Search found 31 matches

by Noah Fox 1E
Tue Mar 12, 2019 11:08 pm
Forum: Ideal Gases
Topic: How do I know what is an Ideal Gas
Replies: 11
Views: 77

Re: How do I know what is an Ideal Gas

Note ideal gases are usually exemplified by noble gases ie helium argon etc. This is because the molecules are singular
by Noah Fox 1E
Tue Mar 12, 2019 11:06 pm
Forum: Gibbs Free Energy Concepts and Calculations
Topic: Spontaneous Reaction
Replies: 5
Views: 45

Re: Spontaneous Reaction

I don't think this is the way to answer the question but something that helps me conceptualize it is that heat diffuses out. If a sample of water is in a 10 degree Celsius space, heat leaves the sample and the bonds form spontaneously because of the conditions it is in.
by Noah Fox 1E
Tue Mar 12, 2019 11:04 pm
Forum: General Science Questions
Topic: Organic Molec Naming?
Replies: 2
Views: 26

Re: Organic Molec Naming?

I don't think it is on the course outline either so I think we're in the clear
by Noah Fox 1E
Tue Mar 12, 2019 10:54 pm
Forum: Arrhenius Equation, Activation Energies, Catalysts
Topic: catalyst and equilibrium constant
Replies: 2
Views: 20

Re: catalyst and equilibrium constant

Don't we also have to keep the catalysts saturated with reactants? Or am I misrembering it.
by Noah Fox 1E
Tue Mar 12, 2019 10:53 pm
Forum: Administrative Questions and Class Announcements
Topic: Sig Figs
Replies: 9
Views: 41

Re: Sig Figs

They definitely did check sig figs on the midterm
by Noah Fox 1E
Tue Mar 12, 2019 10:52 pm
Forum: Reaction Mechanisms, Reaction Profiles
Topic: Intermediates
Replies: 2
Views: 14

Re: Intermediates

You have the general idea down. Note that reactions with intermediates are elementary steps and when added up completely it should produce the final reaction
by Noah Fox 1E
Tue Mar 12, 2019 10:49 pm
Forum: Reaction Mechanisms, Reaction Profiles
Topic: fast equilibrium approach v steady state equilibrium
Replies: 1
Views: 17

Re: fast equilibrium approach v steady state equilibrium

Honestly, steady-state is so math intensive and so time consuming that it is most likely best to avoid it at all circumstances.
by Noah Fox 1E
Tue Mar 12, 2019 10:47 pm
Forum: Reaction Mechanisms, Reaction Profiles
Topic: organic chem stuff
Replies: 1
Views: 20

Re: organic chem stuff

I would think if it isn't included in the outline that it wouldn't be included in the test
by Noah Fox 1E
Tue Mar 12, 2019 10:46 pm
Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
Topic: Nernst
Replies: 14
Views: 65

Re: Nernst

Yes, it is the amount of electrons released in a balanced galvanic reaction
by Noah Fox 1E
Tue Mar 12, 2019 10:44 pm
Forum: Gibbs Free Energy Concepts and Calculations
Topic: Ice melting
Replies: 4
Views: 32

Re: Ice melting

The melting of ice is spontaneous because its something that occurs naturally (in the right temperature). The way I like to think about it is that in an area with high heat the ice cube (devoid of heat) will naturally see energy diffuse into the ice breaking the bonds at the same time. The combustio...
by Noah Fox 1E
Tue Mar 12, 2019 10:41 pm
Forum: Balancing Redox Reactions
Topic: Coefficients
Replies: 3
Views: 17

Re: Coefficients

So that means oxidation number is extensive or intensive? Or would it be neither
by Noah Fox 1E
Tue Mar 12, 2019 10:39 pm
Forum: Reaction Mechanisms, Reaction Profiles
Topic: Pre-equilibrium vs. steady-state
Replies: 4
Views: 21

Re: Pre-equilibrium vs. steady-state

I would avoid steady-state even as a sanity check primarily because it's long math intensive and time consuming.
by Noah Fox 1E
Tue Mar 12, 2019 10:38 pm
Forum: Zero Order Reactions
Topic: Reaction Rate
Replies: 10
Views: 41

Re: Reaction Rate

Wait, I thought initial concentration would be included especially for second order reactions
by Noah Fox 1E
Tue Mar 12, 2019 10:35 pm
Forum: Reaction Mechanisms, Reaction Profiles
Topic: Reaction mechanisms- elementary steps
Replies: 1
Views: 7

Re: Reaction mechanisms- elementary steps

I think so, because the slow reaction is rate defining. Much in the same way if the second elementary step is slow here is a bottle neck in the first elementary step which has to be fast and the fast step has a reversible reaction
by Noah Fox 1E
Tue Mar 12, 2019 10:33 pm
Forum: Administrative Questions and Class Announcements
Topic: Sig Figs
Replies: 9
Views: 41

Re: Sig Figs

I would assume so, but I can't confirm. I also have concerns about how sig figs are graded. They seem to mark you down on sig figs if you so much as have another decimal place beyond the sigfigs in the work.
by Noah Fox 1E
Tue Mar 12, 2019 10:27 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: Boltzmann Equation
Replies: 3
Views: 24

Re: Boltzmann Equation

A usual tip off to use the boltzman's equation is that they talk about micro states or state spaces. The midterm problem described the state spaces of nanoparticles.
by Noah Fox 1E
Wed Feb 06, 2019 11:05 am
Forum: Calculating Work of Expansion
Topic: Isothermal Expansions
Replies: 3
Views: 36

Re: Isothermal Expansions

isothermal refers to the fact that the system will have the same amount of heat no matter what process occurs. This may mean work takes the form of heat. reversible and irreversible are terms relating to the way pressure is exerted on a system
by Noah Fox 1E
Wed Feb 06, 2019 11:03 am
Forum: Thermodynamic Systems (Open, Closed, Isolated)
Topic: Midterm [ENDORSED]
Replies: 48
Views: 643

Re: Midterm [ENDORSED]

Some UA's and LA's provide worksheets for more practice problems. These sometimes come with walkthroughs. Linden's reviews are usually pretty good.
by Noah Fox 1E
Wed Feb 06, 2019 11:02 am
Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
Topic: Irreversible/Reversible Processes
Replies: 3
Views: 29

Re: Irreversible/Reversible Processes

Isothermal reversible reactions produce more work because it is done slowly and done with tiny steps and allows the system to come back to equilibrium. Irreversible processes in comparison is one massive push that doesn't achieve the same amount of work because it is less efficient.
by Noah Fox 1E
Mon Jan 28, 2019 2:07 pm
Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
Topic: Extensive vs intensive
Replies: 2
Views: 25

Re: Extensive vs intensive

Extensive properties are things that are not universal properties and are sample dependent. This can include weight and temperature, where as intensive properties are properties that pertain to all samples of an object such as the number of protons in an element.
by Noah Fox 1E
Mon Jan 28, 2019 2:05 pm
Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
Topic: Q and H
Replies: 2
Views: 34

Re: Q and H

H is a state function which means that whichever way it goes there is always a net change and takes into account the whole reaction, where as q is the change of heat and may be dependent on the reaction itself as well as the possibility of incomplete reactions (I think)
by Noah Fox 1E
Sun Jan 27, 2019 10:28 am
Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
Topic: energy production
Replies: 4
Views: 64

Re: energy production

The breaking of bonds between glucose creates an exothermic reaction which subsequently powers the process of cellular respiration an endothermic process. Cellular respiration produces ATP which dissociates into ADP and P(inorganic) and produces a muscle contraction within the heart.
by Noah Fox 1E
Sat Jan 26, 2019 3:15 pm
Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
Topic: H and Q
Replies: 4
Views: 41

Re: H and Q

In Enthalpy delta H is a state function of the holistic change in energy configuration, where as q is the heat flow either into or out of the reaction as a result of the change in delta H Sources: https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_M...
by Noah Fox 1E
Sat Jan 26, 2019 3:12 pm
Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
Topic: Standard enthalpy of formation
Replies: 2
Views: 38

Re: Standard enthalpy of formation

Standard enthalpy of formation is the change of enthalpy when only one mole of that molecule is formed by its constituent elements ie elements found in their natural forms such as H2 and N2. Standard reaction enthalpy is the change in enthalpy that occurs in a system when matter is transformed by a ...
by Noah Fox 1E
Sat Jan 26, 2019 3:06 pm
Forum: Phase Changes & Related Calculations
Topic: Sublimation
Replies: 6
Views: 83

Re: Sublimation

I suppose it would be able to bypass the step of turning into a liquid because of incredibly strong intermolecular forces, however I do not know if this would create solid materials or incredibly viscous non-newtonian-like fluids
by Noah Fox 1E
Mon Jan 14, 2019 10:22 am
Forum: Equilibrium Constants & Calculating Concentrations
Topic: Concentration Affecting K
Replies: 7
Views: 67

Re: Concentration Affecting K

Adding more concentration of reactants or products will not change Kc. This is because Kc focuses on the rates of the reaction rather than the equality of the concentrates. The reaction will naturally begin to move back to its state of equilibrium but with increased values on both sides.
by Noah Fox 1E
Mon Jan 14, 2019 10:19 am
Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
Topic: Exothermic Reaction
Replies: 3
Views: 38

Re: Exothermic Reaction

An exothermic reaction shifts toward the formation of products because the products are at a lower energy level than the reactants. The universe naturally wants to gravitate to the lowest energy level and the most chaos through entropy. Because of this the decomposition of a complex (high energy) mo...
by Noah Fox 1E
Mon Jan 14, 2019 10:15 am
Forum: Equilibrium Constants & Calculating Concentrations
Topic: Example from lecture on Wednesday
Replies: 2
Views: 34

Re: Example from lecture on Wednesday

In the problem he gave us the given reaction of ATP hydrolysis of ATP + H2O --> ADP + P(inorganic) The initial concentrations were based on real numbers from both healthy and dead tissues. The equilibrium point isn't necesarilly an equilibrium point more as the end point of the reaction as the last ...
by Noah Fox 1E
Thu Jan 10, 2019 3:41 pm
Forum: Ideal Gases
Topic: Equilibrium Constant and Reaction Quotient
Replies: 3
Views: 28

Re: Equilibrium Constant and Reaction Quotient

The reaction quotient is the ratio of products and reactants with their stoichiometric counterparts of an equilibrium reaction at ANY point. Equilibrium constants however is this ratio at equilibrium. Q and K are both calculated the same exact way but at (possibly) different points of the equilibriu...
by Noah Fox 1E
Thu Jan 10, 2019 3:38 pm
Forum: Ideal Gases
Topic: Reaction Quotient
Replies: 6
Views: 46

Re: Reaction Quotient

Because they do not affect the concentrations of reactants and products, liquids are not taken into account for equilibrium reactions. That being said H2O undergoes a acid base reaction with itself when it produces hydrogen ions and hydroxide ions spontaneously, but it goes disregarded because water...
by Noah Fox 1E
Thu Jan 10, 2019 3:35 pm
Forum: Non-Equilibrium Conditions & The Reaction Quotient
Topic: Solid and Liquids in reaction equilibrium situations
Replies: 1
Views: 65

Solid and Liquids in reaction equilibrium situations

Water has a dynamic of producing hydroxide and hydronium ions forming H3O+ and OH-, which then can react to form H2O. Are there any examples of solids doing anything akin to this?

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