Q3 : Week 7 – 3/20 – 3/24
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Jump to: Monday Homework
d) To derive Gibb’s Free energy (∆G) and how it measures the ∆S universe by using system’s values
Period 2/3a, 4:
3. Review of the 2nd FRQ
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a) Micro lesson on Specific heat and heating and cooling curves problems.
4. Today we start our discussion towards the Second Law of Thermodynamics: No one got to this in class.
Use the follow along by taking notes. If you want to use the Thermo pages I gave you last week or your
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TODAY’s NOTES:
1. Review of Laws of Thermodynamics:
The second Law tell us that entropy ∆S of the universe must increase for a spontaneous process.
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If you notice in your Thermodynamic tables there are 2 other thermodynamic quantities, S(absolute) and ∆G.
We can calculate the ∆S and ∆G through tablature by using the following formulas. Also ∆G can be determined through a formula that measures the Universe’s Entropy Change by just looking at the system!
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Thermodynamics: The end of it all!!!
Ion Dipole or Molecule ion IMF of a Salt Solution- p can waters compete with the Ionic Bonds of the ions in the crystal lattice. Is the Lattice energy too large?
Heating Curve Demo- The potential Energy changes at the phase diagrams can be measured by enthalpy!
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3/20 – Monday’s Homework: –
STEP #1 (all classes)

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3: The signs lecture:
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3/21 – Tuesday – B Day – 2, 3b/4 Lab
b) To derive Gibb’s Free energy (∆G) and how it measures the ∆S universe by using system’s values
c) To identify the values of ∆G in terms of a spontaneous and nonspontaneous process.
d) To identify an entropy or enthalpy driven reaction.
e) To calculate the ∆G and ∆S through tablature.
Period 2,3b/4:
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f) Values of ∆G, demos
Thermodynamics: The end of it all!!!
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TODAY’s NOTES:

Sometime Rule Demo: Hand warmers
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 .
The products (2CO2(g) + 4H2O(g) ) are the chemicals that are on the right side and they include 6 gases. So 3 gas molecules and 2 liquid molecules become 6 gas molecules .
The entropy is increasing and the chemical reaction is spontaneous.
Uplifting COOL DEMO NOTES:
Whoosh Bottle Demo: (always rule!)
A COOL Demo!: (Entropy Driven!)
3/21 – Tuesday’s Homework: –
1. Please complete the FRQ as a test to hand in tomorrow:
THermo Test 1 – 7a – THermo Test 1.pdf
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2. Please view the lecture below on the derivation. I am asking that you follow along and try to pick up the major understandings of the derivation.
2: Nonstandard ∆G Derivation (this gets us to equilibrium!!!!)
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Additional Resource: Classroom lecture reviewing Last nights Form:
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3/22 – Wednesday – A Day – 2/3a Lab, 4
a) To derive the non-standard ∆G equation
b) To write the Law of Mass Action (@ equilibrium, Keq and when not at equlibrium Q)
c) To calculate Gibbs free energy with tablature.
Period 2/3a,4:
1. Review Yesterdays Demo, especially the “uplifting demo” in terms of the signs in the form and the ∆G changes and that we could also calculate the Standard ∆G using tablature also.
3. Derivation Review of the NON-Standard ∆G.
Thermo 9 Notes for nonstandard.pdf
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NONstandard Form most wrong 2019 form p.pdf
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Thermodynamics: The end of it all!!!
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TODAY’s NOTES:

Nonstandard Gibbs Free Energy Lecture with form review:
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3/22 – Wednesday Homework:
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2. Non-standard Gibbs Free energy formula review:
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3/23 – Thursday – B Day – 2, 3b/4 Lab
c) To identify changes in equilibrium at different temperatures that cause shifts.
Period 2,3b/4:
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3 . Review of the last 2 questions of Tuesday form –
NONstandard Form most wrong 2019 form p.pdf
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∆G formula that ties spontaneity with equilibrium (Keq).
5. Using our new formula of ∆G that relates to Keq (equilibrium constants):
The value of ∆G depends on the value of the Keq.
LeChateliers Principle!
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TODAY’s NOTES:

Today’s Lecture Non standard ∆G to Keq
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3/22 – Thursday Homework: –
*Period 3/4 does not have to do 1 and 2!
1. Read the posted Notes that are in the separate page in 3rd quarter:
https://mrgrodskichemistry.com/non-std-gibbs-equilibrium-notes/
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2: Lecture for the form(up to question 27:00 min mark only):
3: Equilibrium Tank Demo-
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__________________________________________________________________ Jump to: Friday Homework / top 3/23 – Friday – A Day – 2/3a Lab, 4
a) To identify the shifts in Le Chateliers Principle are actually the spontaneity changes that occur when you compare Q vs. Keq.
b) To recognize that Temperature stress on a reversible reaction actually moves the equilibrium position. Equilibrium temperature sensitive.
c) To identify the basic concepts of equilibrium.
d) Demonstrate the common ion effect, and temperature changes that affect pH.
Period 2,3a/4:
1. Slides 61 – 62 – to review the shifts due to Q vs, K and the size of the Keq with size of the ΔGo
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TODAY’s NOTES:


Brown clear
Review of the Last nights form – questions 1 – 5-
Class lecture (From 27:00 min and to the end):
∆G Derivation to determine how Temperatures affects an Exothermic or Endothermic
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3/24 – Weekend Homework: –
1. Please complete the Le Chateliers Principle Side 1 and review with the key. Think while you are doing the worksheet, “What are we doing with Q in relation to K? “When does Keq move in relation to Q?
THis worksheet should look familiar and was given out earlier this week.
Homework Lecture: Equilibrium Basics
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