Because we are using the unique rate of E, we put 1/(coefficient) in front of the rate. The coefficient in this case is 2, so we have 1/2 d[E]/dt.
In a general rate, we would not use the stoichiometric coefficient.
Search found 51 matches
- Sat Mar 17, 2018 12:12 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Q7b Lyndon's Review
- Replies: 6
- Views: 729
- Mon Mar 12, 2018 5:17 pm
- Forum: Biological Examples
- Topic: Nitric Oxide Catalyses
- Replies: 7
- Views: 1679
Re: Nitric Oxide Catalyses
diangelosoriano wrote:Is there a way to tell by looking at these equations if the catalyst was heterogeneous or homogeneous?
A catalyst is homogeneous if it is in the same phase as the reactant R.
It is heterogeneous when it is in a different phase as R; in this case it is usually a solid.
- Mon Mar 12, 2018 5:12 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Slow Step in Reaction Mechanisms
- Replies: 7
- Views: 3052
Re: Slow Step in Reaction Mechanisms
If I am understanding your question correctly: I believe that if the early step is the slow step, yes, the overall reaction rate is the rate of that first slow step. If the early step is fast, however, and the second step is the slow step, there is a "bottleneck" effect and a build-up of i...
- Mon Mar 12, 2018 4:36 pm
- Forum: *Free Energy of Activation vs Activation Energy
- Topic: Relation between k and activation energy
- Replies: 10
- Views: 5663
Re: Relation between k and activation energy
diangelosoriano wrote:If a catalyst were added, how would this also affect k or activation energy?
When you add a catalyst, the reaction is sped up - k is increased and Ea is lowered. The new pathway has a lower activation energy.
- Tue Mar 06, 2018 5:18 pm
- Forum: General Rate Laws
- Topic: Half Reaction rate
- Replies: 1
- Views: 280
Re: Half Reaction rate
I believe you are talking about the Half-life for a first order rxn: 1) Start with the integrated rate law: ln [A] = -kt + ln [A] o 2) At t = t 1/2 , [A] = 1/2[A] o 3) Substitute in 1/2[A] o : ln 1/2[A] o = -kt 1/2 + ln [A] o 4) Separate variables: ln 1/2[A] o - ln [A] o = -kt 1/2 5) Simplify: ln 1/...
- Tue Mar 06, 2018 5:14 pm
- Forum: General Rate Laws
- Topic: Integrating
- Replies: 2
- Views: 374
Re: Integrating
1) Start with: d[A]/dt = k[A]
2) Separate the variables: d[A]/[A] = -k dt
3) Integrate both sides: ln [A] = -kt + C
4) Because at t=0, ln[A]o = C: ln [A]t = -kt + ln [A]o
2) Separate the variables: d[A]/[A] = -k dt
3) Integrate both sides: ln [A] = -kt + C
4) Because at t=0, ln[A]o = C: ln [A]t = -kt + ln [A]o
- Tue Mar 06, 2018 5:10 pm
- Forum: First Order Reactions
- Topic: Psuedo First Order Reaction
- Replies: 2
- Views: 343
Re: Psuedo First Order Reaction
So when we have a reaction with multiple reactants changing, such as A + B + C -> P, we make one [R] small and the others very large. In practice, we would thus have: k' = [A] N , just like in a normal first-order rate problem (except the fact that we denote k as k'). Then you would do the same by m...
- Tue Feb 27, 2018 11:01 am
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: 5.13
- Replies: 2
- Views: 422
Re: 5.13
Convert grams to mols using molar masses of H2 and I2. Then use .750 L to convert it to Molarity. You should have roughly 0.35 mol/L H2 and 0.001 mol/L I2.
Rate = k[H2][I2]
Rate = 2.2 x 10-5 mol/(L x S)
Rate = k[H2][I2]
Rate = 2.2 x 10-5 mol/(L x S)
- Tue Feb 27, 2018 10:39 am
- Forum: General Rate Laws
- Topic: 15.3/Unique Rate
- Replies: 2
- Views: 345
Re: 15.3/Unique Rate
Did you mean the reaction: 2NO2 -> 2NO + O2?
Then yes, the decomposition of NO2 is used to find the unique rate of the reaction which is 1/2(Δ[NO2]/Δt)
Then yes, the decomposition of NO2 is used to find the unique rate of the reaction which is 1/2(Δ[NO2]/Δt)
- Tue Feb 27, 2018 10:33 am
- Forum: General Rate Laws
- Topic: 15.17
- Replies: 4
- Views: 655
Re: 15.17
With respect to [B], the reaction is second-order. You use the different values for the rates and concentrations to solve for the exponents (x, y, z) on the concentrations.
- Thu Feb 22, 2018 3:18 pm
- Forum: First Order Reactions
- Topic: 15.15
- Replies: 4
- Views: 595
Re: 15.15
The concentration increased by a factor of 1.2 means that the rate of the reaction also increases by a factor of 1.2:
1.2Rate = k [1.2CH3Br]x[OH-]y
1.2Rate = k [1.2CH3Br]x[OH-]y
- Thu Feb 22, 2018 3:10 pm
- Forum: Balancing Redox Reactions
- Topic: Textbook 14.1
- Replies: 3
- Views: 500
Re: Textbook 14.1
The balanced reduction half reaction should be Cr2O72- (aq) + 14H+ (aq) + 6e- -> 2Cr3+ (aq) + 7H2O (l)
- Thu Feb 22, 2018 3:00 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell Diagram Order for Same Phases
- Replies: 4
- Views: 613
Re: Cell Diagram Order for Same Phases
The elements in the anode are to the left of the salt bridge and the cathode on the right. From there, I believe each side is written in order of reactants to products.
- Thu Feb 15, 2018 4:52 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: s vs. delta s
- Replies: 7
- Views: 1733
Re: s vs. delta s
When dealing with statistical/residual entropy and the make-up of molecules and crystals, we will use S = K + ln W to calculate is as a value. When dealing with reactions and changes, we have delta S = q/T and other derivations that reflect delta S as a state function.
- Thu Feb 15, 2018 4:49 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Isothermal
- Replies: 2
- Views: 466
Re: Isothermal
Internal energy is a state function dependent on temperature, thus, when temperature does not change (definition of isothermal), there is no change in internal energy. Additional note: Dealing with ideal gases, contributions to U are kinetic energy and intermolecular interactions. The latter is 0, b...
- Thu Feb 15, 2018 4:43 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Standard Gibbs Free Energy
- Replies: 3
- Views: 482
Re: Standard Gibbs Free Energy
Standard Gibbs Free Energy entails 1 bar of pressure and a specified temperature (in this case being 25oC (298 K)). Otherwise, it should be noted as just a "Gibbs Free Energy" value.
- Mon Feb 05, 2018 4:08 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: hw9.47b
- Replies: 1
- Views: 286
Re: hw9.47b
For "free expansion" we know that ∆U = 0 and w = 0. Since ∆U = q + w, q = ∆U - w = 0 (qSYS = 0),
qsys = -qsurr, thus qsurr = 0.
Calculating ∆Ssurr = qsurr/T = 0/323 = 0; ∆Ssurr = 0.
qsys = -qsurr, thus qsurr = 0.
Calculating ∆Ssurr = qsurr/T = 0/323 = 0; ∆Ssurr = 0.
- Mon Feb 05, 2018 3:59 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Homework Problem 9.17
- Replies: 1
- Views: 306
Re: Homework Problem 9.17
I believe you are asking about Problem 9.19? If so, we need to find the standard entropy of the vaporization of water at 85 o C because that is what the problem is asking of us. We have ∆S TOT = ∆S 1 + ∆S 2 + ∆S 3 . ∆S 1 = Heat Capacity of liquid water x ln T 2 /T 1 or 75.3 x ln 373/358 ∆S 2 = Stand...
- Mon Feb 05, 2018 3:52 pm
- 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: 9.27 Part D
- Replies: 1
- Views: 273
Re: 9.27 Part D
Volume is inversely proportional to the pressure, and with a decrease in volume (increase of pressure), the random movement of gaseous molecules decreases. Thus, the molar entropy decreases. I'm pretty sure that in this case we are regarding T as a constant.
- Wed Jan 31, 2018 2:08 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: 9.5
- Replies: 5
- Views: 613
Re: 9.5
∆STOT = ∆SSYS + ∆SSURR. When heat is leaving the system, the value is negative. As heat leaves the system, it enters the surroundings.
- Wed Jan 31, 2018 2:00 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Class Example
- Replies: 6
- Views: 598
Re: Class Example
Setting T = 333K is not the final answer; it's the "boiling point." But it is necessary to find that value to come up with the final answer: T > 333K favors the forward reaction and makes delta G negative.
- Wed Jan 31, 2018 1:58 pm
- 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: Homework 9.25
- Replies: 1
- Views: 336
Re: Homework 9.25
You have the correct initial equation with (1.38 x 10-23) x ln(66.02 x 10^23). Using properties of natural logs, move the exponent NA in front of the natural log:
(1.38 x 10-23) x (6.02 x 1023) x (ln 6) and this will get you 14.9 J/K
(1.38 x 10-23) x (6.02 x 1023) x (ln 6) and this will get you 14.9 J/K
- Wed Jan 24, 2018 3:41 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Textbook 8.113
- Replies: 1
- Views: 270
Re: Textbook 8.113
Using mean bond enthalpies will result in an answer close to that of the answer from enthalpy of formation, but will be different because the bond enthalpy method is less accurate (uses averages).
- Wed Jan 24, 2018 3:38 pm
- Forum: Calculating Work of Expansion
- Topic: 8.93
- Replies: 3
- Views: 461
Re: 8.93
The problem states that this is a combustion reaction at 25°C. The two products that come from combustion are CO2(g) and H2O - the H2O is liquid water because the combustion happens at room temperature.
- Wed Jan 24, 2018 3:34 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Homework 8.55
- Replies: 2
- Views: 276
Re: Homework 8.55
To balance the second equation, you must add the coefficient 3/2 to O2. This does not change the enthalpy of the reaction because the enthalpy of an element in its natural elemental state, such as O2 gas, is zero.
- Thu Jan 18, 2018 10:46 am
- Forum: Calculating Work of Expansion
- Topic: Homework 8.11
- Replies: 8
- Views: 865
Re: Homework 8.11
An irreversible expansion happens instantaneously while a reversible expansion maximizes work. For the reversible expansion, you solve with dw = -PdV, and this calculus accounts for work in continuously through intervals.
- Thu Jan 18, 2018 10:35 am
- Forum: Phase Changes & Related Calculations
- Topic: Question about Problem 8.41
- Replies: 5
- Views: 621
Re: Question about Problem 8.41
Yes, in thermodynamics we must remember that energy is conserved and that qsys + qsurr = 0, and thus qsys = -qsurr; the system being the ice and the surroundings being the water.
- Thu Jan 18, 2018 10:32 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: 8.55
- Replies: 2
- Views: 256
Re: 8.55
Remember that the enthalpy of a naturally occurring element (such as O2 gas) is always 0. So I believe changing the coefficient of O2 would not affect the enthalpy of the reaction.
- Wed Jan 10, 2018 4:47 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Bond Enthalpies
- Replies: 5
- Views: 498
Re: Bond Enthalpies
That's correct! ΔH RXN is equal to Energy required to break bonds (positive values) minus energy required to form bonds (or using addition and making sure to include that the values are negative.) The example in class was C=C (+612 kJ/mol), H-Br (+366 kJ/mol) -> C-C (-348 kJ/mol), C-H (-412 kJ/mol),...
- Wed Jan 10, 2018 4:39 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: 8.55 typo?
- Replies: 2
- Views: 126
Re: 8.55 typo?
In order to get the desired reaction, you have to choose and manipulate the two given reactions. In doing so, you would have to first choose Reaction 1, reverse it, and multiply the coefficients by 3/2 (make sure to change the value for enthalpy too). Then with Reaction 2, I believe we need it to ma...
- Wed Jan 10, 2018 4:07 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Heat capacity of calorimeters
- Replies: 1
- Views: 183
Re: Heat capacity of calorimeters
Choosing what to include in heat capacity depends on what is being asked/given. The heat capacity of just the calorimeter is different from the heat capacity of the entire calorimeter system (calorimeter and water). The heat capacity of the entire system (C) is the sum of the heat capacities of the ...
- Mon Dec 04, 2017 2:20 pm
- Forum: Polyprotic Acids & Bases
- Topic: Section 12.14
- Replies: 2
- Views: 696
Re: Section 12.14
I think it's a good thing to know how to identify polyprotic acids and maybe give the section a quick read, but I don't believe it'll be necessary to spend too much time focusing on the pH of polyprotic acids, which is why he omitted the homework problems on that section.
- Mon Dec 04, 2017 2:17 pm
- Forum: Sigma & Pi Bonds
- Topic: Delocalization
- Replies: 3
- Views: 457
Re: Delocalization
Identifying resonance in a structure is a way to find delocalized pi bonds in a molecule. In resonance structures, electrons are able to move to stabilize the molecule -> this movement is delocalization.
- Mon Nov 27, 2017 2:23 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Polar vs Nonpolar [ENDORSED]
- Replies: 2
- Views: 282
Re: Polar vs Nonpolar [ENDORSED]
Using what we know about Lewis Structures and VSEPR models, you first have to draw out the molecule with its atoms and lone pairs. If there is no symmetry and atoms' dipoles (as a result of electronegativity values of atoms) do not cancel out, then the molecule is most likely polar (like H 2 O). If ...
- Mon Nov 27, 2017 2:09 pm
- Forum: Hybridization
- Topic: Numbers in front of hybrid orbitals [ENDORSED]
- Replies: 2
- Views: 537
Re: Numbers in front of hybrid orbitals [ENDORSED]
When asked to just name the hybridization orbital, you would, for example, write sp3. However, when discussing the hybridization bonding model, you would refer to an atom's specific hybrid orbital (for example: 2sp3) overlapping with another orbital.
- Mon Nov 20, 2017 2:20 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 11.11 Part b
- Replies: 2
- Views: 1136
Re: 11.11 Part b
Knowing that the volume of the containers are the same, we only have to look at the amount of O 2 in each container. Our products and reactants are the same in both containers, and only the amount (moles) of O 3 changes from .10 to .50 -> therefore, O 2 will also have more moles in container 2 than ...
Re: Q. 37C
We know that ethylenediamine is bidentate because it has 2 atoms that would coordinate to Pt in this case. ethylenediamine, C2H4(NH2)2, uses both its NH2 atoms to bond with the metal atom
- Wed Nov 15, 2017 9:52 am
- Forum: Hybridization
- Topic: Coefficient of Hybridization? [ENDORSED]
- Replies: 2
- Views: 629
Coefficient of Hybridization? [ENDORSED]
I think this is a matter of notation but when asked the hybridization of the molecule, do we have to write the coefficient, notating quantum # n, with it or does it matter?
E.g. Ammonia, NH3: "sp3" or "2sp3"?
E.g. Ammonia, NH3: "sp3" or "2sp3"?
- Wed Nov 15, 2017 9:43 am
- Forum: Hybridization
- Topic: Does hybridization only occur when bonding?
- Replies: 3
- Views: 318
Re: Does hybridization only occur when bonding?
Hybridization of orbitals requires a "higher state of energy" of an atom (like the Carbon example Prof. Lavelle used in lecture for CH 4 ) and thus only occurs when it is involved with bonding. Really I believe it is to be considered as a model to describe bonding and explain observed stru...
- Mon Nov 06, 2017 2:56 pm
- Forum: Octet Exceptions
- Topic: When to expand an octet
- Replies: 2
- Views: 849
Re: When to expand an octet
If I am understanding your question correctly, in looking at BrO + , we're split between choosing a double bond, Br and O with two lone pairs vs. a triple bond where Br has two lone pairs and O has one? Because we can draw the structure of :Br: = :O:, with a double bond and two lone pairs on each at...
- Mon Nov 06, 2017 2:37 pm
- Forum: Lewis Structures
- Topic: Lone Pair Placement
- Replies: 2
- Views: 342
Re: Lone Pair Placement
The midterm covers up to Chapter 3, which is Lewis structures; this means that you won't need to apply the specific molecular shapes. I also believe we won't need to apply certain placement of lone pair electrons because the VSEPR model (where we minimize e- repulsion) is in Chapter 4 and Prof. Lave...
- Tue Oct 31, 2017 3:15 pm
- Forum: Resonance Structures
- Topic: 3.59
- Replies: 2
- Views: 385
Re: 3.59
Prof. Lavelle said the correct answer (of Octet O and lone Cl) is based off molecular orbital arguments just outside the scope of this course (everything plus what was said above^). A Lewis structure connecting Cl and O with a single bond, giving Cl the octet and O the single lone electron would res...
- Tue Oct 31, 2017 2:59 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Anion vs Cation electron configuration
- Replies: 2
- Views: 1609
Re: Anion vs Cation electron configuration
Yes, you will basically write the electron configuration the same way as a neutral ground-state atom. You must still consider Aufbau's Principle, Hund's Rule, and the Pauli Exclusion Principle. You will add to the outermost orbital, then to the next higher orbital.
- Thu Oct 26, 2017 9:29 am
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: s- electrons vs p- electrons [ENDORSED]
- Replies: 7
- Views: 1660
Re: s- electrons vs p- electrons [ENDORSED]
In many-electron atoms, electron-electron repulsion causes increasing orbitals to be increasing in energy (because electrons in "greater" orbitals are shielded from the full attraction of the nucleus & we know that when electrons are more strongly attracted to the nucleus, they are low...
- Thu Oct 26, 2017 9:23 am
- Forum: Quantum Numbers and The H-Atom
- Topic: P-Orbitals (x,y,z) [ENDORSED]
- Replies: 3
- Views: 4212
Re: P-Orbitals (x,y,z) [ENDORSED]
P x , P y , and P z just specify the different locations/orientation of electrons in a P-orbital (Whether an electron lies on the x-/y-/z-axis on the 3D Cartesian graph). I believe that Prof. Lavelle said this concept is only to help our understanding of these different orbitals, so when writing the...
- Tue Oct 17, 2017 11:01 pm
- Forum: Properties of Light
- Topic: Oscillation of Light
- Replies: 3
- Views: 353
Re: Oscillation of Light
If I am interpreting your question correctly: EMR is able to oscillate through empty space because EM waves don't need a medium to propagate itself. If we were to imagine a separated electromagnetic field - the electric field generates a magnetic field at a different angle and vice versa. In short, ...
- Tue Oct 17, 2017 10:48 pm
- Forum: DeBroglie Equation
- Topic: Detecting wavelength and observing wavelike characteristics
- Replies: 1
- Views: 348
Re: Detecting wavelength and observing wavelike characteristics
Looking at my notes from one of the lectures, I remember Prof. Lavelle saying that anything ≤ 10 -15 m is too small to detect. In the examples he used, a classical object had something of a wavelength of 1.64x10 -34 m, which is way too small. While for example, an electron at 5.3x10 6 m/s would resu...
- Mon Oct 09, 2017 6:53 pm
- Forum: Properties of Light
- Topic: Chapter 1 #3 c
- Replies: 1
- Views: 270
Re: Chapter 1 #3 c
When talking about Electromagnetic radiation, you are correct that as frequency decreases, the wavelength must increase due to their inverse relationship. When we look at how the electric and magnetic fields oscillate as light goes through space with a decreased frequency, the field has less energy ...
- Mon Oct 09, 2017 5:59 pm
- Forum: Photoelectric Effect
- Topic: Results of Photoelectric experiments
- Replies: 3
- Views: 458
Re: Results of Photoelectric experiments
I believe that it would be from the wave model to the particle model. The textbook notes that the results of some experiments (Photoelectric effect) compelled scientists to view that electromagnetic radiation is particlelike.
- Fri Oct 06, 2017 9:38 pm
- Forum: Balancing Chemical Reactions
- Topic: What’s the quickest way to approaching writing a balanced equation with only one given compound?
- Replies: 3
- Views: 443
Re: What’s the quickest way to approaching writing a balanced equation with only one given compound?
Usually in these cases, the mass of the two products will be given, as well as the mass of the unknown compound. Normally this will be a combustion question. In combustion, you have O 2 reacting with the compound to produce Carbon Dioxide and Water vapor. For example, if you have the oxidation: C x ...
- Mon Oct 02, 2017 10:16 pm
- Forum: Empirical & Molecular Formulas
- Topic: Problem F21
- Replies: 2
- Views: 431
Re: Problem F21
In Problem F21, after you find all of the mmol values of the elements in didemnin-A, the smallest value is 0.0113 mmol of Nitrogen, so you would divide all values by 0.0113, leaving you with 8.18 C : 13.0 H : 1.00 N : 2.00 O. Note that this isn't an incorrect ratio, but you still have to multiply ea...