisions…..faster reaction! Extra energy  accelerate the reaction  brighter, (but for a shorter amount of time) Cool the light stick  slow reaction  light will dim. If you want to preserve your light stick for the next day, put it in the freezer -- it won't stop the process, but it will drag out the reaction considerably. 2. Particle Size/Structure of the compounds 3. Presence of a Catalyst? (more on this later)

4. Concentration (aq) or a change in volume or pressure (g) Any change that makes molecules closer together will cause them to collide more frequently

Which molecules in the lightstick “decide” to react first? We recognize that we can't precisely predict the behavior of one molecule but we CAN do this with groups molecules using statistics Maxwell Boltzmann Distribution As temperature increases, the curve will spread to the right but the area under the curve remains the same (always 100% molecules). As T increases, the fraction of molecules with energies greater than the red line increase. The molecules that “decide’ to react first are the ones with enough energy to react. When molecules meet the threshold energy, they have enough energy to react %

There are fancy and nonfancy ways to measure how much phenyl oxalate ester (POE) is left….don’t worry about this too much. If 1/10 (10.0%) of the remaining chemical is used up every 10.0 minutes, calculate the amount of chemical remaining at the end of each 10.0 minute increment. x 20 = (x 10 – 0.100x 10 ) = 81.0 Time (min) mass POE left (mg)

Time (min) mass POE left (mg) Go ahead and graph our data What units should be used to describe the rate at which the POE is being used? rate = ∆ mg/ ∆ min

What is the rate for the first ten minutes? Rate = 10.0mg/ 10.0 min = The POE is decomposing at a rate of 1.00 mg/min during the first 10 minutes Can measure rate as: 1.Rate of disappearance of reactant (usually) 2. Rate of product appearance (sometimes) Units = [ ]/time We can calculate the reaction rate if the [reactants and products] is known

Time (min) mass POE left (mg) Rate ( ∆ mg/ ∆ min) What is the reaction rate for the second ten minutes? ∆ min = 20.0 – 10.0 min ∆ mg = 90.0 – 81.0 = 9.0mg Rate = 9.0mg/10.0 min = mg/min Finish filling in the 3 rd column. What is the average rate during the first 50 minutes of the reaction? Rate = 41.0mg/50.0 min = mg/min What is the average rate during the course of the whole reaction? Rate = 57.0mg/80.0min = mg/min The point? The reaction rate changes during the course of a reaction (curve!)

Catalysts: allow bonds in the reactants to break and form more readily Transition-state theory As molecules approach each other, their orbitals distort each other and bonds weaken This allows bonds to break and reform with other atoms

Energy Reaction coordinate Reactants Products Increase of energy as reactants approach each other Maximum energy when they collide Decrease in energy as products recoil

Energy Reaction coordinate Reactants Products Activation Energy: minimum energy to make the reaction happen Reaction rate depends on the E a in this potential energy profile Activated Complex or Transition State: where old bond is half-broken and new bond is half- formed

Energy Reaction coordinate Reactants Products Catalyst: substance that speeds up reaction without being used up. The reaction goes faster. The overall energy is the same! EaEa It gives reaction a new path, with a lower activation energy.

Pt surface HHHH C HH C HH Catalysts can be enzymes (biology!), or atoms or ions which like to give away or accept electrons. Platinum is the catalyst in our vehicles to break down gas emissions into “greener gases.”

Pt surface HHHH C HH C HH The double bond breaks and bonds to the catalyst. Catalysts can be enzymes (biology!), or atoms or ions which like to give away or accept electrons. Platinum is the catalyst in our vehicles to break down gas emissions into “greener gases.”

Pt surface HHHH C HH C HH The hydrogen atoms bond with the carbon Catalysts can be enzymes (biology!), or atoms or ions which like to give away or accept electrons. Platinum is the catalyst in our vehicles to break down gas emissions into “greener gases.”

Pt surface H C HH C HH HHH Catalysts can be enzymes (biology!), or atoms or ions which like to give away or accept electrons. Platinum is the catalyst in our vehicles to break down gas emissions into “greener gases.”

123 Blastoff! demonstration One of the reactions in rocket propulsion is the reduction of potassium permanganate. Reduction is when a species (ion, compound, etc) gains electrons. Two possible permanganate reduction reactions are shown below: Reaction #1: 8H 3 O + + MnO Fe 2+  5Fe 3+ + Mn H 2 O reduction by iron(II) Reaction #2: 16H 3 O + + 2MnO O 2 2-  2Mn O H 2 O reduction by peroxide Materials Two 6g FeSO 4 solid samples 200ml 3% liquid H2O2 distilled water20 ml 3.0M MnSO 4 50ml 0.02M KMnSO 4 three 10ml graduated cylinders four 125ml Erlenmeyer flasks

Part 1: H 2 SO 4 as a Catalyst 1.Into both Erlenmeyer flasks, dissolve 4g iron(II)sulfate in a few ml of 0.5M H 2 SO 4. 2.Fill one flask to 100ml with distilled water. Fill the other with the sulfuric acid. 3.Measure 10 ml MnO 4 - solution into two different graduated cylinders. Add the MnO 4 - into each flask simultaneously. 3. Observe and record results. Does the reduction of MnO 4 - to Mn 2+ proceed faster or slower in the presence of H 2 SO 4 ?

Part 2: MnSO 4 as a Catalyst 1.Add 100 ml H 2 O 2 solution into two Erlenmeyer flasks. 2.Measure 10 ml MnO 4 - solution into two different graduated cylinders. Add the MnO 4 - into each flask simultaneously. 3. Using the third graduated cylinder, add 10 ml of Mn 2+ solution to just one of the flasks. Does the reduction of MnO 4 - to Mn 2+ proceed faster or slower in the presence of MnSO 4 ?