Search found 31 matches
- Sat Mar 18, 2023 5:56 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: what does i-> 0 represent
- Replies: 2
- Views: 138
Re: what does i-> 0 represent
Hello, I believe that i---->0 is meant to represent the notation for when the battery has max voltage at it's initial stage. This is when the hatch it still open on the circuit, and there is little to no electron flow because of the disconnect from the anode to the cathode. After the hatch is close ...
- Sat Mar 18, 2023 5:43 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Week 1 Achieve, question # 8
- Replies: 4
- Views: 583
Re: Week 1 Achieve, question # 8
Hello, For this problem, our only hint is that the reaction produces a negative enthalpy. A negative enthalpy indicates that the reaction is exothermic; this is important because when the temperature is increased and it produces an exothermic reaction, we know that K has decreased. Therefore if K ha...
- Sat Mar 18, 2023 11:15 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Initial Voltage
- Replies: 4
- Views: 290
Re: Initial Voltage
Hello, The initial voltage can also be thought of as the Ecell. The max voltage is the initial voltage because we have the hatch open on the circuit that connects the anode and cathode. If this hatch remains open that means that electrons cannot flow from the anode to cathode because there is 'break...
- Sat Mar 18, 2023 11:06 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Inert Electrodes
- Replies: 3
- Views: 668
Re: Inert Electrodes
Hello, From I understanding, we need to add inert electrodes like Platinum when half reactions both only have products with aqueous states; this implies that there are no solids in the reaction. This problematic because solid electrodes are used as conductors that allow electron transfer ( cu, zn, a...
- Sat Mar 18, 2023 10:43 am
- Forum: Zero Order Reactions
- Topic: Half Lives and Temperature
- Replies: 3
- Views: 129
Re: Half Lives and Temperature
Hello, From my understanding, half-life reactions are indirectly influenced by temperature. k, the rate constant, is directly affected by temperature; when temperature increases, k increases as well. As we have learned, k and the half-life are inverse of each other, meaning that when the temperature...
- Fri Mar 17, 2023 4:07 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Nernst equation
- Replies: 3
- Views: 182
Re: Nernst equation
Hello, Both sides of the equation are the same, but the right side is a bit more helpful because we can use 2.303 as tangible number to then plug in the rest of our variables. We got to the left side (w/2.303) by changing lnQ (on the right) to logQ (on the left): ln 10 = 2.302585093 OR log=1. For ex...
- Fri Mar 17, 2023 4:05 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Inert Electrode
- Replies: 3
- Views: 133
Re: Inert Electrode
Hello, From I understand we need to add inert electrodes like Platinum when half reactions both only have products with aqueous states; this implies that there are no solids in the reaction. This problematic because solid electrodes are used as conductors that allow electron transfer ( cu, zn, ag, e...
- Fri Mar 17, 2023 3:34 pm
- Forum: Calculating Work of Expansion
- Topic: Irreversible vs. Reversible Expansion
- Replies: 3
- Views: 653
Re: Irreversible vs. Reversible Expansion
Hello, Reversible reactions are an unnatural phenomena (which makes sense due to lack of spontaneity when going in the reverse), but they are more efficient than irreversible reactions. Although irreversible processes do less work, they are unable t conserve energy and cause the entropy to change mu...
- Fri Mar 17, 2023 2:57 pm
- Forum: General Rate Laws
- Topic: intermediates
- Replies: 11
- Views: 328
Re: intermediates
Hello, Intermediate's purpose is to help reaction to create the final product. Therefore it is only a mechanism that is being utilized, but is not the purpose of the reaction, and therefore will not be in the final equation. Intermediates are created by reactants in a prior step, but will eventually...
- Fri Mar 17, 2023 2:46 pm
- Forum: Second Order Reactions
- Topic: achieve hw #12
- Replies: 5
- Views: 784
Re: achieve hw #12
Hey, So we can identify that this is a second order reaction by looking at the relationship between time and concentration. In this problem, the half-life first decomposes at 165s when its initial concentration is 0.264 M, and also decomposes with a half‑life of 207 s when its initial concentration ...
- Sun Mar 05, 2023 11:27 pm
- Forum: Balancing Redox Reactions
- Topic: Achieve week 7/8 Q9
- Replies: 9
- Views: 570
Re: Achieve week 7/8 Q9
First you can identify the reduction potentials for both ions in the table [Mg2+(aq)+2e−⟶Mg(s) E=−2.38 V and Cu+(aq)+e−⟶Cu(s) E=+0.52 V]. Since we are dealing with a galvanic cell, we know that reaction is spontaneous and therefore the cell potential is positive. In order to finish the problem we ne...
- Sun Mar 05, 2023 11:09 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Standard Cell Potential and Free Energy
- Replies: 2
- Views: 114
Re: Standard Cell Potential and Free Energy
Two equations help to understand the correlation: DeltaG0=−RTln(K) and E0cell=−DeltaG0/nF. When K is 1 (equilibrium), we know that G0 equals 0 because there is no spontaneity, DeltaG0=−RT(1)=0. Now that we see that DeltaG0 is zero when K is 1, then we can plug in 0 into our second equation and see t...
- Sun Mar 05, 2023 11:09 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Standard Cell Potential and Free Energy
- Replies: 2
- Views: 114
Re: Standard Cell Potential and Free Energy
Two equations help to understand the correlation: DeltaG0=−RTln(K) and E0cell=−DeltaG0/nF. When K is 1 (equilibrium), we know that G0 equals 0 because there is no spontaneity, DeltaG0=−RT(1)=0. Now that we see that DeltaG0 is zero when K is 1, then we can plug in 0 into our second equation and see t...
- Sun Mar 05, 2023 10:20 pm
- Forum: Balancing Redox Reactions
- Topic: Oxidizing vs Reducing Agents
- Replies: 6
- Views: 1543
Re: Oxidizing vs Reducing Agents
Oxidizing and reducing agents are a bit confusing because they are doing/ causing their namesakes but the end result for them is the opposite. Oxidizing agents oxidize other molecules by accepting more electrons; because they accept electrons in order to cause oxidation, they end up with a more nega...
- Sun Mar 05, 2023 10:03 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Achieve Week 7/8 #17
- Replies: 7
- Views: 205
Re: Achieve Week 7/8 #17
Using the Nerst equation, first we have to identify the reduction reaction of SHE, which is 2H+(aq)+2e−↽−−⇀H2(g). Knowing that the potential reaction under the standard conditions is 0V, we know that E naught is also 0V. We also know that since 2 electrons are being transferred, that the n in the Ne...
- Sun Feb 12, 2023 11:44 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Achieve Weeks 3 & 4: Delta U and q
- Replies: 1
- Views: 66
Re: Achieve Weeks 3 & 4: Delta U and q
I believe it is because as we add heat to the gas, it begins to expand which means that we have to take volume into account. I hope this made sense and helped!
- Sun Feb 12, 2023 11:36 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Achieve weeks 3-4 #17
- Replies: 7
- Views: 220
Re: Achieve weeks 3-4 #17
You have to find the relation between Cv and Cp to answer the question. Since Cv=Cp-R the Cv=5/2. Now you just multiply the #moles* Cv * R constant* Temp change. Hope this helps!
- Sun Feb 12, 2023 11:27 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Midterm 2
- Replies: 2
- Views: 247
Re: Midterm 2
Hey, I was wondering the same thing but I'm assuming it will be weeks 3-6, maybe 3-5 if he is feeling merciful. Good luck!
- Sun Feb 05, 2023 10:35 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 5126032
Re: Post All Chemistry Jokes Here
Chemists are so happy in the lab because they're in their element.
- Sun Feb 05, 2023 10:31 pm
- Forum: Student Social/Study Group
- Topic: Chemistry News
- Replies: 135
- Views: 287464
Re: Chemistry News
Thought this was pretty interesting and relevant given the past couple of years:
https://www.sciencedaily.com/releases/2 ... 124418.htm
https://www.sciencedaily.com/releases/2 ... 124418.htm
- Sun Feb 05, 2023 10:31 pm
- Forum: Student Social/Study Group
- Topic: Chemistry News
- Replies: 135
- Views: 287464
Re: Chemistry News
Thought this was pretty interesting and relevant given the past couple of years:
https://www.sciencedaily.com/releases/2 ... 124418.htm
https://www.sciencedaily.com/releases/2 ... 124418.htm
- Mon Jan 30, 2023 9:39 am
- Forum: Administrative Questions and Class Announcements
- Topic: Textbook Answer Key
- Replies: 1
- Views: 152
Textbook Answer Key
Hey, I was working through the practice problems for the textbook, but I can't find the answer key. Please let me know if anyone knows where to find it, thanks!
- Sun Jan 29, 2023 10:14 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Exam Logistics
- Replies: 1
- Views: 77
Exam Logistics
Hello, does anyone know how many questions will be on the exam and how long we have to complete it? thanks!
- Sun Jan 29, 2023 10:11 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Achieve Week 2 Question 7 and 8
- Replies: 3
- Views: 190
Re: Achieve Week 2 Question 7 and 8
Hey, So for question 7, as an example, they give us the Ka but say that the salt acts as weak base. This tells us that we need to figure out the Kb by using the Kw expression (ka * kb= 10^-14)\. Once you figure out kb then the equation proceeds like normal: use the ice table, solve for x, and then u...
- Sun Jan 29, 2023 10:03 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Midterm
- Replies: 20
- Views: 848
Re: Midterm
hey, so it will be in person on Wednesday at 6pm, but we need respondus downloaded because we are taking the exam on our computers. We will be able to write our equations on pen and paper, btu we submit answers online. Good luck!
- Sun Jan 22, 2023 12:28 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Sig Figs number [ENDORSED]
- Replies: 6
- Views: 371
Re: Sig Figs number [ENDORSED]
I think it depends on each question, and you look for how many sfs are present in the given numbers.
- Fri Jan 20, 2023 12:32 pm
- Forum: Administrative Questions and Class Announcements
- Topic: In Person Friday's For Online Students
- Replies: 2
- Views: 168
Re: In Person Friday's For Online Students
Hi, he posts the lectures on bruinlearn after class. All the lectures are under the tab labeled UCLA Media Reserves. Hope this helps!
- Tue Jan 17, 2023 11:21 am
- Forum: Student Social/Study Group
- Topic: Exam Dates
- Replies: 1
- Views: 123
Exam Dates
Hey, I was wondering if anyone knew what day our midterms and final are? Thanks!
- Sun Jan 15, 2023 5:23 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Homogeneous and Heterogenous Reactions
- Replies: 6
- Views: 176
Re: Homogeneous and Heterogenous Reactions
If solids and liquids are given in a reaction they sould NOT be used when solving the K equation. Only gases and aqueous solutions should be solved in K equations.
- Sun Jan 15, 2023 5:17 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: changes in concentration
- Replies: 7
- Views: 198
Re: changes in concentration
The concentration would change if the volume is changed because concentration is partially dependent on the amount of volume. Now that the concentration has changed the reaction can not be equilibrium any longer and we would have to use Q to solve for the reaction.
- Sun Jan 15, 2023 5:13 pm
- Forum: Ideal Gases
- Topic: Kc vs Kp vs K
- Replies: 28
- Views: 2953
Re: Kc vs Kp vs K
K, Kc, and Kp are all used for the same equation (P/R), but they just specify what units the products and reactants used.