Search found 30 matches
- Tue Mar 13, 2018 10:58 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: 15.63
- Replies: 6
- Views: 668
Re: 15.63
I had the same question, I'm wondering how they were able to derive that from the arrhenius equation
- Tue Mar 13, 2018 9:28 pm
- Forum: First Order Reactions
- Topic: The integrated rate laws
- Replies: 3
- Views: 572
Re: The integrated rate laws
Just use the integrated rate laws that he gives on the equation sheet!
- Tue Mar 13, 2018 9:27 pm
- Forum: Zero Order Reactions
- Topic: Applications
- Replies: 2
- Views: 542
Re: Applications
For zero order, that just means that the concentration of that reactant does not affect the rate of the reaction. That can be seen in the problems where you compare the concentrations and rate constants of different reactions to find their orders; if it is zero order, then changing the concentration...
- Tue Mar 13, 2018 9:25 pm
- Forum: First Order Reactions
- Topic: k' in Pseudo-First-Order Rate Laws
- Replies: 4
- Views: 1509
Re: k' in Pseudo-First-Order Rate Laws
Yes, k prime if the reverse reaction's rate constant. You can use that and the forward reaction's k to figure out the equilibrium constant, K.
- Tue Mar 06, 2018 8:47 pm
- Forum: General Rate Laws
- Topic: Proper units
- Replies: 7
- Views: 800
Re: Proper units
For problems 17 and 19, it is confusing to know which units to use, but you should probably keep it consistent with what they give you unless you need to convert (eg. seconds to hours).
- Tue Mar 06, 2018 8:44 pm
- Forum: General Rate Laws
- Topic: Coefficients
- Replies: 6
- Views: 935
Re: Coefficients
Coefficients do not determine the order of the reaction, they just matter when it says the concentration of the products vs reactants and you have to multiply by a coefficient to keep the rate consistent.
- Tue Mar 06, 2018 8:43 pm
- Forum: General Rate Laws
- Topic: Units in 15.17 vs. 15.19
- Replies: 2
- Views: 381
Re: Units in 15.17 vs. 15.19
I would just keep the units of the answer the same units that they give you, I know that sometimes they change the units interchangeably from minutes and seconds and as long as the answers are consistent with each other I believe its ok.
- Thu Mar 01, 2018 10:05 am
- Forum: General Rate Laws
- Topic: half life vs rate
- Replies: 2
- Views: 408
Re: half life vs rate
Like they said, a half life is the time it takes for half of the concentration of the specific reaction to deplete by 50%, and the rate is just how fast it depletes throughout the reaction.
- Thu Mar 01, 2018 10:04 am
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Graphs in Lecture
- Replies: 2
- Views: 415
Re: Graphs in Lecture
It depends which order you are talking about. For a first order reaction, the linear graph is the graph of ln[A] vs time, and the curved graph is just concentration vs time.
- Thu Mar 01, 2018 10:02 am
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Overall order
- Replies: 4
- Views: 761
Re: Overall order
You just add up each order of the reactants to find total order.
- Wed Feb 21, 2018 2:26 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Q & K?
- Replies: 4
- Views: 556
Re: Q & K?
In the problems that they are giving in the homework, they are treating Q as if it was K, and using that value to determine whether the reactants or products are favored. In other words, they usually will not give you a K value to compare it to.
- Wed Feb 21, 2018 2:25 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Nernst equation usage
- Replies: 3
- Views: 584
Re: Nernst equation usage
Yes, you use it under nonstandard conditions, such as a change in the molarities (not 1M like you said), a different temperature, pressure, etc.
- Wed Feb 21, 2018 2:23 pm
- Forum: Balancing Redox Reactions
- Topic: Defining Cathodes and Anodes through standard cell potential
- Replies: 2
- Views: 365
Re: Defining Cathodes and Anodes through standard cell potential
Yes you can do it like that, but not all the time. In an electrolytic cell, the potential is supposed to be negative; so, if you did it like you said, then you would mix them up because you are solving for the standard potential to be negative. It is a more safe bet to look at the overall reaction a...
- Wed Feb 21, 2018 2:21 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: calculating n
- Replies: 9
- Views: 1161
Re: calculating n
You can look at the overall reaction, and split it into 2 half reactions. For example, if one of the half reactions for the total equation is Cr3+ + 1e- -----> Cr2+, then here one electron is being transferred. However, if there are 2Cr3+ and Cr2+, then you know there are 2 electrons transferred bec...
- Wed Feb 21, 2018 2:18 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Gold ring example
- Replies: 1
- Views: 208
Re: Gold ring example
They just took the Hydrogen off of the NO3-, then Nitrogen is reduced from 5+ charge to 2+ charge in NO.
- Sun Feb 11, 2018 1:32 pm
- Forum: Environment, Fossil Fuels, Alternative Fuels
- Topic: fossil fuels on midterm [ENDORSED]
- Replies: 2
- Views: 1632
fossil fuels on midterm [ENDORSED]
What would be an example in this category that would be on the midterm?
- Sun Feb 11, 2018 1:29 pm
- Forum: Balancing Redox Reactions
- Topic: cat/anions
- Replies: 2
- Views: 387
cat/anions
Are the ions that flow from the cathode to the anode through the salt bridge cations or anions?
- Sun Feb 11, 2018 1:25 pm
- Forum: Phase Changes & Related Calculations
- Topic: Environmental impact?
- Replies: 6
- Views: 994
Re: Environmental impact?
I would assume that the question he would ask would have to do with a temperature raise in the atmosphere (like how we use q=-q) but I doubt it will be covered on the exam.
- Mon Jan 29, 2018 7:42 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Pressure and Volume on Spontaneity
- Replies: 2
- Views: 1248
Re: Pressure and Volume on Spontaneity
Yes, you have to take into account the different ways that you can solve for deltaS. Since deltaG is the spontaneity of a reaction, it depends on S so it also depends on pressure and volume.
- Mon Jan 29, 2018 7:39 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Gibbs Free Energy [ENDORSED]
- Replies: 6
- Views: 1283
Gibbs Free Energy [ENDORSED]
If deltaS is the disorder (for use of a better word) or a reaction, how is that different than delta G?
- Mon Jan 29, 2018 7:37 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Spontaneity of a reaction
- Replies: 2
- Views: 365
Re: Spontaneity of a reaction
I see what you're saying, and I think that it would be easier to just imagine what would make G negative (stated above). But for some of them, the reverse reaction will be the opposite sign of deltaG, changing whether or not it is spontaneous.
- Wed Jan 24, 2018 8:52 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Internal Energy and Enthalpy [ENDORSED]
- Replies: 2
- Views: 462
Re: Internal Energy and Enthalpy [ENDORSED]
Along with that, qp=delta H only if the pressure is constant. Therefore, having the work be 0 with a system with constant pressure would result in the only thing changing the internal energy of the system be the change in heat.
- Wed Jan 24, 2018 8:50 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Open System
- Replies: 16
- Views: 2184
Re: Open System
It also depends what kind of system you are trying to increase the q on; you cannot add or remove a substance from a closed system because matter cannot be transferred. However, for a closed system, you can do work on it or change the temperature.
- Wed Jan 24, 2018 8:49 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: q isn't a state function
- Replies: 3
- Views: 3448
Re: q isn't a state function
Q is not a state function because throughout a reaction, the heat changes; therefore, you cannot solve for q with qfinal-qinitial. With work, it is the same thing. The amount of work done on a system is not solved for just by the final and initial work.
- Tue Jan 16, 2018 7:24 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Pressure in enthalpy vs heat capacity
- Replies: 2
- Views: 239
Re: Pressure in enthalpy vs heat capacity
You always just use what they give you for enthalpies, but heat capacity is definitely more specific. So yes, it does depend on whether the pressure/volume is constant for heat capacity.
- Tue Jan 16, 2018 7:22 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Work function
- Replies: 4
- Views: 311
Re: Work function
I'm pretty sure it depends on whether work is being done by the system or on the system. I'm assuming if it was being done ON the system, it would be positive and vice versa.
- Tue Jan 16, 2018 7:19 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Calculating enthalpy using bond energies [ENDORSED]
- Replies: 2
- Views: 976
Re: Calculating enthalpy using bond energies [ENDORSED]
In the textbook, they are only taking into account which specific bonds were broken and produced from the reactants to products. When I do these problems, I tend to write out all of the bonds and multiply by the number of them (it's easier for me), but wither way is fine.
- Wed Jan 10, 2018 5:32 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: What is bond enthalpy and can someone explain to me what Lavelle was doing with the Lewis Structures in today's lecture?
- Replies: 3
- Views: 280
Re: What is bond enthalpy and can someone explain to me what Lavelle was doing with the Lewis Structures in today's lect
Bond enthalpy is the energy needed to break a bond. In today's lecture, Lavelle was essentially trying to show us which bonds are broken in the specific reaction, and how you use the enthalpies from both the reactants and products to find the total change in enthalpy. Since there were bonds broken a...
- Wed Jan 10, 2018 5:27 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Heating Curve: How is the kJ calculated?
- Replies: 2
- Views: 204
Re: Heating Curve: How is the kJ calculated?
Sometimes you have to convert the units given to you in order to do the calculation correctly. For example, the specific heat capacity and the heat of fusion have different units, so in order to get both of them to kJ, you have to cancel out the units in each equation to be converted to kJ.
- Wed Jan 10, 2018 5:25 pm
- Forum: Phase Changes & Related Calculations
- Topic: Exothermic Rxn
- Replies: 6
- Views: 669
Re: Exothermic Rxn
The meaning of an exothermic reaction means that it gives off energy once completed, not that the reactants need to be spontaneous in order to do so.