CHEMISTRY COMMUNITY

105169446

But if you have a plot of [reactant] vs time for a first order reaction then in that case you'll get an exponential curve which is decreasing.

105169446

What happens if the slow step has an intermediate in it?

105169446

I am still unsure about what an activated complex model is. Could someone clarify?

105169446

What is the difference between a differential rate law and an integrated rate law?

105169446

I have another question about this problem. The solution manual says that Ka = sqrt(K), but I don't remember learning this. How do we know this?

105169446

The solution of this problem mentions the formula ln K = nFE/RT.
I am not sure how to get to this formula.

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Yes, because the unique rate is an instantaneous rate which means it is different at each point in time.

105169446

It mainly allows us to identify the speed at which a reaction occurs, in particular the rate at which reactants decrease and products form.

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In what cases do we use the differential rate law formula, K[R]^n?

105169446

What is the oxidation number?

105169446

In the lecture from February 15th, Dr Lavelle wrote in his notes that "If Gr different from Gp, then the system (reaction) is not at equilibrium." I just want to make sure that r is for reactants and p for products.

105169446

In the formula for delta Srxn, we have the sum of the products of Sm minus the sum of the reactant of Sm.
I'm confused about what the "m" of Sm is.

105169446

When the change in entropy is reversible, you can also use delta S = nrln(V2/V1) or delta S = nCln(P1/P2) because pressure is inversely related to volume.

105169446

Delta S=q/T so since temperature is the denominator, if you make T bigger, delta S will be smaller and vice versa, if you make T smaller, delta S will be bigger. That explains why the change in entropy is larger when the temperature is lower.

105169446

And just as a reminder, a state property is not dependent on the path taken to obtain that state.

105169446

What are the 2nd and 3rd law of thermodynamics be if we summarize them in a sentence each?

105169446

Are we only going to have to calculate the change in Gibbs free energy, or will we ever have to calculate the actual Gibbs free energy for a certain point?

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I am still confused as to what exactly the difference between degeneracy and entropy? Don't both of these concepts relate to disorder in a system?

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Dr Lavelle just sent an email today I believe with all the dates and times for midterm review sessions this coming week.

105169446

Could someone explain the detailed reasoning for questions 2.a. and b. on worksheet 1?

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Is an isolated system always closed?

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I don't think they will be given to us since learning and knowing basic Lewis structures was gone over in Chem 14A.

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In number a of 6D.3, the solution manual gives the Ka of chlorous acid and it says [HClO2] is 0.10-0.06, 0.06 being the concentration of HClO2's conjugate base, ClO2-. I don't understand why it's 0.10-0.06 and not just 0.10.

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Are there specific cases in which we should use one of the three methods over the others to calculate delta H?

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No, I believe combustion is never reversible, no matter the circumstances. The C02 and water formed cannot react to reform the fuel and oxygen, so the reaction is always irreversible.

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In lecture, Prof Lavelle alternates between delta H and delta Hº. Is there a difference between the two? If there is, I which situation should I use which symbol?

105169446

In lecture, Prof Lavelle alternates between delta H and delta Hº. Is there a difference between the two? If there is, I which situation should I use which symbol?

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I looked at the solution for this question and the manual says "The concentration of N2 and O2 remain practically the same at 0.114 mol/L". I don't understand how we can come to this solution. Could someone enlighten me?

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I was absent on the day of the first lecture, so there is something in the notes I received that I don't quite understand. When we are given the example of a forward reaction with N2 and H2 as reactants and NH3 as the product. We calculate the Kc for the forward reaction by replacing the Kc formula ...

105169446

I was absent on the day of the first lecture, so there is something in the notes I received that I don't quite understand. When we are given the example of a forward reaction with N2 and H2 as reactants and NH3 as the product. We calculate the Kc for the forward reaction by replacing the Kc formula ...

105169446

Could I have a clarification on what it means exactly when a reaction reaches equilibrium? Thank you

105169446

Hello, I am having a difficult time figuring out how to solve the two following questions: "23. 5.00 g of KMnO4 is dissolved in a 150.00 mL flask of water. If 20.00 mL of this solution is removed and placed in a new 2nd 250.00 mL flask and filled with water, what is the concentration of the sol...

CHEMISTRY COMMUNITY

Search found 32 matches

Re: Kinetics Plots

Re: Rate Determining Step

Re: Activated complex

Rate laws

Re: Problem 6.57 - 7th edition

Problem 6.57 - 7th edition

Re: Unique rates

Re: rate law

Differential rate law

Oxidation number

Gr and Gp from lecture

Delta Srxn

Re: Converting to q rev

Re: Enthalpy

Re: Gibbs Free Energy in relation to H and S

2nd and 3rd law of thermodynamics

Gibbs free energy

Re: Degeneracy

Re: Midterm Review

Re: DOWNLOAD SESSION WORKSHEETS HERE - Sun 7-9PM (Karen)

Type of systems

Re: Thermo Test/Midterm

7th edition 6D.3

Different enthalpy calculation methods

Re: reversible/irreversible

Delta Hº versus delta H

Delta Hº versus delta H

Question Focus 5I.17 7th edition

Clarification from lecture 1 - Jan 7th

Clarification from lecture 1 - Jan 7th

Definition of equilibrium

Pre-Module Assessment Q23 and Q25