Search found 30 matches
- Fri Mar 16, 2018 1:39 pm
- Forum: *Enzyme Kinetics
- Topic: Question 15.85
- Replies: 4
- Views: 973
Re: Question 15.85
How do we determine the molecularity given the rate laws? You can look at the number of reactants in the chemical equation to determine the molecularity of the rate laws. If there is only one reactant=unimolecular two reactants=bimolecular three reactants=termolecular (highly unlikely in real life ...
- Fri Mar 16, 2018 1:27 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Steady-State Approximation vs. Pre-equilibrium Condition
- Replies: 4
- Views: 787
Re: Steady-State Approximation vs. Pre-equilibrium Condition
Yes. Dr. Lavelle said that it would be way too much work to use the steady-state and so we wouldn't be using this method for this class.
Just focus on the pre-equilibrium condition!
Just focus on the pre-equilibrium condition!
- Fri Mar 16, 2018 1:25 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: HW #15.85 b
- Replies: 1
- Views: 238
HW #15.85 b
Could someone explain in detail 15.85b?
#85b what does it mean that the role of the Ar is to remove energy as the product forms?
Ar doesn't appear in the chemical equation but we still have to count it in the overall molecularity?
#85b what does it mean that the role of the Ar is to remove energy as the product forms?
Ar doesn't appear in the chemical equation but we still have to count it in the overall molecularity?
- Fri Mar 16, 2018 1:19 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Identifying a catalyst in a reaction
- Replies: 4
- Views: 13376
Re: Identifying a catalyst in a reaction
Yes, intermediates will always appear as the products first and then used up as a reactant in the following step. However, catalysts will always appear on the reactant side first. Catalysts are not consumed!
- Fri Mar 16, 2018 1:15 pm
- Forum: *Enzyme Kinetics
- Topic: Final-Collision Theory
- Replies: 3
- Views: 938
Final-Collision Theory
I understand that we need to know the overall relationship between reactions, temperature, kinetic energy, and activation energy in the collision theory. Do we also need to know the collision frequency, mean relative speed equations, and steric factors as well?
- Fri Mar 16, 2018 1:10 pm
- Forum: First Order Reactions
- Topic: HW #15.37c
- Replies: 2
- Views: 477
HW #15.37c
When we use the integrated first order rate law for this particular problem, why is it not necessary to convert the mass given to concentrations in molarity? It says that the "knowledge of the volume is not required" in the solutions manual.
- Thu Mar 08, 2018 11:31 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: HW 15.19a
- Replies: 3
- Views: 638
HW 15.19a
Can someone explain how to get the order of [B]?
I got exact numbers for [A] and [C] but I keep getting decimal points for [B].
I got exact numbers for [A] and [C] but I keep getting decimal points for [B].
- Thu Mar 01, 2018 12:56 am
- Forum: General Rate Laws
- Topic: Using more than one species [ENDORSED]
- Replies: 1
- Views: 288
Using more than one species [ENDORSED]
How do we know when and when not to use more than one species' concentration?
- Thu Mar 01, 2018 12:55 am
- Forum: First Order Reactions
- Topic: Pseudo-First Order Reaction [ENDORSED]
- Replies: 4
- Views: 595
Pseudo-First Order Reaction [ENDORSED]
What is pseudo-first order reaction and how is that related to the second-order reaction?
- Thu Mar 01, 2018 12:54 am
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Overall order
- Replies: 4
- Views: 799
Overall order
what is the significance of the overall order?
- Thu Feb 22, 2018 8:36 pm
- Forum: Balancing Redox Reactions
- Topic: Does order matter?
- Replies: 7
- Views: 942
Re: Does order matter?
No, I think as long as you have a balance equation with all the H+, e-, and H20 on the right side (reactant or product) with the arrow pointing in the right direction (reduction/oxidation) you will be fine.
- Thu Feb 22, 2018 5:58 pm
- Forum: Balancing Redox Reactions
- Topic: Half Reaction Order
- Replies: 9
- Views: 2894
Half Reaction Order
Does the order matter when we are writing the half reactions as long as we are able to cancel the number of electrons correctly?
If we are writing an oxidation half reaction, does it have to be Zn+ arrow Zn2+ + e-? or can we write it as Zn2+ + e- arrow Zn+ ?
If we are writing an oxidation half reaction, does it have to be Zn+ arrow Zn2+ + e-? or can we write it as Zn2+ + e- arrow Zn+ ?
- Thu Feb 22, 2018 3:45 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 14.11d
- Replies: 1
- Views: 302
14.11d
For the anode reaction, O2 being oxidized to H+, do we ignore the H+ and balance it with 2H2O or do we balance the reaction by adding H+ on the O2 side?
- Thu Feb 22, 2018 1:16 pm
- Forum: Balancing Redox Reactions
- Topic: Balancing H+
- Replies: 4
- Views: 511
Re: Balancing H+
So balancing the number of H with H+ or H3O+ is both considered correct? If I balance H with H30+ I have to go back and balance the other side's number of O again...
- Thu Feb 22, 2018 11:58 am
- Forum: Balancing Redox Reactions
- Topic: Balancing H+
- Replies: 4
- Views: 511
Balancing H+
Our textbook and the Redox Instruction on the web posted by Dr. Lavelle tells us to just add H+ to balance the number of H on the other side, but our TA said it would be wrong to do so. The correct way to balance H is to add H30+ so which way are we supposed to balance the H? H30+ is making it confu...
- Mon Feb 12, 2018 8:43 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Section 11.11
- Replies: 1
- Views: 271
Section 11.11
Equilibrium constant is unchanged when concentrations or pressure change, but it changes with temperature. Why is that?
- Mon Feb 12, 2018 8:42 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Vibrational Energy State
- Replies: 4
- Views: 558
Re: Vibrational Energy State
Entropy is the amount of disorder in the universe and the more complex and higher the mass (heavier), it is going to create much more vibrational energy which adds more disorder.
- Mon Feb 12, 2018 8:39 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Gibbs free
- Replies: 5
- Views: 606
Re: Gibbs free
What is the difference between Gibbs free energy of reaction and Standard Gibbs free energy of reaction?
- Mon Feb 12, 2018 8:38 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Example 9.8
- Replies: 2
- Views: 371
Example 9.8
How do we know that it is 4^N and not 4^4?
- Mon Feb 12, 2018 8:37 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Residual Entropy
- Replies: 1
- Views: 288
Residual Entropy
Could someone explain what exactly the residual entropy means?
- Mon Feb 12, 2018 8:36 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: entropy sign
- Replies: 5
- Views: 745
Re: entropy sign
Do we have to indicate the signs of entropy?
- Mon Feb 12, 2018 8:34 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Spontaneous Change
- Replies: 1
- Views: 244
Spontaneous Change
How can spontaneous change not even occur at all? (from section 9.1)
- Mon Feb 12, 2018 8:33 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: delta S(system) vs delta S(surroundings)
- Replies: 4
- Views: 15516
Re: delta S(system) vs delta S(surroundings)
You can always assume that delta S(system)= -delta S(surrounding) for a reversible expansion at equilibrium because the heat that flows to the surrounding is being released by the system.
- Mon Feb 12, 2018 8:28 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: entropy
- Replies: 4
- Views: 589
Re: entropy
I think that is the definition of a reversible deltaStot. For a it to be considered a reversible reaction, entropy of the system must be exactly the opposite of the surrounding and vice versa.
- Sun Jan 21, 2018 9:05 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Week 3 Test Topic is endorsed
- Replies: 37
- Views: 4951
Re: Week 3 Test Topic is endorsed
If you look at the outline for chapter 8, it says that born-haber is not included!
- Wed Jan 17, 2018 7:48 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Self-Test 8.5B
- Replies: 3
- Views: 394
Self-Test 8.5B
A system was heated by using 300.J of heat, yet it was found that its internal energy decreased by 150. J Calculate w. Was work done on the system, or did the system do work?
How do you tell that 300. J is a negative? Is it because it produced heat?
How do you tell that 300. J is a negative? Is it because it produced heat?
- Wed Jan 17, 2018 7:44 pm
- Forum: Phase Changes & Related Calculations
- Topic: Heating Curves
- Replies: 1
- Views: 172
Heating Curves
Which substances might show characteristics of superheating and supercooling? If one substance were to have superheating characteristics, does that mean it will also have supercooling as well? Or are the characteristics independent of each other?
- Thu Jan 11, 2018 11:34 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: 8.3 Reversible Isothermal Expansion
- Replies: 3
- Views: 399
Re: 8.3 Reversible Isothermal Expansion
Yes. I think that in order to maintain reversible process during gas expansion, the external pressure has to match the pressure of the gas at every stage of the expansion and reach the maximum work since even an infinitely small change makes it reversible.
- Thu Jan 11, 2018 11:28 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Celsius the same as Kelvin? [ENDORSED]
- Replies: 9
- Views: 6580
Re: Celsius the same as Kelvin? [ENDORSED]
Just as the others above have mentioned, "per degree Celsius" and "per Kelvin" are the same since it is just dealing with delta T (change in temperature). So you wouldn't necessarily have to convert Celsius to Kelvin by adding 273.15. You can also note that it is the same when ca...
- Thu Jan 11, 2018 11:17 pm
- Forum: Calculating Work of Expansion
- Topic: Irreversible vs Reversible
- Replies: 2
- Views: 298
Irreversible vs Reversible
If reversible process is one that is reversed by an infinitely small change, how come an expansion against an external pressure that differs by finite amount from the pressure of the system be an irreversible one?