Search found 154 matches
- Mon Mar 16, 2020 2:57 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Delta G of Ionization of water on Final
- Replies: 1
- Views: 280
Delta G of Ionization of water on Final
On the final, there was a problem where it asked you to calc the deltaG/deltaH/deltaS of ionization of water of a specific temp. How would you have approached this problem?
- Mon Mar 16, 2020 2:55 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: ATP QUESTION ON FINAL
- Replies: 9
- Views: 916
Re: ATP QUESTION ON FINAL
Sine it says pi comes from ATP, the two concentrations cancels and K depends on [ADP] only. Maybe I am wrong about how I interpreted this problem, but I assumed that since all the Pi came from ATP, I assumed it meant that it only came from ATP that was broken into ADP...so Pi = ADP concentration......
- Sat Mar 14, 2020 3:54 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Arrhenius Equation "A"
- Replies: 3
- Views: 316
Re: Arrhenius Equation "A"
IM pretty sure it stays constant
- Sat Mar 14, 2020 3:53 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Determining if a reaction mechanism is feasible
- Replies: 3
- Views: 360
Re: Determining if a reaction mechanism is feasible
One way is to see if the slow step rate law matches the overall rate law. Remember that no matter the substitutions u may have to make for intermediates, the rate law will have the same order no matter what.
- Sat Mar 14, 2020 3:52 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Endgame Q15
- Replies: 2
- Views: 297
Re: Endgame Q15
Yes this is the concept of a pseudo rate law
- Sat Mar 14, 2020 2:34 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: UA Practice Final Q4
- Replies: 2
- Views: 309
Re: UA Practice Final Q4
First, you would wanna figure out how much H+ there is in solution. You do this by setting up an ice table and solve for H+ (remember is 2H+ in the equation). Then you have the amount of H+ in solution, and in order to neutralize it, you need the same amount of OH- to balance this out. You then use ...
- Sat Mar 14, 2020 2:09 pm
- Forum: General Rate Laws
- Topic: Hw 7A.13
- Replies: 9
- Views: 695
Re: Hw 7A.13
So the rate law would be based off of if each reactant is a first, second, or zero order reactant. Based from the info, you can infer that both reactants are first order because as you increase their concentration by a constant, the rate also increases by the same amount. therefore it would be k[CH3...
- Thu Mar 12, 2020 8:38 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Lavelle's review slides
- Replies: 1
- Views: 230
Re: Lavelle's review slides
He's referencing deltaG overall. He used this equation to see which side (reactants or products) will be favored given the conditions. Since deltaG is positive, it isn't spontaneous but that's for the forward reaction, the reverse reaction will be spontaneous in this case.
- Wed Mar 11, 2020 12:48 am
- Forum: Administrative Questions and Class Announcements
- Topic: Saying Thank You to Dr. Lavelle
- Replies: 490
- Views: 559657
Re: Saying Thank You to Dr. Lavelle
Even with the current situation, Lavelle has been a really great professor for both my 14a and 14b careers. I truly thank him for making my chemistry “good chemistry” :)
- Tue Mar 10, 2020 11:07 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Pre-Equil Approach
- Replies: 2
- Views: 259
Pre-Equil Approach
Does anyone know any book problem with a situation that we need to use this? The example in the book is the example we did in class. I also dont understand how to do number 14 on the "endgame" worksheet pertaining to this.
- Tue Mar 10, 2020 5:00 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Review Sessions for Final Exam
- Replies: 2
- Views: 270
Re: Review Sessions for Final Exam
Will there also still be TA Office Hours?
- Mon Mar 09, 2020 7:09 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: 7.11 part b
- Replies: 2
- Views: 213
Re: 7.11 part b
Ok thank you!
- Mon Mar 09, 2020 5:28 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: 7.11 part b
- Replies: 2
- Views: 213
7.11 part b
How do we know, when drawing this reaction profile, where the energies of the products of the first reactants lie energy-wise in relation to the whole profile? I know the whole reaction must be exothermic but where should the middle products/reactants lie? The answer implies they are both the same e...
- Sun Mar 08, 2020 6:53 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Example 7C.1
- Replies: 1
- Views: 175
Example 7C.1
How should we think of the rate of decomposition vs rate of formation in this type of scenario? Will we have to do this one a test?
- Sun Mar 08, 2020 6:33 pm
- Forum: General Rate Laws
- Topic: Difference b/w General Rate Laws/Elementary
- Replies: 2
- Views: 278
Difference b/w General Rate Laws/Elementary
Lavelle states on a worksheet on his website that "2N2O(g) → 2NO(g) + O2(g) • Write the overall rate expression for this first-order reaction. rate= k[N2O] *Note that the exponent does not match the coefficient in front of N2O. By just looking at the overall balanced equation, you cannot tell t...
- Sun Mar 08, 2020 6:23 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: 7.31
- Replies: 3
- Views: 273
Re: 7.31
I keep getting 1.12x10^8 M/s =k2 regardless of the order of the equation, but that's incorrect according to the book which has 2.5x10^9M/s as the answer.
- Sun Mar 08, 2020 6:19 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: A in the Arrhenius Equation
- Replies: 3
- Views: 288
A in the Arrhenius Equation
What does the A stand for in the Ae^(-Ea/RT) equation? I haven't seen this equation directly tested/used on the homework
- Sun Mar 08, 2020 6:16 pm
- Forum: Zero Order Reactions
- Topic: Half life of zero order runs
- Replies: 3
- Views: 288
Half life of zero order runs
Why is it when you plot the half-life against [A] for a reaction that is zero order, that the plot is linear?
Also, why is the initial rate of a 1st order rxn vs [A] linear?
Also, why is the initial rate of a 1st order rxn vs [A] linear?
- Sun Mar 08, 2020 6:11 pm
- Forum: Zero Order Reactions
- Topic: slope of zero order reaction
- Replies: 2
- Views: 264
Re: slope of zero order reaction
Well, when we derived the equation in class, the equation so happened to yield a negative number in front of k resulting in a negative slope. Remember, zero-order reactants don't affect the rate, so it doesn't mean much to the reaction rate, it just speaks to the relationship between [A] vs time.
- Sun Mar 08, 2020 6:07 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: 7E.3A
- Replies: 1
- Views: 230
Re: 7E.3A
I found an equation in book which helped. Ea(with catalyst)-Ea(w/o catalyst)/RT= a number. That number you then add a negative sign to and raise it to the e^power. Basically, its putting k2/k1 with the Arrhenius equations both on the top and bottom, respectively. so for part a i got 75000-125000/(8....
- Sun Mar 08, 2020 5:22 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: 7.31
- Replies: 3
- Views: 273
7.31
7.31 The rate constant of the reaction O2(g) + N2(g) --> NO(g) + N(g), which takes place in the stratosphere, is 9.7 x 10^10 M/s at 800 degree C. The activation energy of the reaction is 315 kJ/mol. What is the rate constant at 700 degrees C? I used the equation ln(k2/k1)=Ea/R(1/T2-1/T1) but im gett...
- Sun Mar 08, 2020 4:37 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: 7B.13
- Replies: 1
- Views: 188
7B.13
Half-life of A in a second-order reaction is 50.5 sec when [A]intial=.84 M. Calc the time needed for the conc of A to decrease to (a) one-sixteenth, (b)one-fourth, (c)one-fifth its original value. Can someone explain their thought process and method of doing this problem? I thought all you had to do...
- Sun Mar 08, 2020 4:26 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: 7B.3 part c
- Replies: 2
- Views: 227
Re: 7B.3 part c
Thank you!
- Sun Mar 08, 2020 1:26 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: 7B.3 part c
- Replies: 2
- Views: 227
7B.3 part c
c) 2 A --> B + C, given that [A]intial= 0.153 M and that after 115 s the
concentration of B rises to .034 M.
How would I set up this problem? I dont understand how i should use the conc of B since the problem also gave us the initial conc of A.
concentration of B rises to .034 M.
How would I set up this problem? I dont understand how i should use the conc of B since the problem also gave us the initial conc of A.
- Sun Mar 08, 2020 1:17 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: 7E.5
- Replies: 1
- Views: 188
7E.5
7E.5 The hydrolysis of an organic nitrile, a compound containing a OCqN group, in basic solution, is proposed to proceed by the following mechanism. Write a complete balanced equation for the overall reaction, list any intermediates, and identify the catalyst in this reaction. Why is the catalyst fo...
- Sun Mar 08, 2020 12:51 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: 7D.7
- Replies: 1
- Views: 110
7D.7
7D.7 For the reversible, one-step reaction A + a <—>C + D the forward rate constant for the formation B is 265 L/molmin and the rate constant for the reverse reaction is 392 L?mol ?h . The activation energy of the forward reaction was found to be 39.7 kJ?mol21 and 25.4.0 kJ?mol21 for the reverse rea...
- Sat Mar 07, 2020 2:40 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: 7C.7
- Replies: 3
- Views: 311
7C.7
Step 1 NO + Br2 --> NOBr2 slow
Step 2 NOBr2 + NO --> NOBr + NOBr fast
Write the rate law for the formation of NOBr implied by this
mechanism.
I got rate= k[NO2]^2[Br2], but the book has rate= k[NO2][Br2], why is that?
Step 2 NOBr2 + NO --> NOBr + NOBr fast
Write the rate law for the formation of NOBr implied by this
mechanism.
I got rate= k[NO2]^2[Br2], but the book has rate= k[NO2][Br2], why is that?
- Mon Mar 02, 2020 8:10 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Electrolytic Cells
- Replies: 1
- Views: 173
Electrolytic Cells
"The potential supplied to an electrolytic cell must be at least as great as that of the cell reaction to be reversed. If there is more than one reducible species in solution, the species with the greater potential for reduction is preferentially reduced. The same principle applies to oxidation...
- Mon Mar 02, 2020 7:43 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 6.43
- Replies: 3
- Views: 281
6.43
6.43 Indicate for each of the following statements whether it applies to Ecell8, to Ecell, to both, or to neither: (a) decreases as the cell reaction progresses; (b) changes with temperature; (c) doubles when the coefficients of the equation are doubled; (d) can be cal- culated from K; (e) is a meas...
- Mon Mar 02, 2020 7:18 pm
- Forum: Interesting Applications: Rechargeable Batteries (Cell Phones, Notebooks, Cars), Fuel Cells (Space Shuttle), Photovoltaic Cells (Solar Panels), Electrolysis, Rust
- Topic: Nerve Cell
- Replies: 1
- Views: 139
Nerve Cell
In a neuron (a nerve cell), the concentration of K+ ions inside the cell is about 20–30 times as great as that outside. What potential difference between the inside and the outside of the cell would you expect to measure if the difference is due only to the imbalance of potassium ions? Do we conside...
- Mon Mar 02, 2020 7:13 pm
- Forum: General Rate Laws
- Topic: Homework 7A.17
- Replies: 2
- Views: 329
Re: Homework 7A.17
Reactant B is second order. Since you know reactant C is zero order, you can focus on two reactions where reactant A is constant and reactant B is doubling and look at what it does to the rate constant. Hope this helps
- Mon Mar 02, 2020 7:10 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Knowing if a Metal will dissolve
- Replies: 1
- Views: 145
Knowing if a Metal will dissolve
How do I know if a metal will dissolve in a certain solution? Should it be in a spontaneous way, where the metal will be oxidized by the molecules in the solution?
- Mon Mar 02, 2020 7:06 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Final Review Sessions
- Replies: 6
- Views: 381
Final Review Sessions
When will Final Review Sessions start? i need to go to all of them lol
- Mon Mar 02, 2020 6:55 pm
- Forum: Balancing Redox Reactions
- Topic: Basic vs Acidic Conditions.
- Replies: 6
- Views: 479
Re: Basic vs Acidic Conditions.
I wouldn't think of it like that just to be sure, I would just make sure I know how to balance them
- Mon Mar 02, 2020 6:54 pm
- Forum: Student Social/Study Group
- Topic: Today's Workshop
- Replies: 2
- Views: 296
Re: Today's Workshop
^^^^^
- Mon Mar 02, 2020 6:51 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Homework 5.55
- Replies: 1
- Views: 97
Re: Homework 5.55
You can use the general equation for Gibbs free energy of formation (products-reactants=rxn total) and then set that equal to deltaG=-RTlnK. For part b its a regular ice table problem.
- Mon Mar 02, 2020 6:47 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Week 8 - Wednesday Lecture
- Replies: 2
- Views: 273
Re: Week 8 - Wednesday Lecture
I would also suggest reading lesson 7A in the book as a good overview as well. Make sure to understand initial versus average rates
- Wed Feb 26, 2020 9:21 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: 6.63
- Replies: 1
- Views: 210
6.63
When a pH meter was calibrated with a boric acid–borate buffer with a pH of 9.40, the cell potential was +0.060 V. When the buffer was replaced with a solution of unknown hydronium ion concentration, the cell potential was +0.22 V. What is the pH of the solution? How would i begin this problem? I do...
- Wed Feb 26, 2020 9:05 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Electrochemical Series
- Replies: 2
- Views: 231
Electrochemical Series
The Outline for EChem mentions the electrochemical series, what should we know about this? It seems like its just a ranking of the most likely to get oxidized metal to the most likely to get reduced metal. Am i missing something else?
- Wed Feb 26, 2020 7:02 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Free energy dependent on Temp and Pressure
- Replies: 1
- Views: 156
Free energy dependent on Temp and Pressure
Thermo outline 4: Understand why reaction free energy depends on pressure and the equilibrium constant
I understand the equations that go along with this statement, but what else should we know about this?
I understand the equations that go along with this statement, but what else should we know about this?
- Tue Feb 25, 2020 10:19 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: 6.57
- Replies: 3
- Views: 352
6.57
6.57 Use the data in Appendix 2B and the fact that, for the half- reaction F2(g) + 2 H+(aq) + 2 e- ---> 2 HF(aq), E(knot)= +3.03 V, to calculate the value of Ka for HF.
How would I do this problem?
How would I do this problem?
- Tue Feb 25, 2020 1:37 pm
- Forum: Balancing Redox Reactions
- Topic: 6K. D
- Replies: 3
- Views: 337
Re: 6K. D
Oh yes, my bad.
- Mon Feb 24, 2020 9:08 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: 6N.15
- Replies: 1
- Views: 242
6N.15
Calculate the potential of a cell constructed with two nickel electrodes. The electrolyte in one compartment is 1.0 m Ni(NO3)2(aq).In the other compartment, NaOH has been added to a Ni(NO3)2 solution until the pH was 11.0 at 298 K. Ksp=6.5x10^-18 How would I start this problem? I got the concentrati...
- Mon Feb 24, 2020 3:59 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: 6N.5
- Replies: 1
- Views: 106
6N.5
This question asks for a concentration of one of the species given the cell potential in the problem. However, they give us partial pressures for the other species in the reaction. Do we have to factor this into our Q equation or not at all? How would this work exactly?
- Mon Feb 24, 2020 12:40 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Picking up 14A Finals in Young Hall
- Replies: 3
- Views: 280
Picking up 14A Finals in Young Hall
Are we still able to pick up 14A finals? I definitely forgot until now.
- Sat Feb 22, 2020 12:41 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 6L.7
- Replies: 2
- Views: 195
6L.7
6L.7 Write the half-reactions and devise a galvanic cell (write a cell diagram) to study each of the following reactions: (a) AgBr(s) --> Ag+(aq) + Br2(aq), a solubility equilibrium (b) H+(aq) + OH-(aq)--> H2O(l) How would i write the half reactions for these and the cell diagrams? Its confusing to ...
- Sat Feb 22, 2020 12:04 pm
- Forum: Phase Changes & Related Calculations
- Topic: delta G0 versus delta G
- Replies: 15
- Views: 2618
Re: delta G0 versus delta G
The difference between the two is that delta G naught is at standard conditions. The reason Professor Lavelle emphasized it is because delta G naught is always the same because it is referring to when the reactants/products are at standard temperature/pressure. As the rxn goes towards equilibrium, ...
- Thu Feb 20, 2020 2:51 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: 6L.9 Part A
- Replies: 1
- Views: 221
6L.9 Part A
6L.9 (a) Write balanced half-reactions for the redox reaction of an acidified solution of potassium permanganate and iron(II) chloride. (b) Write the balanced equation for the cell reaction and devise a galvanic cell to study the reaction (write its cell diagram). Are we supposed to know that the Fe...
- Thu Feb 20, 2020 2:00 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: 6L.3 part c
- Replies: 1
- Views: 126
6L.3 part c
How would you write the half-reactions given the cell is :
Pt(s) I O2 (g) I H+(aq) I OH-(aq) I O2 (g) I Pt(s)
Pt(s) I O2 (g) I H+(aq) I OH-(aq) I O2 (g) I Pt(s)
- Wed Feb 19, 2020 4:32 pm
- Forum: Balancing Redox Reactions
- Topic: Balancing Redox
- Replies: 5
- Views: 388
Re: Balancing Redox
Most likely on tests im pretty sure lavelle would give us the charges. If not, just know some common ones like phosphate, sulfate, etc.
- Wed Feb 19, 2020 4:30 pm
- Forum: Balancing Redox Reactions
- Topic: 6K. D
- Replies: 3
- Views: 337
Re: 6K. D
The way i start this problem is by balancing the solution in acidic solution and then, at the end, adding OH- to both sides so the H+'s cancel out. The OH- + H+ turns into neutral H2O molecules (which may or may not cancel out. Therefore, Oxidation: 8OH- +P4 --> H2PO2-+4e- Reduction: 12e-+ 12H2O+ P4...
- Wed Feb 19, 2020 4:13 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: 6M. 13
- Replies: 1
- Views: 196
Re: 6M. 13
Could you fix the formatting of this question?
- Wed Feb 19, 2020 4:11 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Midterm Question 6B
- Replies: 3
- Views: 288
Re: Midterm Question 6B
Your logic is correct. Using the equation delta G = delta H - (T)(delta S), it is apparent that the value of delta G will be close to that of delta H when you have a value of delta S close to or equal to 0. Therefore, the answer with the smallest change in entropy, as you mentioned, would be the co...
- Wed Feb 19, 2020 4:09 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Midterm Q3B and Q3D
- Replies: 1
- Views: 169
Midterm Q3B and Q3D
Q3B Why is the answer for the question 50ml of 2M HCl and 50ml of 2 M NaOH?
Q3D: How are we supposed to determine the net charge of acetic acid given its at a pH of 6 with pKa = 4.75?
Q3D: How are we supposed to determine the net charge of acetic acid given its at a pH of 6 with pKa = 4.75?
- Tue Feb 18, 2020 9:45 pm
- Forum: Balancing Redox Reactions
- Topic: 6K.3 Part D
- Replies: 2
- Views: 220
6K.3 Part D
Reaction of chlorine in water:
Cl2(g) --> HClO(aq) + Cl2(g)
Can someone help me balance this in an acidic solution?
Cl2(g) --> HClO(aq) + Cl2(g)
Can someone help me balance this in an acidic solution?
- Tue Feb 18, 2020 9:16 pm
- Forum: Balancing Redox Reactions
- Topic: Balancing half reactions
- Replies: 11
- Views: 693
Re: Balancing half reactions
Make sure that the amount of electrons transferred are all accounted for on the other side of the equation
- Tue Feb 18, 2020 9:14 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Cubic to quadratic function
- Replies: 4
- Views: 440
Re: Cubic to quadratic function
If you find yourself with a cubic function you can probably approximate.
- Tue Feb 18, 2020 9:13 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Concepts
- Replies: 3
- Views: 294
Re: Concepts
Cell potential is also equivalent to the max amount of work that the battery can do.
- Mon Feb 10, 2020 6:49 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3622648
Re: Post All Chemistry Jokes Here
https://www.relatably.com/m/img/light-memes/thumb.jpeg
You won't regret seeing this even though its a Chem14A joke
You won't regret seeing this even though its a Chem14A joke
- Mon Feb 10, 2020 11:30 am
- Forum: Calculating Work of Expansion
- Topic: Reversible and Isobaric
- Replies: 4
- Views: 329
Re: Reversible and Isobaric
I would only do the calculation for irreversible reactions if the problem says specifically.
- Mon Feb 10, 2020 11:24 am
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: delta U
- Replies: 8
- Views: 250
Re: delta U
805317518 wrote:Conceptually speaking, would an adiabatic system always be an isolated system? Or is there a more specific definition?
It would be an isolated system usually because there is no heat transfer
- Sun Feb 09, 2020 2:34 pm
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: 4H.1 part B
- Replies: 4
- Views: 190
Re: 4H.1 part B
I would look at complexity first. The more orientation it has, the higher the entropy will be. Ne may be heavier but can occupy fewer orientations then NH3.
- Sun Feb 09, 2020 2:33 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Calorimeter and Bomb Calorimeter
- Replies: 4
- Views: 438
Re: Calorimeter and Bomb Calorimeter
Calorimeters measure the temperature difference in a reaction. Bomb calorimeter means that the volume is constant. I would review what it means for a system to be isolated, closed, or open.
- Sun Feb 09, 2020 2:30 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: delta U
- Replies: 8
- Views: 250
Re: delta U
In an adiabatic process, deltaH is equal to 0, so deltaU is equal to work.
- Wed Feb 05, 2020 6:12 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Max work
- Replies: 2
- Views: 101
Re: Max work
It does more work then an irreversible reaction due to that fact.
- Wed Feb 05, 2020 6:11 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: State functions; definition and clarifications
- Replies: 3
- Views: 227
Re: State functions; definition and clarifications
I think about it like this, if you and your friend go on a hike and there are two paths, one more difficult and one easier. You take the easier way while your friend goes the long way. Remember, work = pdeltav but also work= force x distance. If your friend goes a farther distance then you but you b...
- Fri Jan 31, 2020 11:01 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Test 1 #5
- Replies: 7
- Views: 328
Re: Test 1 #5
You're given pKb so you can find Kb. However, in the reaction given you need Ka because HF is an acid. Solve for Ka by using Ka*Kb=Kw, K =1*10^-14. Ka is now your equilibrium constant.Then use the given initial concentration of hydrogen fluoride, 0.12M, and complete an ice table using the Ka consta...
- Thu Jan 30, 2020 1:52 pm
- Forum: Calculating Work of Expansion
- Topic: Work equation
- Replies: 5
- Views: 203
Re: Work equation
Because when work is being done into the surroundings, the system loses energy and thus the work is negative. If work is being done on the system then there is a positive sign.
- Thu Jan 30, 2020 1:15 pm
- Forum: Calculating Work of Expansion
- Topic: Reversible processes and greatest work
- Replies: 3
- Views: 213
Re: Reversible processes and greatest work
It's also easier to think about the amount of work as synonymous with energy or the amount of effort it would take to do something like that.
- Thu Jan 30, 2020 1:14 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Test 1 #5
- Replies: 7
- Views: 328
Test 1 #5
Hi, can someone explain how they got the answer on test 1 for #5? For reference, "The pkb of fluoride is 10.8. A .12 M solution of hydrogen fluoride was made for silicon water processing. What is the pOH of this solution at equilibrium? HF + H2O -> F- + H3O+"
- Mon Jan 27, 2020 12:26 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Extensive vs intensive propeties
- Replies: 5
- Views: 371
Extensive vs intensive propeties
Can someone explain the difference between intensive vs extensive properties?
- Mon Jan 27, 2020 12:24 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Standard Enthalpy of Diatomic Gases
- Replies: 4
- Views: 212
Re: Standard Enthalpy of Diatomic Gases
They have the ability to form naturally with very little energy required but a lot of energy released when formed (thus why it is so stable).
- Tue Jan 21, 2020 6:50 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Chemical Equilibrium Part 4 Question 13
- Replies: 3
- Views: 194
Re: Chemical Equilibrium Part 4 Question 13
I believe part a is correct, treat heat as a product and apply le chatlier.
- Tue Jan 21, 2020 6:48 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Temperature
- Replies: 2
- Views: 136
Re: Temperature
The way I understand it is from treating heat as a reactant/product and therefore apply le chatliers principle to it.
- Tue Jan 21, 2020 6:47 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: salt and water reactions
- Replies: 2
- Views: 139
Re: salt and water reactions
I would just remove an H from the polyprotic acid and give it the conjugate base a negative charge.
- Tue Jan 21, 2020 6:45 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Acids and Bases
- Replies: 7
- Views: 194
Re: Acids and Bases
Will we be given equations on test 1 or will we have to infer whether the molecule acts as an acid or a base?
- Tue Jan 21, 2020 6:42 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Test #1
- Replies: 2
- Views: 201
Re: Test #1
Probably, keep it in mind while doing calculations. Look for the Ka/b value that is lower then 10^-3. If you are unsure you can always calculate it and see that the x is insignificant at the end.
- Mon Jan 13, 2020 12:31 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Change in Pressure
- Replies: 6
- Views: 207
Re: Change in Pressure
I would just know how to look for a change in pressure in terms of moles on each side to make it easier, but also make sure to understand how the changes in pressure affect the molecules themselves,
- Mon Jan 13, 2020 12:29 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Kw calcuation
- Replies: 5
- Views: 233
Re: Kw calcuation
I would suggest to just look at it in terms of concentration, activity seems like an advanced topic for gen chem.
- Mon Jan 13, 2020 12:28 pm
- Forum: General Science Questions
- Topic: Salt Dissolving in Water
- Replies: 3
- Views: 342
Re: Salt Dissolving in Water
I think its a physical change. But I also think you should see someone about this nightmare.
- Mon Jan 13, 2020 12:27 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Water in Equilibrium Constant
- Replies: 2
- Views: 698
Water in Equilibrium Constant
Water is usually implied to be H20(liquid), therefore when do we put it into the Kc equation? Some problems include H20 while others leave it out. Any help would be appreciated
- Mon Jan 13, 2020 12:24 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: PV=nRT
- Replies: 9
- Views: 414
Re: PV=nRT
Concentration of gases would be one of the only reasons we would use the ideal gas law at this point of the class.
- Wed Jan 08, 2020 12:22 pm
- Forum: Ideal Gases
- Topic: Dynamic Equilibrium
- Replies: 10
- Views: 411
Re: Dynamic Equilibrium
It could be disturbed by either taking away/adding products/reactants to the reaction momentarily.
- Wed Jan 08, 2020 12:19 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Concentration
- Replies: 3
- Views: 149
Re: Concentration
When you increase the concentration of a reactant, the reaction must shift left in order to balance out the change in the reaction.
- Wed Jan 08, 2020 12:17 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Comparing Q and K
- Replies: 3
- Views: 124
Re: Comparing Q and K
Q is also calculated the same exact way as the K value would be calculated. The only difference is that it's not at equilibrium.
- Wed Jan 08, 2020 12:15 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Kp of an Aqueous Solution
- Replies: 2
- Views: 298
Re: Kp of an Aqueous Solution
I don't think that would work, gases are usual in concentrations relating to the gaseous form, so making the assumption that it's in the liquid form would be incorrect. I think gaseous products/reactants are most likely always going to be in the Kp form.
- Wed Jan 08, 2020 12:13 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Gibs free energy
- Replies: 3
- Views: 133
Re: Gibs free energy
Gibbs free energy is energy that is able to do work
- Sun Dec 08, 2019 9:29 am
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: melting point
- Replies: 4
- Views: 392
Re: melting point
Determine it by the intermolecular forces of the molecules as compared with another.
- Sat Dec 07, 2019 8:06 pm
- Forum: Conjugate Acids & Bases
- Topic: single arrow vs double arrow
- Replies: 2
- Views: 2011
Re: single arrow vs double arrow
Yea that works
- Sat Dec 07, 2019 8:05 pm
- Forum: Amphoteric Compounds
- Topic: acid, base, or amphoteric
- Replies: 4
- Views: 356
Re: acid, base, or amphoteric
Identify the acid or oxyacid and then determine if it has an electron pair to donate to a proton and therefore maybe also amphoteric.
- Fri Dec 06, 2019 11:10 am
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: pKa and Ka
- Replies: 10
- Views: 636
Re: pKa and Ka
SGonzales_3L wrote:One thing to know that Dr. Lavelle mentioned in class is that if a pKa value is given it is highly likely that that acid is a weak acid. Strong acids strongly favor the products and, thus, have an astronomically large pKa.
Does that mean strong acids have a high conc of H+?
- Fri Dec 06, 2019 11:09 am
- Forum: Sigma & Pi Bonds
- Topic: test 2 #7a
- Replies: 4
- Views: 262
Re: test 2 #7a
i believe it was 11 hydrogen bonding sites if I remember correctly. Count up the number of lone pairs and the number of hydrogens that are bonded to NOF to and add them together to get the number of hbonding sites
- Fri Dec 06, 2019 11:07 am
- Forum: Bronsted Acids & Bases
- Topic: Formic acid strength
- Replies: 2
- Views: 199
Re: Formic acid strength
An acid will be stronger if it can easily lose hydrogen to a base. The CH3 in acetic acid donates electrons which makes the O-H bond stronger due to electronegativity therefore the H is harder to remove, which isn't what we want. This makes formic acid the stronger acid. Basically CH3 is electron d...
- Fri Dec 06, 2019 11:05 am
- Forum: Resonance Structures
- Topic: Resonance
- Replies: 3
- Views: 352
Re: Resonance
Resonance generally makes a molecule stable, therefore it would be less likely to react if put into water. So I would say in general, resonance doesn't correlate with how strong an acid is.
- Fri Dec 06, 2019 11:03 am
- Forum: Bronsted Acids & Bases
- Topic: Strong Acids and Bases
- Replies: 2
- Views: 224
Re: Strong Acids and Bases
Remember when a polyprotic acid gives up a proton (H+), the resulting conjugate base is also able to dissociate more but at a much lower pKa value and is generally not considered a strong acid anymore.
- Tue Dec 03, 2019 10:03 am
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Oxalate denticity
- Replies: 1
- Views: 179
Re: Oxalate denticity
Im pretty sure it always acts a bidentate.
- Tue Dec 03, 2019 10:01 am
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: Confusion about Ph>Pka
- Replies: 2
- Views: 232
Re: Confusion about Ph>Pka
I am also confused about this. In my notes I have that "pH>Pka: the solution is more alkaline and the acid will give off H+ to form A- and is negatively charged." I'm not completely sure what the application of this means though.
- Tue Dec 03, 2019 9:58 am
- Forum: Bronsted Acids & Bases
- Topic: Stronger Acids and Bases
- Replies: 2
- Views: 168
Re: Stronger Acids and Bases
You can use multiple tests. First, check whether each acid/base is a known strong acid or base. For bases, it would be alkaline oxide/hydroxides and for acids, it would be any halogen bonded with hydrogen or an inorganic anion bonded with hydrogen (HNO3). If this isn't the case, I would try to ident...
- Mon Dec 02, 2019 6:53 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: Test 2 7a
- Replies: 6
- Views: 387
Re: Test 2 7a
Jorge Ramirez_4H wrote:Wait, I thought that it was one bonding site. Why do the lone pairs count I thought it explicitly needed to show H bonding to F,O, or N.
Lone pairs count because the resulting shape (trigonal pyramidal, tetrahedral, etc.) may not cancel out the enlarged lone pair thus leaving a delta negative charge
- Tue Nov 26, 2019 12:29 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: 9C.3
- Replies: 4
- Views: 364
Re: 9C.3
Always balance the charges using the outside potassium and not the chromate.