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Author:
Rosemary
- Replies:
1
- Views: 303
Calculating RRKM Rate Constants from Vibrational Frequencies and Their Dynamic Interp
[color=#555555][font=Arial,]ABSTRACT: Rice–Rampsberger–Kassel–Marcus (RRKM) theory calculates an energy-dependent microcanonical unimolecular rate constant for a chemical reaction from a sum and density of vibrational quantum states. This article demonstrates how to program the Beyer–Swinehart direct count of the sum and density of states for harmonic oscillators, as well as the Stein–Rabinovitch extension for anharmonic oscillators. Microcanonical rate constants are calculated for the decomposi
Author:
William07
- Replies:
0
- Views: 141
Decarboxylation (Chemical Reaction Rate)
I'm sorry for posting this as it may be an easy question for most, but it has been years since I took Chemistry and my background is in Microbiology.
I'll pose my question for anyone who has time to help:
I'm trying to use the data from research paper at the link here:
https://www.ncbi.nlm.nih.gov/pmc/articles/PMC5549281/#eq3
[size=medium]I'm trying to make a model wherein one could predict the time neces
Author:
James Dj
- Replies:
0
- Views: 245
For rate equations, are AB+A vs 2A+B vs A2+B equivalent?
For rate equations, are AB+A vs 2A+B vs A2+B equivalent?
I.e. if the reaction is dependent on the concentrations of A, do all three of the above give rate=k[A]2.
I think they would NOT be equal as A is a concentration.
[size=me
Author:
Cartert
- Replies:
0
- Views: 197
Relationship between equilibrium constant and rate constants
I have a question about calculating the equilibrium constant for the following gas phase reaction
2A
[Image:
http://www.chemicalforums.com/Smileys/cl...ibrium.png
]
B + C
[size=medium][color=#000000][font=Verdana, Helvetica, sans-serif]I am given
Author:
Michel
- Replies:
0
- Views: 241
Rate of reaction problem
Hi there,
I'm trying to do a rate of reaction problem I found online and am not getting the same answer as the one that is shown.
This is the reaction:
[size=medium][color=#000000][font=Verdana, Helvetica, sans-serif]2 AB(g) →
Author:
Zora
- Replies:
0
- Views: 139
Initial Rate Method Lab Question
I've just finished my lab report for my Chem 102 Lab, but I am very confused. I've completed the lab with what I know, but I don't know how to make sense of this. The order of the reactants are not equal to whole numbers. One of them is around 1.5 and the other is around 0.2. Below is a link to PDF scans of my calculations (pg 2). I feel that my thought process through the problem is summarized on the second page.
Thank you in advance!!
[size=medium
Author:
Gannon
- Replies:
0
- Views: 239
How to find the average rate based on the average of 2 slopes obtained(Kinetics)
[size=medium]Im really stuck on how to find the average rate based on the two slopes i did for my kinetics lab. For our lab we performed 3 experiments and ran 2 trails for each so a total of 6 trials and 6 graphs i have to show. So I converted the trials into seconds and for the first experiment we performed. I graphed the two trials on excel and for tiral 1 of the slope i got y= 0.0501x-1.5321; R2= 0.9977 and for trial two my slope was y= 0.0165x + 0.6452; R2= 0.994. So I know the slopes will b
Author:
Osbourn
- Replies:
0
- Views: 321
Integrated rate law when the stoichiometric coefficient of a reactant is 2/more
When we have an equation that is 2A-->B and we are told that it is a first order reaction, would the integrated rate law look like this: ln[A]t/[A]o = -2kt?
And the derivation looking like this:
Reaction rate = -Δ[A]/2t
-Δ[A]/2t = k[A]
-Δ[A]/t =2k[A]
therefore ln[A]t/[A]o = -2kt
[size=medium]So in an exam question where in the first part, we are first required to c
Author:
Caroline
- Replies:
0
- Views: 131
Rate of reaction and rate constant
[size=medium]In an experiment (reaction between acetone and iodine under acidic conditions), initial conc of iodine = 0.00455; initial concentration of H+ = 0.0455, and initial concentration of acetone is unknown. After 5 min intervals, reaction mixture is titrated against 0.0005 M thiosulfate solution. After calculating concentration of iodine remaining at time=t, i plotted a graph of concentration of iodine against time which is a straight line graph. Rate of reaction is zero order w.r.t iodin
Author:
Williamn
- Replies:
0
- Views: 152
Question on rate of reaction using concentration
Hello! So I have a question about concentration. We are given this balanced equation.
2Al(CH3)3(g)+3H2O(g) ::equil:: Al2O3(s)+6CH4(g)
The question says: "While the reaction number one is running, which of the following does not describe the rate of the reaction?"
A. -(1/3)(Δ[H2O]/Δt)
B. -(1/2)(Δ[Al(CH3)3]/Δt)
C. (-1/6)(Δ[CH4]/Δt)
[size=medium]D. Δ[Al2O3]/Δt[/s
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