Q2 – Week 9 – 19-20
week 9
Week of 1/13 – 1/17
1/13 – Monday – period 6/7 – LAB
1. Complete the Genetics Test –
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Spontaneous = dispersion (spreading out) of energy
= Increase in entropy
concentrated source of energy —-> less concentrated source
example: paper burning
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Wood has concentrated source ———> Less concentrated source of energy because
of energy because it was once living energy was released AND smaller particles of
and living things collect energy by matter (CO2 gas and water gas) are moving
building more cells, proteins, DNA, etc away from reaction.
Simplified chemical reaction:
*Notice there are 2 C6H12O6 + 2 Ca + 13 O2 = 17 individual molecules that we started in paper
*Notice there are 2 CaCO3 + 10 CO2 + 10 H2O = 22 individual molecules produced in burning it!
17 particles and some of these are large ——-> 22 particles and most of these particles are particles that are slow moving solids. fast moving gases).
Solids have lower absolute entropy ——–> gases have greater absolute entropy
Energy is being dispersed by the increase of individual molecules (increase of the degrees of freedom) and their ability move faster as gases.
INCREASING THE NUMBER OF INDIVIDUAL MOVING PARTS INCREASES ENTROPY!
Energy was ALSO dispersed because energy ( Energy is written on the product side of the reaction to show that it is produced ) is RELEASED into the surroundings
The heat released by the reaction can make the surrounding molecules move faster (increase their kinetic energy) and DISPERSE!! This leads to and increase in Entropy.
Spontaneous Process – The universe allows things to occur IF ENERGY is dispersed through Energy (heat) being released and increasing the number of free molecules = increase in Entropy!
If a process is Spontaneous it gives us FREE ENERGY to do things!
NOW if a process is spontaneous the reverse process process MUST be non- spontaneous, which means energy is being organized and concentrated AND THAT REQUIRES A CONSTANT INPUT OF ENERGY. THink about it !! Is the reverse of burning spontaneous? Have you ever seen CO2 and water vapor come together to make paper?? ONLY IN PHOTOSYNTHESIS!!!! Which requires a constant energy (LIGHT!) and thus the making of wood (or a tree growing) from photosynthesis is Non-spontaneous because energy is being concentrated.
1/13 – Monday Homework:
1. Make one more submission form this weekends form (Metabolism 1)
2. Read the my notes above regarding the burning of paper AND Connections below:
It might be helpful to re-read the notes I posted Under last Friday.
3. Watch the lecture.
a) watch the whoosh demonstration.
Read the notes for the demonstration
b) gummi bear demo.
Read the notes for the demonstration
4. Complete the form using information below and the Vsauce Video:
*Connections:
Most of the all the organisms on the earth including plants and animals require glucose, C6H12O6 (s) for Free Energy.
C6H12O6 (s) + 6 O2 (g) ——> 6 CO2 (g) + 6 H2O (g) + Energy
7 molecules ——> 12 molecules
A concentrated source of energy ——> To a less concentrated source
We use this spontaneous reaction to provide the Free Energy to Force non-spontaneous reactions of life (building complex organized structures).
Spontaneous Reaction = Exergonic Reaction = an increase in Entropy = favorable pathway
Lecture – I did have some problems with one demo (lol) it wound up being non-spontaneous due to the alcohol have too much water mixed with it. Good times!!
Today’s demo: Whoosh bottle – this one better
Whoosh bottle Demo Notes:
Once the I have the alcohol in the gas phase, which has now mixed with the oxygen in the air inside the container I ignite the flammable mixture by providing a spark and the combustion reaction begins. This is an example of an spontaneous reaction that releases energy exothermically, (exergonic reaction). Here is the chemical change that takes place:
2CH3OH(l) + 3O2(g)
→
2CO2(g) + 4H2O(g) + Energy
Alcohol Oxygen carbon dioxide water
(l) = liquid, (g) = gas
Notice the Coefficients that balance the reaction due to the Law of Conservation of Mass. We have the same number of Carbon (C), Hydrogen (H), and Oxygen (O) atoms on both sides. This is chemical change due to the fact that there are new substances (compounds) produced which means bond have been broken and reformed.
Notice that initially 3 gas molecules (
3O2(g)
) are used with 2 liquid molecules .
These are called Reactants as they on the left side of the chemical reaction and this is what we start with before the chemical reaction begins.
The products are the chemicals that are on the right side and they include 6 gases (
2CO2(g) + 4H2O(g) ). So 3 gas molecules and 2 liquid molecules become 6 gas molecules . The entropy is increasing and the chemical reaction is spontaneous.
Gummy Bear Demo Notes:
In this demonstration potassium chlorate – K2ClO3 was heated to a liquid demonstrating an endothermic phase change and then decomposed into O2 and KCl. The oxygen reacted with the sugar in the Gummi Bear exothermically. KClO3(s) + heat —> KClO3(l)
2KClO3(l) + heat —> 2 KCl(s) + 3 O2(g)
C12H22O11 + 35/2 O2 —> 12CO2 + 11H2O + heat (5635 kJ)
Vsauce video:
GIVE THIS VIDEO A CHANCE!! It appears initially that it has nothing to do with what we are learning but THEN IT WILL HAPPEN!!
The form below:
I know that some may be really lost BUT I promise it will be crystal clear after tomorrow when I redo these demo’s and Teach this topic in class. I will look like a hero because you will have struggled a bit at home and I will (hopefully) make sense of all of this in class.
Picture of some of the chemical reactions (Metabolism) in our body:
Notice how they are interconnected!
End of Monday..
1/14 – Tuesday – period 7 – Academic Study hall
Academic Study hall – complete Genetics Test is you need.
period 8-
1: Completed 1st page class worksheet – Gibbs free Energy and Entropy.pdf
2: Demos (Dancing Gummy Bears) – Note-taking with worksheet handed out yesterday.
3: Completed side 2 – Completed 1st page class worksheet – Gibbs free Energy and Entropy.pdf
Reviewed the Free Energy Diagrams –
-focused on the energy barrier/ activated complex / How enzymes lower the energy barrier
Every chemical reaction requires collision that are effective = Effective Collisions
effective collisions require 2 things:
1. Energy to overcome repulsive forces of electrons (that are on the outside of the molecules) . ELECTRONS FROM ONE REACTANT REPELS THE ELECTRONS FROM THE OTHER SINCE ELECTRONS ARE NEGATIVE AND LIKE CHARGES REPEL.
Thus as two reacting molecules start to collide they start to repel until they reach a maximum energy of repulsion = peak energy = Activated Complex. The energy needed to overcome the activated complex peak is called Activation Energy (Ea).
Every chemical reaction exergonic or endergonic must overcome the energy barrier with Ea.
2. Molecules have to collide in areas that can bond and not in area that it cannot. Thus molecules must collide with the correct orientation ALONG with Ea.
A couple of points to keep straight.
A reaction that is non-spontaneous by itself can be made spontaneous is it coupled with a spontaneous process.
Free energy is based on Heat coming or going AND the entropy of the system (the particles).
You can have the entropy of the surrounding (usually gas molecules moving ) and you can have entropy of the system (particle changes).
1/14 – Tuesday – Homework :
1. Please read today’s notes below the form.
2. Complete page 5 of the notes packet (its Titled Gummy Demo) –
*skip the activated complex in the Energy Diagram
I will explain that tomorrow
3. review page 5 with key below – I will review this tomorrow in class.
KClO3 (s) + FREE ENERGY —-> KClO3 (l)
The chemical reaction by itself is endergonic but when combined with the chemical reaction in the torch (coupling) the above reaction with the reaction in the torch IS SPONTANEOUS!!
SOME of the Free Energy of the Torch reaction went into the above reaction but MOST OF IT went into the surrounding this the entropy of the universe increased and the entire coupled process is Spontaneous! Look at the Review of the Gummy Bear demonstration – diagram below.
4. Please make a second submission to last night Vsauce Form.
5: Please complete the following form based on Chapter 8. You will need to read parts
of Chapter 8 in the text to answer the form below.
Today’s Notes:
Exergonic = Spontaneous = self sustaining reactions/process = entropy of universe increases
Creates (releases) Free Energy from a concentrated energy source that can be used to do work.
ΔG = negative (Free energy is decreasing as the reaction/process proceeds). Riding the pony!
Endergonic = Nonspontaneous = requires a constant input of energy = entropy of the universe decreases
Uses (absorbs) Free Energy to make a concentrated energy source.
ΔG = positive (Free energy is increasing as the reaction/process proceeds). Carrying the pony!
Entropy (ΔS )= measure of the amount of dispersed energy.
And according the 2nd Law of Thermodynamics the ΔSuniverse must increase if there is a
pathway for the process to proceed = spontaneous reactions.
The ΔSuniverse is measured by ΔG (Free Energy).
The Entropy ΔSuniverse is affected by two factors
There are two ways that energy can be “dispersed” or released.
1. Heat or thermal energy is released into the surroundings. ΔH = heat of reaction
This thermal energy will increase the temperature of the surroundings and increase the motion of
surrounding molecules. This increased motion will make these surrounding molecules “move away”
and disperse their motion energy “away” from the system.
ΔH = negative if HEAT energy is released – (increases ΔSuniverse )
ΔH = positive if HEAT energy is absorbed – (decreases ΔSuniverse )
2. The degrees of freedom of the particles or molecules increases. ΔS = entropy of particles
The chemical reaction or physical process increases the number of moving “parts” so that motion
energy is dispersed as the chemical or physical process proceeds.
ΔS = positive if degree of freedom increases for molecules as process proceeds.
ΔS = negative if degree of freedom decreases for molecules as process proceeds.
To measure a if the Entropy ΔSuniverse is decreasing or increasing we use Gibbs Free Energy Formula:
ΔG = ΔH – TΔS
IF ΔG = negative then the Entropy ΔSuniverse is increasing = Spontaneous
IF ΔG = positive then the Entropy ΔSuniverse is decreasing = Non – Spontaneous
Review of the Gummy Bear demonstration –
End of Tuesday
1/15 – Wednesday – period 6/7 –
Every chemical reaction requires collision that are effective = Effective Collisions
effective collisions require 2 things:
1. Energy to overcome repulsive forces of electrons (that are on the outside of the molecules) . ELECTRONS FROM ONE REACTANT REPELS THE ELECTRONS FROM THE OTHER SINCE ELECTRONS ARE NEGATIVE AND LIKE CHARGES REPEL.
Thus as two reacting molecules start to collide they start to repel until they reach a maximum energy of repulsion = peak energy = Activated Complex. The energy needed to overcome the activated complex peak is called Activation Energy (Ea).
Every chemical reaction exergonic or endergonic must overcome the energy barrier with Ea.
2. Molecules have to collide in areas that can bond and not in area that it cannot. Thus molecules must collide with the correct orientation ALONG with Ea.
1: Light stick Demo – proved the collision theory of molecules.
2. Nitrogen (l) / balloon – proved motion of gas molecules
3. Rate of reaction – Rate of metabolism Demo – Radio
In all 3 demonstrations Energy is being driven from a system spontaneously by the coupling of a spontaneous process (boiling of the liquid nitrogen) with a non-spontaneous process.
1. Note- taking (above) with worksheet
1/15 – Wednesday – Homework :
1. Be spontaneous ! Ride the pony! Do not carry the Pony up the hill!
2. Resubmit the Form form Tuesday Night!
End of Wednesday..
1/16 – Thursday – period 7 – Academic Study hall
period 8-
None today..
*Review most incorrect answers with last 2 forms
1. Review the Notes with Gummy Bear Demo.
Relate it to Biological Metabolism:
2. Coupled process —–> into Biological reactions.
Exergonic = catabolic —–> Endergonic – anabolic
breaking down Driven building big molecules
glucose making enzymes
** The ΔG must be negative enough to drive the positive Endergonic process!
4. Complete the notes for the Whoosh and the Cool reaction.
Cool reaction demo!
5. Introduction of Gibbs Free Energy equation:
Always Rule, Never Rule, Sometimes Rule
6. Solidification (hand warmer) demo Reviewed – started.
Cool Uplifting Chemical Reaction Demo:
Solidification Demo:
1/16 – Thursday Homework-
1. Complete the last page of the notes packet that we were filling out in class. Please note that in class I incorrectly filled out the page for the freezing of water. By itself water will not freeze at 20 degrees Celsius. Max was correct. I was thinking about the entire coupled process.
2. Please view the signs lecture and take notes.
2. Complete the Thermo signs lecture.
End of Thursday!
1/17 – Friday period 7, 8 – I will give an academic study hall today.
2. Reviewed the Always Rule, Never Rule, and Sometimes Rule in the Gibbs Free Energy Equation
3. Review of Gummi Bear demo – without ΔH and ΔS values.
*Look at the always rule of the combustion reaction of propane (torch). Explain why not all Free Energy is transferred from one process to another. This is important in ecology as the producers have the greatest
amount of energy in an ecosystem.
4. Review of Cool demo with values.
5. Solidification (hand warmer) demo Reviewed.
Cool Reaction: What is spontaneous and what is non-spontaneous is this demo?
The Entropy ΔSuniverse is affected by two factors
There are two ways that energy can be “dispersed” or released.
1. Heat or thermal energy is released into the surroundings. ΔH = heat of reaction
This thermal energy will increase the temperature of the surroundings and increase the motion of
surrounding molecules. This increased motion will make these surrounding molecules “move away”
and disperse their motion energy “away” from the system.
ΔH = negative if HEAT energy is released – (increases ΔSuniverse )
ΔH = positive if HEAT energy is absorbed – (decreases ΔSuniverse )
2. The degrees of freedom of the particles or molecules increases. ΔS = entropy of particles
The chemical reaction or physical process increases the number of moving “parts” so that motion
energy is dispersed as the chemical or physical process proceeds.
ΔS = positive if degree of freedom increases for molecules as process proceeds.
ΔS = negative if degree of freedom decreases for molecules as process proceeds.
To measure a if the Entropy ΔSuniverse is decreasing or increasing we use Gibbs Free Energy Formula:
ΔG = ΔH – TΔS
IF ΔG = negative then the Entropy ΔSuniverse is increasing = Spontaneous
IF ΔG = positive then the Entropy ΔSuniverse is decreasing = Non – Spontaneous
Hand warmer demo: Is this spontaneous? Why must heat be given off in order to for this solution to become a solid? When has this physical process reached equilibrium?
1/17 Friday Homework –
1. Read me! Look at the 2 reactions below. The first reaction is the phosphorylation of glucose which is required in the 1st step to get Free Energy out of the glucose. As you can see the first reaction is not spontaneous (ΔG is not negative!) and it is the driven by the second reaction that is spontaneous (ΔG is negative). In this coupled process the the overall ΔG is -17 to show that the spontaneous reaction of ATP was spontaneous enough to DRIVE the first reaction. You may have learned that ATP is the energy currency of the body AND THE reason it is needed by all life sustaining chemical reactions is to COUPLE the endergonic reactions of life that require a steady supply of Free Energy. We will learn that we get ATP from the breakdown of glucose in our body (cellular respiration).
2. Complete ATP worksheet with textbook (Chapter 8).
3. Review with the key – There are mistakes in my key. Question 1 b should have 2 phosphates NOT 3 and 7b should be Exergonic NOT Endergonic!
ATP Cycle worksheet .pdf
View Download
4. Genetics Test Corrections!
Test 3 – corrections – due Tuesday 1/21 – Complete in the shared google doc only that I will share with you.! (the key is posted in PowerSchool)
Your effort here will determine how many points you will earn back! I want you to analyze these questions and your incorrect choices.
a) Write the test question number.
b) Write your answer ( you can condense it if was a math or essay question)
c) Write the Correct answer
d) Write the CONCEPT that the question is testing.
e) Show me that you understand this question and THE CONCEPT by writing why the correct choice is the correct answer. (show off here!!)
f) include the vocabulary!
End of Week 9!