CHEMISTRY COMMUNITY

DanielLee3H

Carbon monoxide has a double bond and lone pairs on the oxygen, but the oxygen pulls strongly on the carbon making the partial positive charge large. But wouldn't it also have a strong negative charge?

DanielLee3H

What does it mean conceptually that voltage difference does not depend on how many times the reaction occurs? I understand that standard cell potential is a state function, and that you don't multiply the cell potential by the coefficient but why? I figured that if the reaction goes on for longer, t...

DanielLee3H

This is what I think happens, please correct if I'm wrong. When you form bonds spontaneously, the bonds release energy that goes into the system and increases the thermal entropy at a magnitude greater than the decrease in residual entropy, for an overall increase in entropy. When an unstable bond b...

DanielLee3H

I'm still a little confused as to why entropy is at its maximum at equilibrium. I get that mathematically or like according to the laws this makes sense. But conceptually, don't certain reactions that combine two molecules together have less degeneracy even if its spontaneous. Doesn't that make entr...

DanielLee3H

Just to clarify, Steric strains are high in energy due to the instability caused by the physical presence of multiple atoms in a limited area, while torsional strains are caused by repulsion between electron dense clouds of hydrogens when eclipsed? Isn't that essentially the same thing?

DanielLee3H

What exactly does the curved arrow mean when it starts at a single bond and points to an atom or molecule? I get that the bond is breaking and forming around the new atom but does each atom bonded originally take one of the electrons (so does it like split down the middle?). Or do both electrons tha...

DanielLee3H

If the rate function doesn't match the overall reaction in terms of coefficients, you know that there have to be intermediate steps that don't show up in the overall reaction right? And the rate function is based on the slow intermediate step?

DanielLee3H

Oh oops. Thank you. Also, the method of initial rates and the integrated rate law are different ways to find the reaction constant. Do they just give you different ways of modeling the reaction rate? And you can use both to find any reaction rate, whether it is the slow step or the overall reaction?

DanielLee3H

How did we get from the general rate equation (-1/a)*d[A]/dt to the differential rate law k[R]^n?

DanielLee3H

I have no idea how to even approach these.

Do we have to just know the half reactions of these formulas or that you have to add KOH to the cell in part c?

DanielLee3H

Why does gibbs free energy not depend on internal energy, but rather just enthalpy. Basically, why does gibbs free energy not include the energy of work as part of its function?

DanielLee3H

Does isothermal always mean the system is isolated? And does that mean it's always going to be reversible? Because isothermal can also be in a irreversible reaction if number of moles is what is changing right? But in that case then pressure would be constant making it irreversible? So does Isotherm...

DanielLee3H

I thought cell potential decreased as the reaction takes place because of the anode consumption and electrons building up in the cathode part of the galvanic cell. But it says that cell potential is an intensive property and does not depend on how many times the reaction occurs, which is why we don'...

DanielLee3H

Why is a higher K, or more products than reactants, favorable? Meaning negative delta G*?

DanielLee3H

I still don't really understand conceptually why at equilibrium, when energy is at its minimum, entropy is at its maximum? Don't things get more ordered when they get lower in energy?

DanielLee3H

Is the reason that systems at equilibrium release energy slowly but more efficiently than a sudden release of energy be related to something like taking the intergral over an infinite number of time steps versus taking larger changes in time?

DanielLee3H

Why does heat capacity increase with molecular complexity? Does molecular complexity mean just number of molecules or number of bonds in a molecule?

CHEMISTRY COMMUNITY

Search found 17 matches

Is carbon monoxide an electrophile

Cell potential

Re: Entropy at equilibrium pt2

Entropy at equilibrium pt2

Strains

Curved arrow [ENDORSED]

I has question

Re: Deriving the differential rate law

Deriving the differential rate law

Book problem 14.15

Gibbs free energy question

Thermodynamic vocabulary

I am confusion about cell potential. [ENDORSED]

Equilibrium Constants

Entropy at equilibrium

Systems at equilibrium [ENDORSED]

Heat capacity