Search found 57 matches
- Sat Mar 09, 2019 9:24 pm
- Forum: Second Order Reactions
- Topic: Determining the Order of a Reaction
- Replies: 3
- Views: 477
Re: Determining the Order of a Reaction
Most of the time, you will have to find the order of the reaction by testing the different graphs given in lecture and seeing which one is linear.
- Sat Mar 09, 2019 9:16 pm
- Forum: General Rate Laws
- Topic: integrals
- Replies: 8
- Views: 991
Re: integrals
If you look at the class website, you can find videos and links that will help with the math/calculus portion of this topic.
- Sat Mar 09, 2019 9:07 pm
- Forum: General Rate Laws
- Topic: Rate Law Dependence
- Replies: 1
- Views: 200
Re: Rate Law Dependence
Whether or not the rate law depends on the concentration of reactants depends on the order to the reaction.
- Sun Mar 03, 2019 1:28 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: pH at 10 C
- Replies: 3
- Views: 405
Re: pH at 10 C
Yes, for my version, increasing the temperature led to a basic solution.
- Sun Mar 03, 2019 1:26 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Test 2
- Replies: 7
- Views: 838
Re: Test 2
Yes, correct. The more positive the E value, the stronger the oxidizing power.
- Sun Mar 03, 2019 1:23 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: TEST 2
- Replies: 3
- Views: 407
Re: TEST 2
For the pH question, I think you had to use the Van't Hoff equation, which was given on the equation sheet. This equation relates the change in the equilibrium constant with the change in temperature. Using this equation, you can find the new equilibrium constant as a result of the change in tempera...
- Fri Feb 22, 2019 9:51 pm
- Forum: Balancing Redox Reactions
- Topic: Redox Rxn
- Replies: 3
- Views: 444
Re: Redox Rxn
In my opinion, just know the common ones, such as group 1 metals and group 2 metals, which are +1 and +2, respectively. Also, know that oxygen is generally -2 and chlorine is generally -1. Not sure if we will need to memorize the others.
- Fri Feb 22, 2019 9:26 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Spontaneity
- Replies: 2
- Views: 329
Re: Spontaneity
A reaction is considered spontaneous if the Gibbs free energy is negative. Knowing only the change in enthalpy or entropy cannot determine spontaneity.
- Fri Feb 22, 2019 9:24 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Salt bridge
- Replies: 3
- Views: 403
Re: Salt bridge
A salt bridge maintains the electrical neutrality of a battery. Negative ions would flow into the left compartment while positive ions would flow into the right compartment.
- Tue Feb 19, 2019 11:36 am
- 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: Third Law concept and problem types
- Replies: 4
- Views: 663
Re: Third Law concept and problem types
Yes, essentially the third law of thermodynamics is saying that at 0 degrees K, there is no vibrational, rotational, or translational entropy. The only possible entropy results from positional and residual. Thus, knowing the Boltzmann equation would come in handy when asked a question about the resi...
- Tue Feb 19, 2019 11:33 am
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: System vs Surroundings
- Replies: 14
- Views: 2138
Re: System vs Surroundings
Yes, the system vs. surrounding should not be something you have to memorize. As mentioned before, the system is simply the situation in question, such as a piston. Since the first law of thermodynamics states the conservation of energy, a change in energy of the system means a resultant change in s...
- Tue Feb 19, 2019 11:29 am
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: TEST 3
- Replies: 7
- Views: 1013
Re: TEST 3
I believe you mean for Test 2?
- Sun Feb 10, 2019 9:31 pm
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: Entropy and Enthalpy
- Replies: 3
- Views: 428
Re: Entropy and Enthalpy
Enthalpy has the letter "h" in it, so it corresponds to H. Not sure if that helps much, but usually, you should be able to differentiate between entropy and enthalpy based on what the problem is asking.
- Sun Feb 10, 2019 9:28 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Midterm 2019
- Replies: 9
- Views: 900
Re: Midterm 2019
Since he said up to entropy, it is up to the "Second and Third Laws of Thermodynamics", but only part of Chapter 9.
- Sun Feb 10, 2019 9:27 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Midterm
- Replies: 2
- Views: 333
Re: Midterm
Yes, you can check "Important Midterm Information" on his website.
- Sun Feb 03, 2019 6:32 pm
- Forum: Phase Changes & Related Calculations
- Topic: Work by expansion
- Replies: 3
- Views: 374
Re: Work by expansion
Yes, use the conversion ratio which should be given to us, either in the problem or on the formula sheet to convert.
- Sun Feb 03, 2019 6:30 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: PV=nRT
- Replies: 5
- Views: 532
Re: PV=nRT
This equation describes an ideal gas, which is essentially a simplified model of real gases to help us in calculations. Since there are 4 unknown's in this equation, we can use this equation when we have three givens, which then can be used to calculate the final unknown.
- Sun Feb 03, 2019 6:28 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: HW
- Replies: 3
- Views: 384
Re: HW
Yes, we should still be able to do thermochemistry problems for HW.
- Tue Jan 29, 2019 5:51 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: standard enthalpies of formation
- Replies: 2
- Views: 326
Re: standard enthalpies of formation
The standard enthalpy of formation is the net change in enthalpy, or in simpler terms, the net change in heat, for one mole of a substance in standard state to be formed from its pure elements. A standard enthalpy of formation of 0 means that the substance is already in standard state.
- Tue Jan 29, 2019 5:45 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: delta u eqn
- Replies: 3
- Views: 386
Re: delta u eqn
Essentially, the change in internal energy of a system, deltaU, equals the net heat transfer into the system, Q, plus the net work, W, done on the system. This is the first law of thermodynamics.
- Mon Jan 28, 2019 10:34 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: 4E.5
- Replies: 1
- Views: 207
Re: 4E.5
Carbon and Hydrogen cannot have a triple bond because a hydrogen atom only has one valence electron.
- Sat Jan 19, 2019 3:41 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: K - small verses big
- Replies: 4
- Views: 424
Re: K - small verses big
A small Ka essentially means a large Kb, since they are inversely proportional. The larger the acid or base equilibrium constant, the stronger the acid or base.
- Sat Jan 19, 2019 3:32 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Protonation
- Replies: 1
- Views: 257
Re: Protonation
Protonation and Deprotonation is simply the acceptance/donation of a proton as a result of a reaction. For weak acids/bases, since it is not complete disassociation, there is a percentage that remains an acid/base as a result of equilibrium. Percent protonation is the change in concentration for the...
- Sat Jan 19, 2019 3:28 pm
- Forum: Student Social/Study Group
- Topic: ICE Table
- Replies: 6
- Views: 489
Re: ICE Table
Usually, if the problem gives you initial concentrations of the reactants and asks for the equilibrium concentrations of each molecule, you can most likely use an ICE table to solve the problem.
- Sun Jan 13, 2019 1:04 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Equilibrium Constant Eq.
- Replies: 4
- Views: 386
Re: Equilibrium Constant Eq.
No, you do not need to include solids and liquids when calculating the equilibrium constant.
- Sun Jan 13, 2019 1:02 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Equations
- Replies: 6
- Views: 523
Re: Equations
Yes, you could easily convert between partial pressure to concentration by using PV=nRT.
- Sun Jan 13, 2019 12:48 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: "bar" meaning
- Replies: 4
- Views: 490
Re: "bar" meaning
Yes, it is also equivalent to 100 kPa, if that helps.
- Fri Dec 07, 2018 8:50 pm
- Forum: Hybridization
- Topic: Hybridization on Test
- Replies: 3
- Views: 437
Re: Hybridization on Test
Yes. For instance, oxygen is often displayed without its lone pairs, so we must account for them when determining hybridization.
- Fri Dec 07, 2018 8:49 pm
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: Review questions
- Replies: 3
- Views: 1377
Re: Review questions
Although S has a higher electronegativity leading to stronger dipole-dipole interactions, Se has a larger atomic mass, resulting in stronger London dispersion forces which are more stronger than the dipole-dipole interactions. Thus, H2Se has a higher boiling point.
- Fri Dec 07, 2018 8:47 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: AX2E3 (i.e. linear) Molecular geometry
- Replies: 1
- Views: 1421
Re: AX2E3 (i.e. linear) Molecular geometry
The electron density shape would be based off the trigonal bipyramidal shape. The three lone pairs will take the three equatorial positions, leaving the two axial positions for the atoms. This would result in a symmetrical linear molecular shape.
- Sun Dec 02, 2018 3:01 pm
- Forum: Bronsted Acids & Bases
- Topic: Electronegativity
- Replies: 2
- Views: 328
Re: Electronegativity
Higher electronegativity allows for easier dissociation. A strong acid completely dissociates in water, so the higher the electronegativity, the stronger the acid.
- Sun Dec 02, 2018 1:39 pm
- Forum: Bronsted Acids & Bases
- Topic: Proton "Donation"
- Replies: 4
- Views: 515
Re: Proton "Donation"
Yes, a Bronsted acid donates a hydrogen ion (H+).
- Thu Nov 29, 2018 2:45 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: 4.95 6th ed
- Replies: 3
- Views: 406
Re: 4.95 6th ed
I believe it is asking for the lewis structure with the greatest contribution to the resonance, so essentially the most stable structure.
- Sun Nov 25, 2018 2:02 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Hypervalent Compounds
- Replies: 1
- Views: 250
Re: Hypervalent Compounds
To my knowledge, not all compounds containing period 3 or below elements are hypervalent compounds as the expanded octet is not always necessary.
- Sun Nov 25, 2018 1:51 pm
- Forum: Hybridization
- Topic: Equatorial lone pair
- Replies: 2
- Views: 266
Re: Equatorial lone pair
Essentially, an equatorial lone pair is generally the lowest energy because it is only strongly interacting with the two axial electron pairs, whereas axial lone pair strongly interacts the three equatorial electron pairs.
- Sun Nov 25, 2018 1:49 pm
- Forum: Lewis Structures
- Topic: Central atom of CNO-
- Replies: 2
- Views: 184
Re: Central atom of CNO-
Nitrogen would be the central atom in this case. If the chemical formula was given as OCN-, then carbon would be the central atom.
- Sun Nov 18, 2018 6:12 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Molecular Geometry
- Replies: 6
- Views: 629
Re: Molecular Geometry
For instance, the electron density geometry for H2O is tetrahedral, since there are 2 bonded pairs and 2 lone pairs. The molecular geometry of H2O is bent, since only 2 atoms are bonded with the central atom.
- Sun Nov 18, 2018 5:19 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge of Central Atom
- Replies: 4
- Views: 1199
Re: Formal Charge of Central Atom
I'm not exactly sure about ClO2+, but generally, you would want the formal charge for the central atom to be 0, and the outer atoms with the charge.
- Sun Nov 18, 2018 2:36 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Lone Pairs
- Replies: 8
- Views: 2743
Re: Lone Pairs
Lone pairs are considered as an electron density when regarding shape of a molecule. It has a larger repulsion when compared to bonded pairs of electrons.
- Sat Nov 10, 2018 3:55 pm
- Forum: Dipole Moments
- Topic: Dipole-Induced Dipole
- Replies: 3
- Views: 318
Re: Dipole-Induced Dipole
Water is a dipole as the oxygen is electronegative, causing O to be more negative than the H's. If a water molecule (dipole) was nearby a N2 molecule (nonpolar), the N closest to the O would have a slightly positive charge, causing the other N to have a slightly negative charge, creating a dipole. T...
- Sat Nov 10, 2018 3:50 pm
- Forum: Polarisability of Anions, The Polarizing Power of Cations
- Topic: Polarizability
- Replies: 4
- Views: 450
Re: Polarizability
Essentially, the larger the atom (the more electrons), the easier it is for electrons to become distorted, since the pull on the outer electrons is less for larger atoms.
- Sat Nov 10, 2018 3:10 pm
- Forum: Ionic & Covalent Bonds
- Topic: Hydrogen bonding
- Replies: 7
- Views: 1354
Re: Hydrogen bonding
The electronegativity of oxygen causes water to be polar, leading to hydrogen bonding. Because of hydrogen bonding, H2O requires more energy needed to break the bonds, thus it has a much higher boiling point/melting point than that of H2S.
- Sat Nov 03, 2018 4:49 pm
- Forum: Octet Exceptions
- Topic: Adding a Double bond or leaving a lone pair [ENDORSED]
- Replies: 3
- Views: 417
Re: Adding a Double bond or leaving a lone pair [ENDORSED]
You would have to find the formal charges of each atom in each structure. You would want to find the structure with the least formal charge (lowest energy).
- Sat Nov 03, 2018 4:47 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: 6th Edition 2.53
- Replies: 1
- Views: 857
Re: 6th Edition 2.53
Hund's rule states that every subshell must be singlely occupied by one electron before it can be doubly occupied. For instance, you know the electron config of Ga, which is [Ar]3d10 4s2 4p1. There is one unpaired electron in this case, because there is one electron in the 4p orbital. For Se, the el...
- Sat Nov 03, 2018 4:42 pm
- Forum: Student Social/Study Group
- Topic: Sig Figs on Midterm
- Replies: 13
- Views: 1591
Re: Sig Figs on Midterm
I think just to be safe, you should follow the sigfig guidelines.
- Sat Oct 27, 2018 4:09 pm
- Forum: Lewis Structures
- Topic: Order in Drawing Lewis Structures
- Replies: 2
- Views: 133
Re: Order in Drawing Lewis Structures
To my knowledge, it does not matter which side you put the dots, as long as you follow Hund's rule where electrons fill the available subshells before pairing up to have the lowest energy state.
- Sat Oct 27, 2018 3:55 pm
- Forum: DeBroglie Equation
- Topic: Homework Question 1B.15
- Replies: 3
- Views: 215
Re: Homework Question 1B.15
Yes, definitely use meters per second. And in this case, using the KE = (1/2)mv^2 then using the E = (planck's constant)(frequency) would be easiest to solve this problem.
- Sat Oct 27, 2018 3:50 pm
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: Heisenberg- In relation to wavelength
- Replies: 7
- Views: 741
Re: Heisenberg- In relation to wavelength
The uncertainty in momentum is inversely proportional to the uncertainty in wavelength, meaning a larger uncertainty in momentum will lead to a smaller uncertainty in wavelength, and vice versa.
- Sat Oct 20, 2018 9:26 pm
- Forum: Properties of Light
- Topic: Atomic Spectra pre-module quiz
- Replies: 1
- Views: 239
Re: Atomic Spectra pre-module quiz
I'm not quite sure of the difference between atomic absorption vs. atomic emission spectroscopy, but I do know that the lines on the spectrum represent the different energy levels that the electron can be on.
- Sat Oct 20, 2018 9:18 pm
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: HW problem 1.43
- Replies: 1
- Views: 172
Re: HW problem 1.43
I believe just the drawing of the box is sufficient. But, you could include the wavelength of the electron if you want to.
- Sat Oct 20, 2018 9:17 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Coulomb's Law
- Replies: 3
- Views: 230
Re: Coulomb's Law
I believe we discussed Coulomb's law mainly to demonstrate the effects of shielding on electrostatic attraction.
- Sat Oct 13, 2018 5:08 pm
- Forum: Properties of Light
- Topic: Wavelength Units
- Replies: 5
- Views: 461
Re: Wavelength Units
Using nanometers would be better for wavelength.
- Sat Oct 13, 2018 5:01 pm
- Forum: Properties of Electrons
- Topic: Spectral Lines (Balmer Series & Lyman Series)
- Replies: 3
- Views: 279
Re: Spectral Lines (Balmer Series & Lyman Series)
For me, it helps to draw the diagram that Lavelle draws in the lectures. This helps me visualize the electron going from its "excited" state to "resting" state and also the change in energy, which results in the release of photons.
- Sat Oct 13, 2018 4:53 pm
- Forum: DeBroglie Equation
- Topic: WaveLike Properties
- Replies: 3
- Views: 177
Re: WaveLike Properties
Technically, all matter has wave-like properties, but they can only be noticed in moving objects with small mass.
- Fri Oct 05, 2018 10:57 am
- Forum: General Science Questions
- Topic: Common ions
- Replies: 4
- Views: 591
Re: Common ions
Is there a list of all the common ions that we should know? I know a few but I'm not sure if there are more that I am missing.
- Fri Oct 05, 2018 10:48 am
- Forum: Limiting Reactant Calculations
- Topic: Maximum Product Produced
- Replies: 2
- Views: 330
Re: Maximum Product Produced
To determine maximum production, you need to know the number of moles of each reactant. The number of moles of the limiting reactant should determine maximum product via the molar ratio given. In this example, you would need more information in order to solve this question.
- Fri Oct 05, 2018 10:42 am
- Forum: Limiting Reactant Calculations
- Topic: Compensating for Mole Ratios in Limiting Reactants
- Replies: 3
- Views: 445
Re: Compensating for Mole Ratios in Limiting Reactants
Start by finding the number of moles of each reactant that you have. To do that, you need the molar mass, which can be found using the periodic table. After knowing how many moles of each reactant you have, compare these numbers to the molar ratio given in the equation to find out which particular m...