Hi
How can we tell which step is the slow step and which is the fast one? Or will it always be given which one is the slow step and the fast step?
Search found 35 matches
- Sat Mar 18, 2023 5:39 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Reaction Mechanisms
- Replies: 4
- Views: 437
- Mon Mar 13, 2023 11:00 am
- Forum: General Rate Laws
- Topic: Achieve 8-10 #1
- Replies: 7
- Views: 228
Re: Achieve 8-10 #1
In order to start solving this question. First, we can write down the general formula: rate = -\frac{\Delta [a]}{\Delta t} = -\frac{1}{3}\frac{\Delta [B]}{\Delta t} = \frac{1}{2}\frac{\Delta[C]}{\Delta t} . Then we can arrange this to solve for the relative rate of change of each species: \frac{\Del...
- Mon Mar 13, 2023 10:40 am
- Forum: General Rate Laws
- Topic: Homework Q13
- Replies: 3
- Views: 157
Re: Homework Q13
In this problem, we know that rate is based on the slowest step. So, first, we have to identify the slowest step in the mechanism, which is I-(aq) + HClO(aq) --> HIO(aq) +Cl- (aq). After this, we can apply our slowest step to the rate law: rate= k slow [HClO][I-]. However, step 1 has HClO as a produ...
- Wed Mar 08, 2023 10:48 am
- Forum: *Free Energy of Activation vs Activation Energy
- Topic: Sapling #15 Wk.9-10
- Replies: 6
- Views: 14749
Re: Sapling #15 Wk.9-10
For this problem use the arrhenius equation k = Ae^−EaRT where A is the frequency factor 8.07×1011. You should convert the temperature into Kelvin from Celsius, rearrange the equation to kA = e^−EaRT and take the natural log of both sides so that your equation becomes Ea =−RTln(k/A). You can then i...
- Tue Mar 07, 2023 10:13 am
- Forum: General Rate Laws
- Topic: Bimolecular vs Unimolecular
- Replies: 46
- Views: 4459
Re: Bimolecular vs Unimolecular
Unimolecular is when there is only one reactant in the reaction, while Bimolecular Is when there are two reactants in the reaction. For instance,
Unimolecular: A --> C
Bimolecular: A + B --> C
Unimolecular: A --> C
Bimolecular: A + B --> C
- Tue Mar 07, 2023 10:07 am
- Forum: General Rate Laws
- Topic: Rate Constant
- Replies: 50
- Views: 1825
Re: Rate Constant
represents the forward rates for multi-step reactions, while K' represent the reverse rate constant
- Tue Mar 07, 2023 10:04 am
- Forum: General Rate Laws
- Topic: Rate-determining step
- Replies: 19
- Views: 614
Re: Rate-determining step
To tell which step is the rate-determining step is to find which step is the slowest because the slowest step among the given reaction will always be the rate-determining step
- Tue Mar 07, 2023 10:02 am
- Forum: General Rate Laws
- Topic: Overall order
- Replies: 67
- Views: 2430
Re: Overall order
In order to find the overall order, you will have to sum up the exponents of each reactant.
- Tue Mar 07, 2023 12:03 am
- Forum: General Rate Laws
- Topic: Week 8-10, Question5
- Replies: 8
- Views: 252
Week 8-10, Question5
Hi,
Can someone elaborate on how to approach this problem, please? I've been trying to solve this problem. However, I keep getting the wrong answers. Thank you!
Can someone elaborate on how to approach this problem, please? I've been trying to solve this problem. However, I keep getting the wrong answers. Thank you!
- Thu Mar 02, 2023 1:20 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Anode vs Cathode
- Replies: 17
- Views: 724
Re: Anode vs Cathode
The reduction half-reaction (right) and oxidation half-reaction (left) are separated into two half cells by the salt bridge. The half-reaction cell where oxidation (left) occurs is called the anode, while the half-cell where reduction occurs is called the cathode (right).
- Thu Mar 02, 2023 10:41 am
- Forum: Balancing Redox Reactions
- Topic: Oxidized v Reduced
- Replies: 79
- Views: 3751
Re: Oxidized v Reduced
here is a useful Mneonic:
LEO says GER
Losing Electron is Oxidation, while Gaining Electron is Reduction
LEO says GER
Losing Electron is Oxidation, while Gaining Electron is Reduction
- Wed Mar 01, 2023 2:32 pm
- Forum: Balancing Redox Reactions
- Topic: Sapling week 7/8 #18
- Replies: 25
- Views: 5678
Re: Sapling week 7/8 #18
Thank you so much for the answer! This is extremely helpful!
- Wed Mar 01, 2023 10:41 am
- Forum: Balancing Redox Reactions
- Topic: Week 7 and 8, question 5
- Replies: 3
- Views: 160
Week 7 and 8, question 5
Hi, I am stuck on the balancing equation part of question 5. I'm having a hard time using H2O or OH- to cancel things out. Can anyone demonstrate to me how to do this one, please? So I can see how to use H2O or OH- to balance it. Also, how do we know whether we must use H2O or OH- to balance the equ...
- Wed Mar 01, 2023 12:53 am
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 4917658
Re: Post All Chemistry Jokes Here
Hey Exothermic, you are so good at making bonds and the energy you give off is so hot. Do you want to hang out anytime tomorrow?
- Wed Mar 01, 2023 12:40 am
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 4917658
Re: Post All Chemistry Jokes Here
You must be built from Copper and Tellurium... because you are so CuTe
- Tue Feb 28, 2023 5:39 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: enthalpy and q
- Replies: 5
- Views: 208
Re: enthalpy and q
DeltaH and q are not similar. q is the amount of heat that the system absorbs or releases, whereas DeltaH, or enthalpy, is the amount of heat that the system absorbs or releases only when the pressure is constant.
- Tue Feb 28, 2023 3:34 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: What is the difference between heat and enthalpy?
- Replies: 15
- Views: 1617
Re: What is the difference between heat and enthalpy?
Heat transfers energy due to temperature differences, while enthalpy is the amount of heat released or absorbed in a reaction under constant pressure.
- Tue Feb 28, 2023 3:29 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Entropy
- Replies: 7
- Views: 364
Re: Entropy
You do not have to calculate to find Cp of water because it is given in the table.
- Tue Feb 28, 2023 3:23 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Forming and breaking bonds
- Replies: 12
- Views: 767
Re: Forming and breaking bonds
Yes
Breaking bond requires energy --> enthalpy (positive) --> endothermic
Forming bond releases energy --> enthalpy (negative) --> exothermic
Breaking bond requires energy --> enthalpy (positive) --> endothermic
Forming bond releases energy --> enthalpy (negative) --> exothermic
- Tue Feb 28, 2023 3:10 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: delta U
- Replies: 18
- Views: 935
Re: delta U
Yes, Delta U is a state function because the path to get to the final value does not matter since they only depend on the state of the system that is independent
- Tue Feb 28, 2023 3:06 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: q and delta H
- Replies: 6
- Views: 231
Re: q and delta H
q and DeltaH are not the same. q is the amount of heat absorbed or released by the system, while DeltaH, or enthalpy, is the amount of heat absorbed or released by the system only at constant pressure
- Tue Feb 28, 2023 2:59 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: q
- Replies: 8
- Views: 240
Re: q
qp=ΔH are always equal if it's for constant pressure, but if that is not the case, then they are not always equal
- Thu Feb 23, 2023 12:00 am
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: week 5 and 6 question 3
- Replies: 3
- Views: 256
week 5 and 6 question 3
Hi,
Can someone show me how to solve part A? I use the equation n=PV/RT to find the moles and then w=-nRTln(v2/v1), but I keep getting the wrong answer.
Can someone show me how to solve part A? I use the equation n=PV/RT to find the moles and then w=-nRTln(v2/v1), but I keep getting the wrong answer.
- Sun Feb 19, 2023 11:37 am
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: week 5 and 6 question 6
- Replies: 1
- Views: 90
week 5 and 6 question 6
Hi,
Can someone explain to me how to find the change of entropy for gas, please? I used the formula delta S = nR ln(V2/V1) then delta S = Cv ln(T2/T1)
but I keep getting the wrong answers.
Can someone explain to me how to find the change of entropy for gas, please? I used the formula delta S = nR ln(V2/V1) then delta S = Cv ln(T2/T1)
but I keep getting the wrong answers.
- Sun Feb 12, 2023 11:28 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: When -q(metal) = q(H2O) does it matter which is negative?
- Replies: 11
- Views: 687
Re: When -q(metal) = q(H2O) does it matter which is negative?
Hi,
No, it shouldn't matter which q is negative. The negative is commutative, so it does not matter. But it helps with understanding the problem if the +q is on the side that gained heat, while the -q is on the side that loses heat.
No, it shouldn't matter which q is negative. The negative is commutative, so it does not matter. But it helps with understanding the problem if the +q is on the side that gained heat, while the -q is on the side that loses heat.
- Sun Feb 05, 2023 11:35 am
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Week 3 and 4 Assignment, Q 17
- Replies: 2
- Views: 253
Re: Week 3 and 4 Assignment, Q 17
Hi Mathangi,
Can you please show me how to do it? I feel like I am using the correct formulas to find the deltaU but I am making some mistakes in calculation, and I could not figure out what I did wrong. Thank you!
Can you please show me how to do it? I feel like I am using the correct formulas to find the deltaU but I am making some mistakes in calculation, and I could not figure out what I did wrong. Thank you!
- Sun Feb 05, 2023 12:03 am
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Week 3 and 4 Assignment, Q 17
- Replies: 2
- Views: 253
Week 3 and 4 Assignment, Q 17
Hi,
Can someone explain how to the deltaU on this problem? I tried to assume that work was O, but it was wrong. Then I tried to use PV=nRT to find the w and then solve for deltaU with the formula deltaU=q+w, but my answer was still incorrect. Any help would be much appreciated! Here is the question:
Can someone explain how to the deltaU on this problem? I tried to assume that work was O, but it was wrong. Then I tried to use PV=nRT to find the w and then solve for deltaU with the formula deltaU=q+w, but my answer was still incorrect. Any help would be much appreciated! Here is the question:
- Sat Feb 04, 2023 11:23 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Week 3 and 4 Assignment, Q 15
- Replies: 1
- Views: 150
Week 3 and 4 Assignment, Q 15
Hi,
I am having trouble with this question. Can someone explain or explain how to answer this question, please? Any help would be much appreciated! Here is the question:
I am having trouble with this question. Can someone explain or explain how to answer this question, please? Any help would be much appreciated! Here is the question:
- Tue Jan 31, 2023 4:41 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: HW 5.39
- Replies: 1
- Views: 150
HW 5.39
Hi,
Can someone explain how to solve part a because I've been trying and could not get the correct answer? Thank you!
Can someone explain how to solve part a because I've been trying and could not get the correct answer? Thank you!
- Sun Jan 29, 2023 12:14 am
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Achieve Week 2 Q5
- Replies: 4
- Views: 338
Re: Achieve Week 2 Q5
Hi, Since they give Kb and pH, we are going to use the given base to get pOH pOH = 14 - pH (9.462) --> pOH = 4.538 then use that pOH to find the [OH-]=[BH+] [OH-] = 10^(-4.538) = 2.897x10^-5 then use this equation to find the [B]: Kb = ([OH-][BH+])/[B] Now, you find [B], to determine the percentage ...
- Fri Jan 20, 2023 9:43 pm
- Forum: Student Social/Study Group
- Topic: Question about the discussion worksheet
- Replies: 1
- Views: 316
Question about the discussion worksheet
Hi,
I had my discussion today, and according to my TA, the answers for the worksheet are posted on bruinlearn. However, I've been looking at it on bruinlearn and can't find it anywhere. Does anyone here know where the answers for the worksheets were given to us during our discussion?
I had my discussion today, and according to my TA, the answers for the worksheet are posted on bruinlearn. However, I've been looking at it on bruinlearn and can't find it anywhere. Does anyone here know where the answers for the worksheets were given to us during our discussion?
- Fri Jan 20, 2023 9:40 pm
- Forum: Student Social/Study Group
- Topic: Fave food
- Replies: 266
- Views: 76135
Re: Fave food
Sweet spaghetti and for dessert is tiramisu
- Wed Jan 18, 2023 9:38 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Achieve Question #10 Part d
- Replies: 5
- Views: 184
Re: Achieve Question #10 Part d
Hi, Tiffany Wang
We have the same problem, but I got 0.182 for x instead of 0.21955 (which is the right value for x). Can you show your work, please? because I redo my work and I still got 0.182 for x. Thank you!
We have the same problem, but I got 0.182 for x instead of 0.21955 (which is the right value for x). Can you show your work, please? because I redo my work and I still got 0.182 for x. Thank you!
- Mon Jan 16, 2023 12:07 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Question 4 Achieve Homework
- Replies: 2
- Views: 121
Question 4 Achieve Homework
Hi,
I am having some trouble with Achieve Question #5. I have no idea where to start or what to compute to determine the equilibrium constant, K, for the reaction of NH3 with I2. Any help would be appreciated! I've attached the problem. Thank you!
I am having some trouble with Achieve Question #5. I have no idea where to start or what to compute to determine the equilibrium constant, K, for the reaction of NH3 with I2. Any help would be appreciated! I've attached the problem. Thank you!
- Sun Jan 15, 2023 2:20 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Spontaneity
- Replies: 57
- Views: 3955
Re: Spontaneity
The reaction is spontaneous when delta G is negative