Q = [concentration of products] / [concentration of reactants]
Because the molarities/partial pressures of all of the components in the Q equation are given, you simply plug and chug. I believe we may have a different test version so I did not get the same answer as you.
Search found 52 matches
- Sat Mar 17, 2018 9:51 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Solve for Q
- Replies: 2
- Views: 489
- Sat Mar 17, 2018 9:48 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Test 2 Question 8
- Replies: 1
- Views: 371
Re: Test 2 Question 8
There are two ways to calculate E(cell) with the E(knot) values of the half reactions. Method 1: 1. Reverse the anode half-reaction. 2. Keep the E(knot) value the same. 3. Use E(cathode) - E(anode) without changing the sign for the anode reaction, but using the reverse reaction. Method 2: 1. Reverse...
- Sat Mar 17, 2018 9:45 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Test 2 #3
- Replies: 2
- Views: 497
Re: Test 2 #3
I got something different, but that k value would correspond to a spontaneous reaction.
- Sat Mar 10, 2018 5:41 pm
- Forum: Experimental Details
- Topic: Homework Problem 15.3 Part C
- Replies: 5
- Views: 1142
Re: Homework Problem 15.3 Part C
The unique rate is just the basic rate of reaction. When you multiply a coefficient of a reactant by the unique rate, you get the rate of reaction of that compound.
- Sat Mar 10, 2018 5:39 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: The First Law
- Replies: 6
- Views: 990
Re: The First Law
The first law and the conservation of energy are the same. The first law just specifies for isolated systems because it is in discussion of thermodynamics.
- Sat Mar 10, 2018 5:36 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: The universe as a thermodynamic system [ENDORSED]
- Replies: 3
- Views: 592
Re: The universe as a thermodynamic system [ENDORSED]
In addition, the universe does not exchange heat or matter with anything beyond it, as there is nothing to do this with. So it is isolated.
- Wed Feb 28, 2018 12:04 am
- Forum: General Rate Laws
- Topic: Will we ever deal with third order reactions?
- Replies: 2
- Views: 325
Re: Will we ever deal with third order reactions?
Lavelle said third and fourth reactions won't be tested on, but we might cover them a little. He has intimated them a bit in our lectures.
- Wed Feb 28, 2018 12:03 am
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: What is the order of the reaction? [ENDORSED]
- Replies: 4
- Views: 559
Re: What is the order of the reaction? [ENDORSED]
If there are multiple reactants, you add up the exponents to find the total order of the reaction.
- Wed Feb 28, 2018 12:00 am
- Forum: General Rate Laws
- Topic: Negative in 15.5
- Replies: 3
- Views: 761
Re: Negative in 15.5
Since the question is asking for the rate at which O2 reacts, the negative is implied with the question.
- Thu Feb 22, 2018 9:47 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: The order of cell diagrams
- Replies: 1
- Views: 298
Re: The order of cell diagrams
Nope, as long as you separate the same phases with commas and the different phases with a single line.
- Wed Feb 21, 2018 1:15 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Picking between the different applications of the Nernst Equation
- Replies: 2
- Views: 518
Re: Picking between the different applications of the Nernst Equation
No they work interchangeably.
- Wed Feb 21, 2018 1:14 pm
- Forum: Balancing Redox Reactions
- Topic: Defining Cathodes and Anodes through standard cell potential
- Replies: 2
- Views: 380
- Wed Feb 21, 2018 1:13 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell Diagram Order
- Replies: 3
- Views: 439
Re: Cell Diagram Order
No, the order doesn't matter.
- Fri Feb 16, 2018 6:35 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Effect of solids and liquids on K
- Replies: 3
- Views: 454
Re: Effect of solids and liquids on K
Gases are also included in equilibrium solutions.
- Fri Feb 16, 2018 6:32 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Equilibrium
- Replies: 4
- Views: 470
Re: Equilibrium
I think the current stops because there is no longer a need for transfer of electrons, but I'm not sure.
- Fri Feb 16, 2018 6:29 pm
- Forum: Balancing Redox Reactions
- Topic: Basic vs Acidic
- Replies: 2
- Views: 374
Re: Basic vs Acidic
Then you have to make sure you balance the charges as well with electrons!
- Sat Feb 10, 2018 8:51 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: ∆S=q/T and irreversible reactions
- Replies: 2
- Views: 409
Re: ∆S=q/T and irreversible reactions
yep, i think so.
- Sat Feb 10, 2018 8:42 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: deltaG=0, Phases Coexist ?
- Replies: 2
- Views: 454
Re: deltaG=0, Phases Coexist ?
Some are liquid particles and loosely bound together and others are gaseous and flowing throughout the mixture.
- Sat Feb 10, 2018 8:30 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Table 8.3
- Replies: 1
- Views: 378
Re: Table 8.3
Since the textbook said to specifically use the table, I would use the value from there. On the test, you would use the 40 kJ value and that would be fine.
- Sat Feb 03, 2018 11:45 am
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: reversible and irreversible with entropy
- Replies: 2
- Views: 382
Re: reversible and irreversible with entropy
No you won't ever use q(irrev) to calculate the deltaS, but you can use the fact that entropy is a state function to find the amount of energy needed for an irreversible reaction.
- Sat Feb 03, 2018 11:44 am
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: How to tell what happens to entropy by seeing a reaction?
- Replies: 6
- Views: 1041
Re: How to tell what happens to entropy by seeing a reaction?
Like mentioned above, since the entropy of the products is higher, the total entropy would be a positive value.
- Sat Feb 03, 2018 11:40 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: deltaG at equilibrium
- Replies: 5
- Views: 577
Re: deltaG at equilibrium
deltaG = 0 at equilibrium, so that might be an indicator, but I'm not sure if that would be given.
- Thu Jan 25, 2018 6:41 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: exothermic vs endothermic [ENDORSED]
- Replies: 7
- Views: 1152
Re: exothermic vs endothermic [ENDORSED]
The calorimeter can also be apart of the surroundings, as some calorimeters absorb some of the heat released in the reaction. In general though, the water is the surrounding and whatever you're adding is the system.
- Thu Jan 25, 2018 6:38 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: 9.1 Entropy Higher or Lower at Higher Temperatures
- Replies: 2
- Views: 228
Re: 9.1 Entropy Higher or Lower at Higher Temperatures
There is actually an equation stating deltaS = -(deltaH)/T. Because of this, we can infer that deltaS is smaller in this situation.
- Mon Jan 22, 2018 12:25 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Week 3 Homework [ENDORSED]
- Replies: 1
- Views: 383
Week 3 Homework [ENDORSED]
What chapter of homework do we need to do for this week? My TA said we should submit chapter 9 homework, but I have discussion Wednesday morning and we have barely touched on Chapter 9 topics.
- Fri Jan 19, 2018 5:32 pm
- Forum: Calculating Work of Expansion
- Topic: work done on and by the system
- Replies: 12
- Views: 1433
Re: work done on and by the system
Work is negative when the system does work. Work is positive when work is done on the system.
- Fri Jan 19, 2018 5:22 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Problem 8.99
- Replies: 2
- Views: 238
Re: Problem 8.99
For the second question, the 800g comes from the 800 mL of water. Recall that water has a density of 1g/mL so this is used to change the volume to mass. Densities for other substances will be provided, but that's a good one to remember.
- Fri Jan 19, 2018 5:21 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Problem 8.99
- Replies: 2
- Views: 238
Re: Problem 8.99
For the first question, standard energy of formations are 0 when a compound is in its most stable, standard state. The definition of standard enthalpy of formation is the amount of energy required to create a 1 mole of a substance from its original standard state. Examples include O2, H2, I2. Br2, h...
- Fri Jan 19, 2018 5:06 pm
- Forum: Phase Changes & Related Calculations
- Topic: 8.23
- Replies: 5
- Views: 955
Re: 8.23
q = C (delta T) is also an equation that works, although I'm not sure when each is applied.
- Fri Jan 12, 2018 4:09 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Homework grading
- Replies: 6
- Views: 730
Re: Homework grading
In general though, I think they're graded for correctness.
- Fri Jan 12, 2018 4:09 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: tables in chapter 8
- Replies: 5
- Views: 358
Re: tables in chapter 8
He said in class today that all values will be given!
- Fri Jan 12, 2018 4:08 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Enthalpy formula from day 1
- Replies: 2
- Views: 286
Re: Enthalpy formula from day 1
Because the pressure is not changing, none of the heat being released is going into the surroundings. This would make the change a closed system and all of the heat released in a reaction would equal the enthalpy of the reaction.
- Sun Dec 10, 2017 4:42 pm
- Forum: Amphoteric Compounds
- Topic: amphiprotic vs. amphoteric [ENDORSED]
- Replies: 2
- Views: 829
Re: amphiprotic vs. amphoteric [ENDORSED]
They are similar but amphiprotic is more specific. Amphiprotic is when something can donate or receive a proton. Amphoteric is when something can act as an acid or a base.
- Wed Dec 06, 2017 3:20 pm
- Forum: Dipole Moments
- Topic: Dipole Moments and Polarity
- Replies: 9
- Views: 1118
Re: Dipole Moments and Polarity
In trigonal bi-pyramidal, there is no dipole moment because the five atoms around the central atom are evenly spread and symmetrical. For square pyramidal though, where there is a lone pair and 5 bonds to other atoms, this would form a dipole moment.
- Mon Nov 27, 2017 9:41 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Assuming x is negligible
- Replies: 3
- Views: 505
Assuming x is negligible
When can you assume that, in your ICE table, x is negligible and can be removed from your equilibrium constant equation?
- Mon Nov 27, 2017 9:13 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Gas Equilibrium Constant
- Replies: 1
- Views: 180
Gas Equilibrium Constant
If given the reaction 2 NO2(g) + F2(g) <-> 2 FNO2(g) are the following equilibrium constants the same? If not, what are the differences and what units or information do you input into each one? K = \frac{[FNO_{2}]^{2}}{[F^{2}][NO_{2}]^{2}} vs. K = \frac{[P_{FNO_{2})}]^2}{[P_{F_{2}}][P_{NO_{2}}]^...
- Thu Nov 23, 2017 12:14 pm
- Forum: Hybridization
- Topic: Pi Bonds vs. Sigma Bonds
- Replies: 7
- Views: 1100
Re: Pi Bonds vs. Sigma Bonds
Sigma bonds are always the first bonds that form. Pi bonds are all the bonds after that. So the second and triple bond are pi bonds and the first bond is still a sigma bond.
- Thu Nov 23, 2017 12:11 pm
- Forum: Naming
- Topic: Naming the metal
- Replies: 4
- Views: 502
Re: Naming the metal
Yup! -ate is only used when the transition metal forms an anion.
- Sat Nov 18, 2017 9:04 pm
- Forum: Hybridization
- Topic: Why is (CH3)2Be is sp? [ENDORSED]
- Replies: 8
- Views: 6698
Re: Why is (CH3)2Be is sp? [ENDORSED]
The central atom is always the one with the lowest electronegativity. Be is lower than C so it is in between the two carbons
- Sat Nov 18, 2017 9:00 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond angles
- Replies: 3
- Views: 340
Re: Bond angles
Lone pairs provide more repulsion than other atoms with electrons attached. Therefore the angles between the lone pairs and the atoms will be bigger than expected for the shape, and the angles between the atoms will be smaller because the lone pair pushes them closer together.
- Fri Nov 10, 2017 9:52 am
- Forum: Ionic & Covalent Bonds
- Topic: Midterm
- Replies: 6
- Views: 1049
Re: Midterm
I think it was SO2. KCl was ionic. SO2 was polar and N2 was nonpolar.
- Fri Nov 10, 2017 9:52 am
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: Practice Midterm Extra Practice #5
- Replies: 1
- Views: 367
Re: Practice Midterm Extra Practice #5
So you find that the indeterminacy of the position of the gutter ball is an extremely small number -- about 2.42 x 10^-34 m. This is less than a single millimeter, so you cannot blame the Heisenberg Principle for a gutter ball because the principle would only shift your bowling ball an extremely sma...
- Thu Nov 02, 2017 2:44 pm
- Forum: Lewis Structures
- Topic: Lone Pairs
- Replies: 2
- Views: 416
Re: Lone Pairs
So when you draw molecules, such as CO2, there are a total of 16 electrons present. Carbon has 4 valence electrons and oxygen has 6. So you draw the structure and find that Carbon is in the center and has the oxygens on the side. They are connected with double bonds. Carbon has used all of its valen...
- Thu Nov 02, 2017 2:39 pm
- Forum: Trends in The Periodic Table
- Topic: Electron Affinity and Ionization Energy
- Replies: 1
- Views: 329
Re: Electron Affinity and Ionization Energy
Well electron affinity and ionization are fundamentally different things. Electron affinity is the change in energy of an atom for adding an electron. When observed in reactions, it's shown that adding an electron is actually exothermic, meaning it releases energy, instead of needing energy to add e...
- Tue Oct 24, 2017 6:35 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Weekly online discussion points
- Replies: 3
- Views: 524
Re: Weekly online discussion points
I'm pretty sure he'll enter it all in at once or else it would be such a hassle. Someone should ask him in class or ask their TA though.
- Tue Oct 24, 2017 6:31 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Question on the difference between quantum numbers l and ml.
- Replies: 3
- Views: 1604
Re: Question on the difference between quantum numbers l and ml.
So l is the momentum of the electron rotating around the nucleus. Ml on the other hand, is the angle at which the electron is rotating around the nucleus. If you look at orbitals and their different shapes, you'll see that each ml has a different orbital shape and this ml number determines exactly w...
- Sat Oct 21, 2017 5:13 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Hund's Rule [ENDORSED]
- Replies: 6
- Views: 1216
Re: Hund's Rule [ENDORSED]
Hund's Rule basically states that every orbital shell is to be occupied by an electron before any orbital is occupied with two electrons. Usually this means that one spin direction is occupied for all the orbital shells before the opposite spin direction occupies the orbital to fill the shells.
- Sat Oct 21, 2017 5:11 pm
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: Rydberg Equation! [ENDORSED]
- Replies: 8
- Views: 2200
Re: Rydberg Equation! [ENDORSED]
Frequency can't be negative, but I've noticed that when you switch the two original n-values, one will result in a negative frequency and one will result in the same positive frequency. So whatever value you get, just take the positive form of it and continue.
- Fri Oct 13, 2017 3:25 pm
- Forum: Empirical & Molecular Formulas
- Topic: Test 1 Compound X [ENDORSED]
- Replies: 5
- Views: 912
Re: Test 1 Compound X [ENDORSED]
So you are given the mass of CO2 and H2O. You convert these both to moles. We can start with CO2. 7.48 grams of CO2 is 0.16996 moles of CO2. You multiple this value by (1 mol of C/1 mol of CO2) to isolate the moles of C. This will give you 0.16996 moles of C. You do the same for oxygen, multiplying ...
- Fri Oct 13, 2017 3:12 pm
- Forum: Properties of Electrons
- Topic: 1/2mv^2
- Replies: 2
- Views: 435
Re: 1/2mv^2
This equation is for kinetic energy. The total energy of a photon is composed of two energies: threshold and kinetic. The threshold energy is the energy needed to free or move an electron. The kinetic energy is the remaining energy, assuming the energy of the photon is greater than the threshold ene...
- Tue Oct 03, 2017 11:32 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: Atoms
- Replies: 3
- Views: 656
Re: Atoms
If they give you the mass of the compound, you convert it to moles, with the molar mass, and then multiple it by Avogadro's number! That's the amount of atoms that are in each mole of anything.
- Tue Oct 03, 2017 11:30 pm
- Forum: SI Units, Unit Conversions
- Topic: Appendix 1D & 1E
- Replies: 3
- Views: 322
Re: Appendix 1D & 1E
I think all of the appendixes are just for reference in the future. It doesn't necessarily mean we'll be tested on them!