CHEMISTRY COMMUNITY

Noah Fox 1E

Note ideal gases are usually exemplified by noble gases ie helium argon etc. This is because the molecules are singular

Noah Fox 1E

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.

Noah Fox 1E

I don't think it is on the course outline either so I think we're in the clear

Noah Fox 1E

Don't we also have to keep the catalysts saturated with reactants? Or am I misrembering it.

Noah Fox 1E

They definitely did check sig figs on the midterm

Noah Fox 1E

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

Noah Fox 1E

Honestly, steady-state is so math intensive and so time consuming that it is most likely best to avoid it at all circumstances.

Noah Fox 1E

I would think if it isn't included in the outline that it wouldn't be included in the test

Noah Fox 1E

Yes, it is the amount of electrons released in a balanced galvanic reaction

Noah Fox 1E

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...

Noah Fox 1E

So that means oxidation number is extensive or intensive? Or would it be neither

Noah Fox 1E

I would avoid steady-state even as a sanity check primarily because it's long math intensive and time consuming.

Noah Fox 1E

Wait, I thought initial concentration would be included especially for second order reactions

Noah Fox 1E

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

Noah Fox 1E

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.

Noah Fox 1E

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.

Noah Fox 1E

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

Noah Fox 1E

Some UA's and LA's provide worksheets for more practice problems. These sometimes come with walkthroughs. Linden's reviews are usually pretty good.

Noah Fox 1E

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.

Noah Fox 1E

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.

Noah Fox 1E

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)

Noah Fox 1E

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.

Noah Fox 1E

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...

Noah Fox 1E

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 ...

Noah Fox 1E

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

Noah Fox 1E

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.

Noah Fox 1E

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...

Noah Fox 1E

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 ...

Noah Fox 1E

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...

Noah Fox 1E

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...

Noah Fox 1E

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?

CHEMISTRY COMMUNITY

Search found 31 matches

Re: How do I know what is an Ideal Gas

Re: Spontaneous Reaction

Re: Organic Molec Naming?

Re: catalyst and equilibrium constant

Re: Sig Figs

Re: Intermediates

Re: fast equilibrium approach v steady state equilibrium

Re: organic chem stuff

Re: Nernst

Re: Ice melting

Re: Coefficients

Re: Pre-equilibrium vs. steady-state

Re: Reaction Rate

Re: Reaction mechanisms- elementary steps

Re: Sig Figs

Re: Boltzmann Equation

Re: Isothermal Expansions

Re: Midterm [ENDORSED]

Re: Irreversible/Reversible Processes

Re: Extensive vs intensive

Re: Q and H

Re: energy production

Re: H and Q

Re: Standard enthalpy of formation

Re: Sublimation

Re: Concentration Affecting K

Re: Exothermic Reaction

Re: Example from lecture on Wednesday

Re: Equilibrium Constant and Reaction Quotient

Re: Reaction Quotient

Solid and Liquids in reaction equilibrium situations