Search found 58 matches
- Tue Mar 13, 2018 8:22 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Steady-State v Pre equilibrium?
- Replies: 2
- Views: 420
Re: Steady-State v Pre equilibrium?
It explains it well in the book. What I understood from it, is that steady state is assuming that the intermediate formed in the reaction mechanism stays at a constant, low concentration. Most times when you write the rate law for each elementary reaction, and then combine them to form the overall r...
- Tue Mar 13, 2018 8:14 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Test 1 #3
- Replies: 4
- Views: 1244
Re: Test 1 #3
A change in volume means expansion work is occurring!
- Tue Mar 13, 2018 8:10 pm
- Forum: Zero Order Reactions
- Topic: Applications
- Replies: 2
- Views: 546
Re: Applications
I don't think we need to memorize anything.
Just if we plot the [A] vs time, and we get a linear line. Then we know that it is zero order
Just if we plot the [A] vs time, and we get a linear line. Then we know that it is zero order
- Tue Mar 13, 2018 8:08 pm
- Forum: Calculating Work of Expansion
- Topic: Irreversible and reversible
- Replies: 1
- Views: 286
Re: Irreversible and reversible
From my notes "reversible work does more work because pushing against a constant P but in irrversible work, you are pushing against a smaller P."
I don't know if that helps
I don't know if that helps
- Tue Mar 13, 2018 8:00 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: entropy in reversible/irreversible processes
- Replies: 1
- Views: 491
Re: entropy in reversible/irreversible processes
When calculation the change in entropy we use the basic equation of:
ΔS= q(rev)/T
I remember reading in the book that we assume all the work done is reversible when we use work to calculate ΔS. (ΔU=0, so q=-w)
ΔS= q(rev)/T
I remember reading in the book that we assume all the work done is reversible when we use work to calculate ΔS. (ΔU=0, so q=-w)
- Tue Mar 13, 2018 7:56 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Bomb Calorimeter
- Replies: 2
- Views: 626
Re: Bomb Calorimeter
A bomb calorimeter does mean there is no change in volume (ΔV=0). A bomb calorimeter is an isolated system, meaning that there is no heat transfer between the the system (bomb calorimeter) and surrounding. And the surrounding isn't doing work on the system, nor is the system doing work on the surrou...
- Tue Mar 13, 2018 7:50 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Isobaric
- Replies: 1
- Views: 376
Re: Isobaric
Isobaric means constant P. ΔU=w + q
At constant P, the change in heat is equal to the change in enthalpy by definition.
At constant P, w= -P(ex)ΔV.
So, the ΔU= ΔH -P(ex)ΔV in isobaric conditions.
At constant P, the change in heat is equal to the change in enthalpy by definition.
At constant P, w= -P(ex)ΔV.
So, the ΔU= ΔH -P(ex)ΔV in isobaric conditions.
- Tue Mar 13, 2018 7:46 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Pre-Equilibrium Method Conditions
- Replies: 2
- Views: 368
Re: Pre-Equilibrium Method Conditions
Yeah, I agree with the above post. In this way, a lot of product from the first step will be produced and not used up until there is sufficient energy for the second, slower reaction.
- Mon Feb 19, 2018 5:43 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Determining the sign of a cell potential
- Replies: 1
- Views: 289
Determining the sign of a cell potential
In the attached pictures, the textbook is using the standard hydrogen electrode to determine the standard cell potentials of different electrodes. How did they determine one to be positive and one to be negative? I understand that if the cathode is on the right of the cell, then the cell potential i...
- Wed Feb 14, 2018 2:16 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Delta S(tot)
- Replies: 5
- Views: 1269
Re: Delta S(tot)
Varsha Sivaganesh 1A wrote:Also, when the reaction is irreversible, Ssurroundings = 0.
I don't think that's true.
- Tue Feb 13, 2018 7:38 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: UA Karen Week 4 #6 [ENDORSED]
- Replies: 1
- Views: 408
UA Karen Week 4 #6 [ENDORSED]
A sample of 1 mol of gas initially at 1 atm and 298K is heated at constant pressure to 350K, then the gas is compressed isothermally to its initial volume and finally it is cooled to 298K at constant volume. Which of the following values is 0? a. ΔSsurr and ΔG b. ΔSsys and ΔSsurr c. q and w d. W e. ...
- Mon Feb 12, 2018 11:43 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: 11.83
- Replies: 4
- Views: 619
Re: 11.83
^^ Yes! So did I, would it be wrong to use ∑∆G(products)-∑∆G(reactants)?
- Mon Feb 12, 2018 10:18 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Midterm w18 -Last subject?
- Replies: 2
- Views: 483
Re: Midterm w18 -Last subject?
We are meant to know the entire chapter 11. The new sections are 11.3 and 11.11-11.13.
The other parts of chapter 11 were covered in chem 14a.
Electrochemistry is not on the midterm, so you're right no redox reactions.
The other parts of chapter 11 were covered in chem 14a.
Electrochemistry is not on the midterm, so you're right no redox reactions.
- Mon Feb 12, 2018 6:30 pm
- Forum: Third Law of Thermodynamics (For a Unique Ground State (W=1): S -> 0 as T -> 0) and Calculations Using Boltzmann Equation for Entropy
- Topic: Boltzmann Equation
- Replies: 3
- Views: 696
Re: Boltzmann Equation
Oh, I think I can answer my own question lol. When you have an increase in thermal entropy due to an increase in temperature, the system is allowed more possible configurations or mircostates. So that's how it takes into account thermal entropy. With an increase in temperature, there is an increase ...
- Mon Feb 12, 2018 6:28 pm
- Forum: Third Law of Thermodynamics (For a Unique Ground State (W=1): S -> 0 as T -> 0) and Calculations Using Boltzmann Equation for Entropy
- Topic: Boltzmann Equation
- Replies: 3
- Views: 696
Boltzmann Equation
From my understanding, I thought Boltzmann's equation was used to calculate only the positional entropy with out taking into account the thermal entropy. So ideally, if there is any positional entropy left at K=0. However, in the book it says that the Boltzmann formula enables us to calculate the ab...
- Mon Feb 12, 2018 6:12 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Heat Capacity at constant P for a diatomic ideal gas
- Replies: 2
- Views: 497
- Mon Feb 12, 2018 5:54 pm
- Forum: Calculating Work of Expansion
- Topic: Free Expansion
- Replies: 2
- Views: 496
Re: Free Expansion
No work is done in a free expansion, thus w=0. If it was a isothermal free expansion, you can go on to say delta U= 0. So that w=-q. since w=0, q=0. You can go on even further to say whether its a irreversible or reversible process. If it is a reversible process, then the process is at equilibrium, ...
- Mon Feb 12, 2018 5:50 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Extensive vs Intensive
- Replies: 3
- Views: 589
Re: Extensive vs Intensive
So for heat capacity, the more substance you have the more heat is required to raise it by 1 degree C.
However, for specific heat capacity, it does not take into account how much substance you have because it is the heat required to raise 1 gram of a substance by 1 degree C.
However, for specific heat capacity, it does not take into account how much substance you have because it is the heat required to raise 1 gram of a substance by 1 degree C.
- Mon Feb 12, 2018 5:44 pm
- Forum: Calculating Work of Expansion
- Topic: Free Expansion
- Replies: 4
- Views: 662
Re: Free Expansion
In an isothermal, reversible free expansion, delta S tot= 0 because it is an equilibrium.
So, delta S sys= -delta S surr
So, delta S sys= -delta S surr
- Mon Feb 12, 2018 5:41 pm
- Forum: Calculating Work of Expansion
- Topic: Free Expansion
- Replies: 4
- Views: 662
Re: Free Expansion
^^ that is in an irreversible isothermal free expansion
- Mon Feb 12, 2018 5:40 pm
- Forum: Calculating Work of Expansion
- Topic: Free Expansion
- Replies: 4
- Views: 662
Re: Free Expansion
There is no work down on a free expansion. When you are looking at an isothermal free expansion, you know that delta U= 0. So that means -w=q. We just said that there is no work done on a free expansion, so both q & w would equal 0. Thus no heat transferred into the surroundings, so the entropy ...
- Mon Feb 12, 2018 5:36 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Heat Capacity at constant P for a diatomic ideal gas
- Replies: 2
- Views: 497
Heat Capacity at constant P for a diatomic ideal gas
What is the heat capacity at constant P for a diatomic ideal gas?
I know C(p) is 5/2R for a monoatomic ideal gas.
I know C(p) is 5/2R for a monoatomic ideal gas.
- Mon Feb 12, 2018 5:35 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Isochoric Conditions
- Replies: 1
- Views: 373
Isochoric Conditions
In isochoric conditions, the change in V is constant/zero. Thus, that means there must be a change in P. However, we can calculate the change in enthalpy by using this formula: delta H= nC(p)delta T In the formula we are assuming constant P, but that isn't the case right? Can someone explain that to...
- Sun Feb 11, 2018 7:29 pm
- Forum: Third Law of Thermodynamics (For a Unique Ground State (W=1): S -> 0 as T -> 0) and Calculations Using Boltzmann Equation for Entropy
- Topic: Delta S total
- Replies: 2
- Views: 450
Re: Delta S total
When a reaction is at equilibrium or when a reaction is reversible. The delta S total = 0. So delta S surroundings= -delta S system
- Sun Feb 11, 2018 7:22 pm
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: 9.35
- Replies: 2
- Views: 542
9.35
Container A is fi lled with 1.0 mol of the atoms of an ideal monatomic gas. Container B has 1.0 mol of atoms bound together as diatomic molecules that are not vibrationally active. Container C has 1.0 mol of atoms bound together as diatomic molecules that are vibrationally active. The containers all...
- Wed Jan 24, 2018 10:27 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Changing the energy of a system
- Replies: 6
- Views: 682
Re: Changing the energy of a system
When you add more of a substance into the system, you are increasing the internal energy by increasing the potential energy.
Remember that internal energy is equal to KE + PE.
Remember that internal energy is equal to KE + PE.
- Wed Jan 24, 2018 10:26 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: What is the pressure value for standard states?
- Replies: 2
- Views: 423
Re: What is the pressure value for standard states?
1 bar is approx. 1 atm!
They are interchangeable.
They are interchangeable.
- Sun Jan 21, 2018 9:08 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Open System
- Replies: 16
- Views: 2228
Open System
What are three ways you can increase the internal energy?
(chap 8, excerise 2)
(chap 8, excerise 2)
- Sun Jan 21, 2018 7:04 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Heating/Cooling A System
- Replies: 4
- Views: 586
Re: Heating/Cooling A System
I think the only way you can add energy to an open system is by adding or removing the amount of substance.
For example, adding 1 gram of glucose to a system with 9 grams of glucose increases the potential energy.
For example, adding 1 gram of glucose to a system with 9 grams of glucose increases the potential energy.
- Thu Jan 18, 2018 9:25 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: 8.41
- Replies: 3
- Views: 524
8.41
A 50.0-g ice cube at 0.0 C is added to a glass containing 400.0 g of water at 45.0 C. What is the fi nal temperature of the system (see Tables 8.2 and 8.3)? Assume that no heat is lost to the surroundings. I understand that q(ice)=-q(water) So i imagined that we would solve it like this m(ice) x C...
- Thu Jan 18, 2018 10:16 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Bond Breaking or forming
- Replies: 5
- Views: 572
Re: Bond Breaking or forming
You would have to compare bonds of the reactants with bonds of the products.
Another way to solve for the heat of the reaction, would to break ALL the bonds of the reactants and form all the bonds of the products.
This way you won't miss any bonds, but it is a bit more math!
Another way to solve for the heat of the reaction, would to break ALL the bonds of the reactants and form all the bonds of the products.
This way you won't miss any bonds, but it is a bit more math!
- Wed Jan 17, 2018 10:57 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Specific Heat Capacity
- Replies: 5
- Views: 2029
Re: Specific Heat Capacity
Perhaps it works best with the scope of this class.
A diluted solution might not significantly differ in its specific heat compared to the pure solvent for it to be taken into account.
A diluted solution might not significantly differ in its specific heat compared to the pure solvent for it to be taken into account.
- Wed Jan 17, 2018 10:55 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Heating/Cooling A System
- Replies: 4
- Views: 586
Heating/Cooling A System
In class today, Dc. Lavelle said that there are three ways to change the energy of a system. One of the ways was to heat or cool the system and he specifically referred to closed systems. Can this idea be used on open systems as well? Or would the added heat be released to the surroundings bc it isn...
- Wed Jan 17, 2018 10:50 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: 8.25
- Replies: 2
- Views: 218
Re: 8.25
Yes! They were giving us the change in temperature. The change in temperature will be the same in Celsius or K.
- Wed Jan 17, 2018 10:47 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Cm
- Replies: 3
- Views: 360
Re: Cm
Molar heat capacity! with units: J/(mol K)
- Wed Jan 17, 2018 10:46 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Bond Breaking or forming
- Replies: 5
- Views: 572
Re: Bond Breaking or forming
Bond formation is always exothermic, so a negative H. Bond breaking is endothermic, so a positive H. When looking at a reaction, you must draw all the lewis structures of the reactants and products to understand which bonds are broken and which are newly formed. We do this to calculate the heat of t...
- Wed Jan 17, 2018 10:42 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Enthalpy vs Standard Enthalpy
- Replies: 1
- Views: 284
Re: Enthalpy vs Standard Enthalpy
Enthalpy is the heat released or absorbed by a system at constant pressure. ΔH Standard enthalpy has the same definition, however it is measure enthalpy of objects in their standard states.ΔH° Standard states for a liquid, solid, and gas occur at 1 bar, typically at 25C° For solutions the standard s...
- Sat Dec 09, 2017 8:45 pm
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Strong Bases? [ENDORSED]
- Replies: 2
- Views: 720
Strong Bases? [ENDORSED]
I know the rules regarding what makes a strong acid (binary or oxyacid).
Did we go over any rules on what makes a strong base?
Is it right to think that it's conjugate acid must be stable and weak relatively?
Did we go over any rules on what makes a strong base?
Is it right to think that it's conjugate acid must be stable and weak relatively?
- Sat Dec 09, 2017 1:04 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Exothermic Reaction
- Replies: 3
- Views: 493
Re: Exothermic Reaction
You can think of heat as a reactant in exothermic reactions!
- Sat Dec 09, 2017 1:00 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: calculating pH
- Replies: 3
- Views: 419
Re: calculating pH
He was referring to if you add a small quantity of a weak acid and you calculate the pH/ [H3O+], you'll get what looks like a strong base. He was saying that should make you question it because why would adding a small amount of weak acid result in a strong base? So, he brought of the point that the...
- Sat Dec 09, 2017 12:51 pm
- Forum: Lewis Acids & Bases
- Topic: Lewis Acids/Bases vs Bronsted Acids/Bases
- Replies: 3
- Views: 493
Re: Lewis Acids/Bases vs Bronsted Acids/Bases
When I think of Lewis, I think of electrons because of the lewis structures we've been doing. So, I know that lewis acids/bases are concerning electrons. Lewis acids accept electrons and lewis bases donate electrons. Bronsted acids/bases are what I typically think of when I think of acids and bases-...
- Sat Dec 09, 2017 12:48 pm
- Forum: Balancing Chemical Reactions
- Topic: Fundamentals J
- Replies: 2
- Views: 452
Re: Fundamentals J
When you write out the complete ionic equation you include all the species of that reaction. You might notice that you will have unchanged species on either side. So, when you write the net ionic equation, you cross off those unchanged species on either side because they aren't directly involved in ...
- Sun Dec 03, 2017 5:22 pm
- Forum: Lewis Acids & Bases
- Topic: Distinguishing Lewis Acid
- Replies: 2
- Views: 295
Re: Distinguishing Lewis Acid
A lewis acid and a Bronsted acid are describing the same species, however looking at different aspects. A lewis acid is able to accept electrons. A Bronsted acid donates protons (H+).
- Sun Dec 03, 2017 5:19 pm
- Forum: Amphoteric Compounds
- Topic: Amphiprotic compounds
- Replies: 3
- Views: 2134
Re: Amphiprotic compounds
They are able to react in the presence of both an acid and a base.
- Sat Nov 25, 2017 5:24 pm
- Forum: Hybridization
- Topic: Question 4.95
- Replies: 2
- Views: 321
Re: Question 4.95
The 2 in front of sp is referring to the principal level the orbital lies in!
- Sat Nov 25, 2017 5:22 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Polarity of NH3?
- Replies: 4
- Views: 25626
Polarity of NH3?
Hi, I am slightly confused because I was determining the polarity of NH3 and I came to the answer that it's polar because it contains polar bonds making the entire molecule polar. Overall, the hydrogens are more positively charged than the nitrogen. However, I remember in class Professor Lavelle say...
- Sat Nov 18, 2017 9:50 pm
- Forum: Hybridization
- Topic: Double sigma v. pi bonds
- Replies: 4
- Views: 475
Re: Double sigma v. pi bonds
I feel like it will be helpful to refer to the p orbitals and their shape/orientation. Each p-orbital are orientated along an axis. In two atoms, with p-orbital bonding, one of the three orbitals will interact head on. The other one/two will be parallel to the other atoms p-orbitals.
- Sat Nov 18, 2017 9:47 pm
- Forum: Hybridization
- Topic: sigma/pi bond
- Replies: 4
- Views: 683
Re: sigma/pi bond
Yes, if you can imagine. You have two atoms that both contain p-orbitals. When they form a bond, 1 of the 3 p-orbitals of each atom interact head-on with a lot of overlap. The other 2 orbitals are parallel to its partner orbital in the other atom. These orbitals will form pi bonds.
- Thu Nov 09, 2017 5:06 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Radial Nodes/Planes
- Replies: 2
- Views: 523
Re: Radial Nodes/Planes
Radial node is a circular area with zero density, which means no electrons will be found there. Radial plane is a flat region (plane) with zero electron density.
To find the total number of nodes in an orbital= n-1
To find number of angular nodes= l
To find number of radial nodes= n-l-1
To find the total number of nodes in an orbital= n-1
To find number of angular nodes= l
To find number of radial nodes= n-l-1
- Thu Nov 09, 2017 5:01 pm
- Forum: Bond Lengths & Energies
- Topic: Bond Length
- Replies: 3
- Views: 439
Re: Bond Length
No, bond length and ionic character are not correlated. Ionic character is just referring to the electrons.
- Sun Nov 05, 2017 11:07 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Shell, subshell, and orbital
- Replies: 5
- Views: 758
Re: Shell, subshell, and orbital
n is any number above 1. So it can be 1,2,3,4....
l is [0,..., n-1]
ml is [-l,l]
So, for example, if you had n=6.
possible values for l=0,1,2,3,4,5. If we pick an electron in the 3 orbital
ml=-3,-2,-1,0,1,2,3
Hope that helps!!
l is [0,..., n-1]
ml is [-l,l]
So, for example, if you had n=6.
possible values for l=0,1,2,3,4,5. If we pick an electron in the 3 orbital
ml=-3,-2,-1,0,1,2,3
Hope that helps!!
- Sun Nov 05, 2017 11:01 pm
- Forum: Trends in The Periodic Table
- Topic: Electron Affinity [ENDORSED]
- Replies: 6
- Views: 1385
Electron Affinity [ENDORSED]
Hi,
I know that Doctor Lavelle and the book says that electron affinity is not really periodic, but we still have to be able to compare elements and determine which would be higher/lower electron affinity energy. How are we supposed to do that?
I know that Doctor Lavelle and the book says that electron affinity is not really periodic, but we still have to be able to compare elements and determine which would be higher/lower electron affinity energy. How are we supposed to do that?
- Sun Oct 29, 2017 8:52 pm
- Forum: Trends in The Periodic Table
- Topic: 2.97
- Replies: 2
- Views: 487
Re: 2.97
I haven't solved this problem yet, but I'd assume that you look up the Ionization Energy for Argon (I predict will be relatively high). It will most likely be in units of kJ/mol, so you'll have to convert it to J/atom. This energy will be the amount of energy required to remove the electron in gaseo...
- Sun Oct 29, 2017 8:46 pm
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: Two multiple choice questions I was stuck on ...
- Replies: 2
- Views: 1196
Re: Two multiple choice questions I was stuck on ...
For large, everyday objects the Heisenberg's Uncertainty Principle does not apply because the indeterminacy of momentum and position are so small that they're negligible. For example, when a baseball passes between two lasers, we are 100% certain of the path it took and the velocity/momentum it trav...
- Sun Oct 22, 2017 9:26 pm
- Forum: *Shrodinger Equation
- Topic: What is a node?
- Replies: 5
- Views: 717
Re: What is a node?
Yes, correct me if I'm wrong but I think of a node as having zero possibility of an electron being in that space.
- Sun Oct 22, 2017 9:24 pm
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: Test 3 [ENDORSED]
- Replies: 5
- Views: 793
Re: Test 3 [ENDORSED]
Test 3 is covering material up to Oct. 27th.
- Tue Oct 03, 2017 11:54 pm
- Forum: Empirical & Molecular Formulas
- Topic: F. 9
- Replies: 2
- Views: 1653
Re: F. 9
This question is asking you to determine the empirical formula which, by definition, is the ratio between the atoms in the molecule. So, by assuming that you're working with 100 g of Vanillin, you can convert each mass by composition percent to grams. For example, 63.15% C could be expressed as 63.1...
- Tue Oct 03, 2017 11:43 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: Writing formulas
- Replies: 4
- Views: 734
Re: Writing formulas
Yes, I second the statement above. Doctor Lavelle said he'll give you the chemical formulas for all the questions on the test on Friday.