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Physics Electric and Magnetic Fields
Physics Electric and Magnetic Fields
HS PS3-5
HS PS3-5
Biology
LS2-1 Factors Affecting Ecosystems
Page Under Construction
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Chemistry PS1 5 Rate/Kinetics
Project Zero THINKING ROUTINES--see below
Phenomenon--Discover examples of fast reactions Here are a few . . . DO NOT do these at home--the videos include safety equipment: screens, special, non combustible benches and more + correct waste disposal/safe clean-up--NOT HOME EXPERIMENTS
#1 See the combustion of alcohol, magnesium burning in air and lead nitrate and potassium iodide solutions reacting CayerChem
#2 Scroll down this link to see steel wool burning
Chemicool NurdRage
#3 Cesium reacting with water Periodic Videos Prof. Poliakoff
WRITE equations for the reactions--check answers below
Can you think of any SLOW reactions? What are they and do they help us by being slow?
Prior Knowledge/Preview
Being developed
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Aerospace CONNECTIONS:
Applications and examples
Catalysts in Aerospace Washington International School
European Large Logistic Lander Fuel cell NASA
Gemini Fuel Cell -paper given NASM
Catalyst use in ammonia production (scroll down to the video) RSC
Industrial catalysts Lumen Learniing
Corrosion resistance
Rate
Collision theory Washington International School
Energy level diagrams Washington International School
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HS-PS1-5 Matter and its Interactions
Apply scientific principles and evidence to provide an explanation about the effects of changing the temperature or concentration of the reacting particles on the rate at which a reaction occurs.
Collision chemistry
Factors affecting rate of reaction: temperature, concentration
Rate lab equipment:
1: volume of gas produced versus time
2: mass reduction versus time
3: concentration versus time for precipitate to form (obscure an X on a piece of paper under the flask
4. mass of metal deposited at cathode versus time
5: volume of gas produced versus time
6: Light affecting the rate of reaction
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For ONE (or more!) piece of equipment (#s 1 through 5 above),
What chemical reaction can you think of, which could be used to measure the rate of the reaction with your chosen piece of equipment from the diagram above?
Research, if needed!
Inquiry science
Online activity
Under development
LAB activities follow all safety guidelines linked above
and in the activity
Lab #1 Temperature affecting rate
Lab #2 Concentration affecting rate and Washington International School
Lab #3 Surface area and rate NASA
Lab #4 Iodine clock reaction Nuffield Foundation
Lab EXTRA Rate Determining Step Washington International School
EXTENSION material for the curious
Rate and ozone depletion
Maxwell-Boltzmann distribution curves WIS
Driving lessons in Mercury and Gemini capsules--including power supply (launch at 1h 15m 30s) Scott Manley
THINKING ROUTINE
Close looking
Look VERY closely at the diagrams A, B and C on the right
How can you relate to them better?
Try to turn one of them into a hands-on model with simple, everyday (safe) materials.
How does this help your understanding?
Unsuccessful
collision--at the wrong angle
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Correct direction and forms a reaction intermediate
A
Top diagram--not correct collision direction for reaction
Bottom diagram--reaction occurs A2 + B2 --> 2AB
B
C
Reaction mechanism--here forming free radicals when a covalent bond breaks-there are fast reactions with other free radicals
WORKING ROUTINE
Close looking
Look VERY closely at the diagrams D and E on the right
How can you relate to them better?
How can you describe them in words? Write a list of bullet points to help you do this.
How does this help your understanding?
D
The peak of the graph-activation energy-is reduced with a catalyst. The catalyst forms a different reaction intermediate with a lower activation energy, so that the reaction is faster
E
The Maxwell-Boltzmann distribution curves: the area under each curve is the same but there are different numbers of particles, which have more than the activation energy at different temperatures. The lowest temperature is the line with the highest maximum and fewest particles with the required activation energy-so slowest. At the highest temperature there is the line with the lowest maximum value but the largest number of molecules above the activation energy, EA.
F,G and H are a more complex way of looking at reactions--what is the ORDER of the reaction considering rate/concentration/time.
They are graphical models to help advance understanding by comparing different reactions--interestingly, radioactive decay is first order--where the rate is independent of the initial concentration--it takes a fixed amount of time (the half-life, t1/2) for half of the atoms of the material to decay into another element's atoms/isotope with the loss of alpha or beta particles or gamma rays.
Can you see this from the right-hand G graph?
F
Concentration vs time and rate vs time graphs to identify the order of reaction
Same graphs below combined into two graphs
G
H
FILL IN the table:
Decay of a radioactive material, where the nucleus of one element radioactively decays into another, is a FIRST ORDER reaction. Here, the time taken for half of the material to decay, the half-life, is constant
The Arrhenius equation and the plot of ln k versus the reciprocal of the temperature