CHEMISTRY COMMUNITY

Ray Huang 1G

Conceptually pH can't be negative. I'm not sure about the problem itself.

Ray Huang 1G

Nope forward and backwards are different. K = k1/k2. If k1 = k2 K would always = 1.

Ray Huang 1G

My TA specified we should know how to integrate at least the first order equation.

Ray Huang 1G

Determining rate is the slowest bc everything else must wait for it to complete before it can proceed. It's basically the bottleneck.

Ray Huang 1G

The order of each individual reactant tells you how changing the concentration of each will affect the overall rate of the reaction. The overall order will tell you how the reaction occurs and what mechanisms are used.

Ray Huang 1G

k in electro should be Boltzmann's constant while k in kinetics is a number unique to each reaction scaling how quickly the reaction proceeds.

Ray Huang 1G

Kinetically stable is that there is such a large energy hump that it is unlikely for a reaction to occur by itself. Thermodynamically stable is that the product has a higher energy state than the initial.

Ray Huang 1G

Positive potentials are reduced and negative are oxidized.

Ray Huang 1G

Balancing redox reactions requires a balance of charges. Since in normal reactions we don't look at charges, there is no need to (charge of 0 will always balance out with 0).

Ray Huang 1G

Reactions are spontaneous as long as Gibbs free energy is negative. The other values can be any combination of signs as long as the resulting Gibbs free energy value is negative.

Ray Huang 1G

The best way to do it is to look up the rules for oxidation numbers. He essentially looked at each element on each side of the table and found their oxidation number. Then he looked at if the number of the same element went up or down (comparing the left side to the right side). Using this you can f...

Ray Huang 1G

Check the reaction to see if more molecules are produced on the product side vs reactant side. Then check if it's in a container or not. Assuming Cp is usually safer.

Ray Huang 1G

Molecules means the whole thing. O2 is one molecule therefore n = 1. You may be thinking of atoms of O in O2 for n = 2 which is incorrect.

Ray Huang 1G

Cv is used when the problem states the volume doesn't change and Cp is for a constant pressure. In some cases, it's really tricky like the multi change one. But think about what value is changing at independent steps.

Ray Huang 1G

The bond enthalpies should be given or else we can't really solve the problem.

Ray Huang 1G

In a reversible reaction, we assume that the process occurs in minute increments back in forth but tending to one side. An increase in volume can be thought of as the volume increasing a little bit and then decreasing a bit and then increasing a bit. This allows for temperature to "balance out&...

Ray Huang 1G

Open system allows both matter and energy to be exchanged with the environment. A closed system allows only energy to do so. Isolated systems allow nothing to exchange with the env.

Ray Huang 1G

Steam is worse bc it can carry more energy for the same temperature compared to liquid water.

Ray Huang 1G

The sealed beaker can still exchange energy. By definition an isolated system must not exchange energy and matter. If you touch a beaker full of boiling hot water, you can feel how hot the beaker is getting. That's a closed system.

Ray Huang 1G

Enthalpy includes internal energy. Internal energy includes both kinetic and potential energy but enthalpy measure the total thermo potential so it adds on the pressure times volume part.

Ray Huang 1G

A reversible reaction has an equilibrium and will tend to that state naturally. Irreversible processes do not tend towards and equilibrium.

Ray Huang 1G

The units will cancel out when solving for equilibrium constants since the same units are in the numerator and denominator.

Ray Huang 1G

The reason pressure affects the reaction is the probability of one molecule colliding into another. The collision is what results in a change. If you increase the pressure by adding an inert gas, the molecule in question for the reaction crashing into the inert gas won't result in a reaction. The mo...

Ray Huang 1G

You can ignore it when the value of x you calculated is less than 5% of the initial concentration. If the x value is anywhere near or greater than 5% you have to do the quadratic by hand.

Ray Huang 1G

If your calculations are correct, then the solution is neutral. The [H30+]<10^-7 so therefore the amount of change in [H3O+] is negligible and the pH will not change dramatically from neutral.

Ray Huang 1G

Reply to Celine,

It doesn't always have to be in atm. You use whatever units are convenient or given to you. If the problem gives the gas constant in atm you have to use atm for your calculations.

Ray Huang 1G

The point of an ice chart is it gives you a way to organize and see how a reaction affects the concentration of reactants and product. It is used when we cannot assume a reaction goes to "100% completion". If you have the final resulting value of the reaction, you can find C by doing initi...

Ray Huang 1G

For part b the equation is what would happen if you took the original and divide it by two. Part c is when you take the original and multiply by two. I don't think we have yet to go over how to manipulate k when you do a scalar multiplication to the reaction.

Ray Huang 1G

Yeah you have to use a RICE table. If it's any help the book covers them starting page 441 in the 6th edition.

Ray Huang 1G

For question 7 in chapter 11 6th edition how do we visualize the equilibrium of a reaction? From what I can tell there is not a very compelling reason to say flask 3 is a better representation of equilibrium than flask 4 or vice versa. Both flasks have molecules that are kinda spread out and the rat...

CHEMISTRY COMMUNITY

Search found 30 matches

Re: homework question

Re: Rate constants at equilibrium

Re: integrating equations

Re: Reaction mechanisms

Re: Order of the Reaction

Re: k & K

Re: Kinetically Stable

Re: Potentials and Likeliness to be reduced/oxidized

Re: Difference

Re: Spontaneous

Re: Redox and Oxidation

Re: Calculating Delta S with a change in temperature

Re: n in degeneracy

Re: Cv vs. Cp

Re: Hess's Law

Re: Reversible vs. Irreversible processes

Re: Systems

Re: Steam

Re: Closed System

Re: Enthalpy vs Internal energy

Re: Irreversible and Reversible process

Re: Units When Calculating Equilibrium Constant

Re: Le Chatelier's Principle question

Re: ICE Table

Re: 7th edition 6A.23

Re: 11.89 Part B 6th Edition

Re: ICE chart

Re: 5H.1 part B

Re: 11.43

Visualizing Equilibrium