Search found 50 matches
- Fri Mar 12, 2021 6:25 pm
- Forum: General Rate Laws
- Topic: k vs K
- Replies: 6
- Views: 451
Re: k vs K
K is the equilibrium constant while k is the rate constant in kinetics. Furthermore, K = k/k'. k' being the rate constant for the reverse reaction and k being the rate constant for the forward reaction.
- Fri Mar 12, 2021 6:19 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Lowering Activation Energy
- Replies: 34
- Views: 1337
Re: Lowering Activation Energy
Yes! A catalyst lowers the activation energy for both the forward and reverse reactions. This is why the equilibrium constant doesn't change with a catalyst because the rates of both reactions are equally affected.
- Fri Mar 12, 2021 6:12 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Intermediates
- Replies: 6
- Views: 375
Re: Intermediates
Since the intermediates are consumed during the reaction, we never include them in the rate law. However, let's say an intermediate is a reactant in the slow step. We then have to evaluate where this intermediate came from and use that in the rate law.
- Fri Mar 12, 2021 6:07 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Why is the enthalpy of formation method the most accurate?
- Replies: 5
- Views: 699
Re: Why is the enthalpy of formation method the most accurate?
The enthalpy of formation is more accurate compared to using bond enthalpies because the bond enthalpy values given are the average bond enthalpies. These averages are just estimates so they aren't the most accurate. I believe Hess's law is as accurate using enthalpy of formation.
- Fri Mar 12, 2021 6:02 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Kp Units
- Replies: 5
- Views: 468
Re: Kp Units
Technically, the correct unit is bar, however, atm is very close to bar, so we can use both atm and bar when working with partial pressure.
- Fri Mar 05, 2021 1:07 pm
- Forum: General Rate Laws
- Topic: Concentration Denotation
- Replies: 7
- Views: 469
Re: Concentration Denotation
I've always seen concentrated denoted by brackets, especially in equations and formulas. In problems and questions, concentration is often presented in molarity, or moles/liter. However, yes, when it comes to denoting it in formulas it's usually always in brackets as far as I know.
- Fri Mar 05, 2021 1:00 pm
- Forum: First Order Reactions
- Topic: Slope
- Replies: 24
- Views: 1005
Re: Slope
For first-order and zero-order reactions, the slope will be -k and for a second-order reaction, the slope will be +k.The reason the slope is -k for first and zero-order reactions is that the concentration of the reactants decreases over time, but the slope is positive for second-order reactions beca...
- Fri Mar 05, 2021 12:57 pm
- Forum: First Order Reactions
- Topic: 0.693 ?
- Replies: 39
- Views: 8616
Re: 0.693 ?
Essentially, at t = t1/2, [A] = (1/2)[A]0. Then when deriving the equation for the half-life, ln(1/2*[A]/[A_0]) = -kt_1/2, we would have to find ln(1/2), which equals -0.693. After canceling out negatives on both sides we have the value of 0.693.
- Fri Mar 05, 2021 12:52 pm
- Forum: Zero Order Reactions
- Topic: Occurrence of Zero Order Reactions
- Replies: 13
- Views: 814
Re: Occurrence of Zero Order Reactions
In terms of mathematics, the zeroeth rate law is essentially Rate = k. This is because the exponent correlated to the concentration of the reactant in the rate law, Rate = k[A]^n, would be zero and [A]^0 = 1. On a graph of [A] vs time, there would also be a straight line with a negative slope if it ...
- Fri Mar 05, 2021 12:48 pm
- Forum: General Rate Laws
- Topic: Rate Constant
- Replies: 31
- Views: 1288
Re: Rate Constant
Yes, the rate constant can absolutely be altered. One of the ways you can change the rate constant is by altering the temperature. The rate constant can also be changed by altering the activation energy. This can be done by adding a catalyst enzyme (which would lower the activation energy) or by rem...
- Thu Feb 25, 2021 4:33 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: G from K
- Replies: 9
- Views: 536
Re: G from K
So to find delta G, you would need E∘ = (RT/nF)ln(K) and ΔG∘ = -nFE∘. When taking the natural log of a number less than 1, the result is a negative number, and when taking the natural log of a number greater than 1, the result is positive. A K value of less than 1 would result in a negative value th...
- Thu Feb 25, 2021 4:28 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Conceptual understandings
- Replies: 7
- Views: 502
Re: Conceptual understandings
For me, the lectures are helpful, but they may not be to everyone, and so I advise doing what I'd do when the lectures are a bit confusing. The textbooks are always super helpful and many youtube videos are also very helpful, especially for conceptual understanding. A good thing is that most of thes...
- Thu Feb 25, 2021 4:25 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: n in NFE
- Replies: 64
- Views: 4335
Re: n in NFE
Once you balance the redox reaction or even balance the half equations, you should be able to see the coefficient in front of the electrons or see how many electrons are transferred. This number would be the n in the NFE equation.
- Thu Feb 25, 2021 4:21 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Relationship between E naught and spontaneity
- Replies: 8
- Views: 1181
Re: Relationship between E naught and spontaneity
If the E naught value is positive then yes, the redox reaction is spontaneous and favorable. This is true because when E naught is positive, G naught would be negative, thus showing that it is spontaneous and favorable.
- Thu Feb 25, 2021 4:19 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Sapling Week 7/8 #10
- Replies: 4
- Views: 239
Re: Sapling Week 7/8 #10
Yes, I agree with the previous poster. It'd be a great idea to look at the standard reaction potentials and the ones with the higher reduction potential will have a greater ability to act as an oxidation agent.
- Fri Feb 19, 2021 4:42 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Delta U in different systems
- Replies: 4
- Views: 559
Re: Delta U in different systems
I also agree with previous posters that internal energy for an open system would be deltaU = q + w. However, I think this situation is pretty confusing because of all the things to take into account for an open system such as adding in mass or taking mass out. I am not knowledgeable on how this chan...
- Fri Feb 19, 2021 4:31 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: delta U=nCvdeltaT
- Replies: 4
- Views: 2140
Re: delta U=nCvdeltaT
This is not on our equation sheet but it can be deduced. This formula works in constant volume conditions because normally deltaU = q + w. In constant volume, w=0, so deltaU = q. q=nCvdeltaT, therefore deltaU = nCvdeltaT.
- Fri Feb 19, 2021 4:27 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: When does delta H = q?
- Replies: 15
- Views: 5253
Re: When does delta H = q?
Delta H = q at constant pressure or in an isobaric condition. In this condition then Delta U = Delta H + w.
- Fri Feb 19, 2021 4:21 pm
- Forum: Calculating Work of Expansion
- Topic: Work Formula
- Replies: 15
- Views: 851
Re: Work Formula
I'm fairly positive that you only consider the moles of Gas. What makes me believe this is that we would be using the Ideal Gas Constant and this doesn't apply to liquids or solids, or aqueous solutions. I believe in the textbook problems they also only consider moles of gas.
- Fri Feb 19, 2021 4:17 pm
- Forum: Calculating Work of Expansion
- Topic: unit of w
- Replies: 17
- Views: 1304
Re: unit of w
Yes, so when you do P x deltaV the units are in (atm)(L). SO to get it into Joules you need to multiply that answer by 101.325 because 1L.atm = 101.325J.
- Fri Feb 12, 2021 2:05 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: ΔH and q
- Replies: 9
- Views: 506
Re: ΔH and q
delta H and q are the same when pressure is constant. Essentially, qp = delta H, when the change in pressure is zero.
- Fri Feb 12, 2021 1:43 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Temperature for Gibbs Free Energy Calculations
- Replies: 6
- Views: 449
Re: Temperature for Gibbs Free Energy Calculations
I believe that temperature is always in Kelvin for calculations involving Gibbs Free Energy.
- Fri Feb 12, 2021 1:41 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Low temp making DeltaG negative?
- Replies: 8
- Views: 448
Re: Low temp making DeltaG negative?
This would not be possible. When looking at the equation: ∆G = ∆H-T∆S, we can see that by having a negative ∆S, the negatives cancel out thus making the positive change in enthalpy add the temperature times the change in entropy. Thus ∆G could only be positive and non-spontaneous.
- Fri Feb 12, 2021 1:34 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Gibbs and Equilbrium constant
- Replies: 3
- Views: 166
Re: Gibbs and Equilbrium constant
We can relate Gibbs free energy and the Equilibrium constant through some equations. One of which is delta G naught = -RTlnK. From here we can make inferences about their relation. We just recently learned this today in a lecture and I think it answers your question.
- Fri Feb 12, 2021 1:28 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Diff between delta G and delta G nought
- Replies: 3
- Views: 134
Re: Diff between delta G and delta G nought
Delta G is the change in Gibbs Free energy and this is the change for a system during any point in a reaction except at 298K and 1 atm, which is the standard conditions. In these standard conditions, the change in Gibbs Free energy is delta G naught. It is important to note this difference because w...
- Sat Feb 06, 2021 1:37 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: energy replaced by heat
- Replies: 3
- Views: 185
Re: energy replaced by heat
I agree with the previous post, I believe that the heat comes from the surroundings, especially in the diagram he provided during the lecture. However, I'm not entirely sure where the heat would come from in a different scenario, as I don't want to assume that it always comes from the surroundings s...
- Sat Feb 06, 2021 1:30 pm
- Forum: Calculating Work of Expansion
- Topic: integral equation
- Replies: 7
- Views: 346
Re: integral equation
This integral equation is used when there is a reversible pathway, however, it is not necessary to use this exact equation or formula. We learned in the lecture that we could use a much easier equation for the reversible pathway which is: w = -nRTln(V2/V1). This equation is definitely one that is ea...
- Sat Feb 06, 2021 1:24 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Entropy = 0
- Replies: 6
- Views: 272
Re: Entropy = 0
I think you are right on that. Due to O2 having only one type of arrangement, the entropy is 0. Thus, for molecules with only one type of arrangement, the entropy could be 0, because ln1 = 0. Therefore, for diatomic molecules that have two of the same atom, for example, O2, Cl2, or H2, there is only...
- Sat Feb 06, 2021 11:45 am
- Forum: Calculating Work of Expansion
- Topic: Spontaneous
- Replies: 26
- Views: 1650
Re: Spontaneous
If a reaction is spontaneous, that means it can occur without an input of energy, and thus it is favorable. An equation is usually spontaneous when a reaction is exothermic and has high entropy. This is in relation to Gibb's free energy which I'm sure we will go over soon.
- Sat Feb 06, 2021 11:40 am
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Ideal Gas Expansion
- Replies: 7
- Views: 218
Re: Ideal Gas Expansion
The change in internal energy is able to remain the same because the energy lost due to work is replaced as energy in the form of heat. This creates no change and works when you think of the universe as an isolated system. The first law of thermodynamics states that energy cannot be created or destr...
- Sat Jan 30, 2021 11:05 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: percent protonation/deprotonation
- Replies: 15
- Views: 939
Re: percent protonation/deprotonation
Percent protonation is usually calculated when dealing with bases and the Kb constant, and percent deprotonation would be when dealing with acids and the Ka constant. This is because acids can give H+, thus deprotonated, and bases will accept the H+ and get protonated.
- Sat Jan 30, 2021 10:57 am
- Forum: Calculating Work of Expansion
- Topic: Sapling #15
- Replies: 3
- Views: 166
Re: Sapling #15
I was confused about this problem as well for the longest time but then I realized they were asking for the answer in Joules and we have to convert it so it's in joules. You'd just have to multiply your answer by 101.325 J/atm. I didn't really know we had to do this based on the content of the lectu...
- Sat Jan 30, 2021 10:45 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Sapling Question 14
- Replies: 2
- Views: 236
Sapling Question 14
So I was looking at the solution for this question, it advises me to use this formula to find work which is: w = -nRTln(Vfinal/Vinitial). I don't remember learning this in the lecture and I used the formula with the integral instead, but it wasn't correct. I was wondering why the integral formula we...
- Sat Jan 30, 2021 10:37 am
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: q=mCdeltaT
- Replies: 3
- Views: 293
Re: q=mCdeltaT
I'm pretty positive we learned q=mC(Delta T) on Monday's Week 4 lecture. There were quite a bit of sapling questions on this topic so going over Monday's lecture would really help because it is almost entirely about this topic.
- Thu Jan 28, 2021 7:51 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Textbook example 5I.3
- Replies: 4
- Views: 214
Re: Textbook example 5I.3
Since the K value is extremely small and much smaller than 10^-4, we can assume that the x is insignificant. However, only remove the x for the denominators in this case, because we still need to find the actual x value. The x value will just be extremely small.
- Sat Jan 23, 2021 10:17 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Exothermic and Endothermic Reactions
- Replies: 9
- Views: 1371
Re: Exothermic and Endothermic Reactions
Catalysts would not affect the change in enthalpy, whether the reaction is exothermic or endothermic. Because enthalpy is a state function, the path taken isn't relevant to delta H. Catalysts affect only the path taken by lowering the activation energy. So, although the reaction would proceed quicke...
- Sat Jan 23, 2021 10:15 am
- Forum: Phase Changes & Related Calculations
- Topic: H and q
- Replies: 47
- Views: 2018
Re: H and q
q is the denotation for heat (in joules), which is not a state property, and H is the denotation for enthalpy, which is a state property.
- Fri Jan 22, 2021 10:01 pm
- Forum: Phase Changes & Related Calculations
- Topic: Endothermic v. Exothermic
- Replies: 139
- Views: 18882
Re: Endothermic v. Exothermic
An endothermic reaction will always have a positive delta H because, for a reaction to endothermic, it absorbs heat. An exothermic reaction will always be a negative delta H because, for a reaction to be exothermic, it gives off heat.
- Fri Jan 22, 2021 9:51 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: 5J. 5 Textbook problem
- Replies: 3
- Views: 151
Re: 5J. 5 Textbook problem
Hi,
So on professor's website, under the solutions manual errors document, it says that this question has an error in the book. H2 is supposed to be a product, which makes the moles on each side equal. Hope this helps!
So on professor's website, under the solutions manual errors document, it says that this question has an error in the book. H2 is supposed to be a product, which makes the moles on each side equal. Hope this helps!
- Fri Jan 22, 2021 9:41 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Diatomic molecules standard enthalpy of formation
- Replies: 22
- Views: 1416
Re: Diatomic molecules standard enthalpy of formation
I believe that if the diatomic molecule is in their stable state in standard conditions, then the standard enthalpy of formation will be zero.
- Sat Jan 16, 2021 12:25 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: ICE Box
- Replies: 28
- Views: 1422
Re: ICE Box
If you know for certain that you're working with strong acids and strong bases, you don't necessarily need the ICE box because they fully disassociate. So I would use an ICE box for weak acids and bases because they only partially disassociate and it would also help visualize those calculations bett...
- Sat Jan 16, 2021 10:51 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Textbook Question 5I.11
- Replies: 4
- Views: 256
Re: Textbook Question 5I.11
Hi, instead of multiplying by 2, they divided by 0.500. This is essentially the same thing and looked confusing to me at first but then I realized. Hope this helps.
- Sat Jan 16, 2021 10:45 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Weak versus Strong Acid and Base
- Replies: 10
- Views: 601
Re: Weak versus Strong Acid and Base
This is a great question. I came from Chem 20B and we never really went over acids and bases, and we definitely didn't go over which were strong or weak and how to find out. Thanks for bringing this to my attention so that I can memorize the strong ones.
- Sat Jan 16, 2021 10:39 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: When x is negligible in Equilibrium constant
- Replies: 34
- Views: 1745
Re: When x is negligible in Equilibrium constant
In the lecture, I believe we were informed that if the K value is less than 10^-3, we can assume that x is negligible. However, as many others have stated, just to be safe you can use the 5% rule.
- Sat Jan 16, 2021 10:33 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Sapling #5
- Replies: 5
- Views: 290
Re: Sapling #5
Hi! Without giving the answer away, what I did to start was to set up the equilibrium constant ratios for every reaction. For example, the first one would be [HI]^2/[H][I]. I did this for all of the reactions and then noticed which ones would have similar components to the original reaction given to...
- Sat Jan 09, 2021 11:28 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Q and K
- Replies: 46
- Views: 2026
Re: Q and K
Yes, Q is the reaction quotient and is essentially the ratio of products/reactants whenever the reaction is not at equilibrium. K is the ratio when the reaction is at equilibrium. The reaction quotient can help us figure out if the reaction is not at equilibrium and can inform us whether the reactio...
- Sat Jan 09, 2021 11:04 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Partial pressure vs. concentration
- Replies: 3
- Views: 129
Re: Partial pressure vs. concentration
Hi, so you would use usually use partial pressure for gases and when you are solving for Kp and concentrations for solutions and when you are solving for Kc. Or, you can convert partial pressures to concentration and vice versa.
- Sat Jan 09, 2021 10:43 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: terminology
- Replies: 11
- Views: 536
Re: terminology
A forward reaction is when the reaction is forming product or in nontechnical terms, going towards the right, towards the product. A reverse reaction is vice versa, as it is when the reaction is forming reactant. So, when a reaction favors products, it means that the concentration of products is gre...
- Sat Jan 09, 2021 10:30 am
- Forum: Student Social/Study Group
- Topic: Final Exam Study Tips
- Replies: 48
- Views: 2851
Re: Final Exam Study Tips
Hi, like many others have stated, doing practice problems for me are very helpful. It gives me a chance to apply the knowledge we learn and it is very helpful for exams. I also plan to space out my learning. I've been guilty of cramming my studying in the final days before an exam and it can be pret...
- Fri Jan 08, 2021 10:51 am
- Forum: Student Social/Study Group
- Topic: Resources Outside of Class
- Replies: 6
- Views: 352
Resources Outside of Class
Hey everyone, I know this has been asked and answered many times but I'd still like to get clarification on this as I've never experienced this before. Last quarter I took Chem 20A and we had no extra resources outside of class. This class has many and so I'm a bit confused and overwhelmed by the di...