CHEMISTRY COMMUNITY

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During lecture, professor Lavelle mentioned another way to name isopropyl-cyclopentane (pg. 96): methyl ethyl cyclopentane.

I'm confused as to why it's methyl ethyl instead of ethyl methyl, since I would assume that 'e' comes before 'm' (alphabetically).

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I'm still having a hard time understanding the difference between neo- and tert- substituents... can someone help explain? thank you!

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804748473 wrote:Could someone outline the information we need to know about catalysts because I could not find it in the course reader

page 84 also has a little bit of information on catalysts and free energy (activated complex theory).

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But if someone could clarify the second part of the question, it'd be great.

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I read through the chem community answers and understand now-- sorry for a redundant post and thanks.

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Hi, Do we include Pt(s) as an electrode conductor when both substances are of the same phase (ions or aqueous) (pg 5 crs reader)? I saw another problem in the textbook where Pt(s) is included when one is in its gaseous phase and another in aqueous (q 14.13 c). When exactly do we use Pt(s) as an elec...

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Thanks for the clarification!

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I was reviewing the examples on the course reader, and saw that on page 7, the F constant is listed as =96485C/mol e-. I just wanted to double check that this should be 96,4853 C/mol instead? The answer comes out differently when I substitute F with the value listed on the laminated formula sheet, i...

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OH I think I understand now! Thanks a lot for the analogy. If I understood correctly, in a sense, both the energy and entropy here, are referring to those within a system (where in your example, the system=golf balls)? So when a molecule has high energy, it is able to hold its atoms in place, which ...

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Pg. 30 and a few pages after that serves to explain that delta S (change in entropy) = (q/T) = (-w/T), where w = nRTln(V2-V1). In other words, there is a relationship between entropy (micro state) and volume (bulk property). Likewise, the "example of a link b/w accessible states and macroscopic...

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Hi, During lecture, Dr. Lavelle said that entropy is in its maximum and energy in minimum, in a state of equilibrium. Could someone explain how this works? I thought it would be reasonable to think that energy and entropy is proportional (i.e. more energy input creates more entropy due to greater nu...

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Hi,
I was just wondering, if we are able to calculate/predict for a state function by it's final and initial state, is there a way to calculate for other non-state, path functions? Or is it too probabilistic(?)?

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Practically, I also try to think of the concept in this way: Reversible process: If there is a syringe and you block the open tip of the syringe (so the air is trapped) and try to push in the plunger, then the force will induce a small change, but when you let it go, it'll rise back (be reversed). I...

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Thanks for your answer! Definitely helped clarify. Just to double check then, for the example on page 7, the system is the reactants (aqueous HCl and NaOH), and the surrounding is the water? And we calculated the amount of heat released from the system by calculating the amount of heat that the surr...

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Hi,
On the course reader (pg. 7), Dr. Lavelle wrote "perfect system" next to heat q(sys)+ q(surr) =0
Does this apply only to closed systems? Is the "perfect system" referring to closed systems?
Thanks.

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What is the difference between consumption and decomposition of reactions? when do we use consumption instead of decomposition, and does the choice affect the way of calculating the total reaction order?

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do ions not contribute to reaction orders? If so, why not?

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do we need to memorize the value for the midterm? or will only the ones on the worksheet be tested?

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Why is P(change in Volume) zero for aqueous solutions, solids and some gases for (change in U) = (change in H) - P(change in V)?

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Enthalpy is the amount of heat released or absorbed at a constant pressure. My question is: What exactly is the conceptual difference between bond enthalpy and enthalpy change? I know that each are different method that can be used to calculate the enthalpy of a reaction, but I'm uncertain as to whe...

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How do we know that BrOH is a weak acid?

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Attached is a video covering the basic concepts of Equilibrium with examples that illustrate each concept. Made by Angela He and Jane Park, Chem 14a

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Why to orbitals in sigma-bond have more overlap than orbitals in pi-bond? Is it because it's located along the bond axis?

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What does it mean when the bond order is 1/2 or 0?
Does the bond order of 0 just mean that the molecule is very unstable and will react very easily?

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There are p and s characters. The bond angle increases as s-character increases and decreases as p-character increases. So sp hybridization's bond angle would be higher than that of sp(x) hybridization (since s-character has more 'presence' in sp than in sp(x))

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Why does the equation E=-(h*R)/n^2 have a negative sign to it, when it's derived from E=hR*[(1/ n(final)^2 - 1/n(initial)^2], where neither h nor R are negative?

Is it negative only when the quantum number (n) is going from a higher number to a lower number (i.e. when energy is emitted)?

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I don't think you should be getting negative frequencies, since the definition of frequency in the context of chemistry (#of waves per second, also measured in Hz) won't make sense if it is negative. I.e., you can't have a negative number of wave per given time. However, the ENERGY TRANSITION can be...

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Just to recap the experiment, the observations from the experiment showed that 1. no electrons were ejected unless radiation has frequency above a certain threshold value characteristic of the metal 2. electrons were ejected immediately, however low the intensity of the radiation 3. kinetic energy o...

CHEMISTRY COMMUNITY

Search found 28 matches

lecture pg 96 methyl ethyl

Re: Naming with iso- and neo-

Re: Catalyst

Re: Pt(s) when to include in galvanic cell diagram

Re: Pt(s) when to include in galvanic cell diagram

Pt(s) when to include in galvanic cell diagram

Re: Course reader example pg. 7 electrochemistry

Course reader example pg. 7 electrochemistry

Re: Energy and entropy in equilibrium

Re: Microstates and macroscopic property

Energy and entropy in equilibrium

State functions and Path functions, and predictability

Re: Reversible vs. Irreversible Reactions

Re: heat q(sys)+ q(surr) =0

heat q(sys)+ q(surr) =0

difference between consumption and decomposition

ions and reaction orders

Re: quiz 1 prep winter 2012 5.

Internal energy and state property

Bond enthalpy and Enthalpy change

Re: 12.49 Stronger Base

Video: Equilibrium concepts and examples

orbitals in sigma-bond overlap

Bond order of 1/2 and 0

Re: Ch. 4 #43

Rydberg Equation concept

Re: Negative Frequency with the Rydberg Equation

Re: Question: Wave Model vs. Photon Model of Light