Number of results: 168
The profit (in millions of dollars) from the sale of x million units of Blue Glue is given by p= .7x-25.5. The cost is given by c= .9x +25.5 (a) Find the revenue equation. (b) What is the revenue from selling 10 million units? (c)What is the break-even point...
Monday, July 4, 2005 at 9:51am by GetYourLeash
A rocket blasts off vertically from rest on the launch pad with an upward acceleration of 2.30 m/s^2. At 10.0 s after blastoff, the engines suddenly fail, which means that the force they produce instantly stops. How high above the launch pad will the rocket eventually go? got ...
Saturday, September 16, 2006 at 4:02pm by Josh
The Decomposistion of nitrosyl chloride was studied: 2NOCl(g)--2NO(g)=Cl2(g) The following data were obtained where Rate= - change[NOCl] ------------ change in temp [NOCl]0 Initial Rate (molecules/cm^3) (molecules/cm^3*s) --------------------------------------- 3.0*10^16 5.98*...
Tuesday, December 5, 2006 at 5:43pm by Adrienne
chemistry - kinetics
The activation energy for the isomerization of methyl isonitrile is 160 kJ/mol. Calculate the fraction of methyl isonitrile molecules that have an energy of 160 or greater at 500 K? 510 K? What is the ratio of the fraction at 510K to that at 500K? I missed this lesson today ...
Tuesday, March 6, 2007 at 7:13pm by Mark
When experimentally determining the rate law, i am getting a negative fraction. is that right or am i doing something wrong? It is possibly right. I'd have to see you calculations to determine that. It would mean that the reaction is proceeding backwards.
Wednesday, March 7, 2007 at 10:56am by Kara
If I am titrating KMnO4 against a sample of Fe2+, but there is also I- in the sample which of the iron and iodine will be oxidised first? Unless something is present in the sample to complex the iodide ion, KMnO4 may titrate both. How are you titatrating it? What are you using...
Saturday, March 10, 2007 at 4:41pm by James
Heyy, okay I have this chemistry assingmnet and its on kinetics, and I got every single one except this one question and I've been trying for over an hour. I know that I'm probably jus tmissing something but everything I've tried doesnt work. Any help is greatly apprecaited. ...
Tuesday, March 20, 2007 at 12:28pm by Tracy
1.what term best describes the measure of hte increase in the concentration of a product per unit time? A)activation energy B)kinetics C)reaction rate D)reaction time 2. In the following equation, which of the reactants that is a bronsted-lowry acid HCN+H20-->H30+ + CN I ...
Friday, April 27, 2007 at 3:12pm by keith
A student proposes to use visible spectroscopy to measure the kinetics of the permanganate/oxalic acid reaction. The initial permanganate solution was very dark. For a 1 cm sample cell, the absorbance A = 2,500[MnO4]. As a practical rule of thumb, Beer's law is only accurate ...
Tuesday, January 22, 2013 at 3:04pm by Amy
Since this is not my area of expertise, I searched Google under the key words "enzyme inhibitors" to get these possible sources: http://en.wikipedia.org/wiki/Enzyme_inhibitor http://en.wikipedia.org/wiki/Enzyme http://www.elmhurst.edu/~chm/vchembook/573inhibit.html http://...
Monday, September 10, 2007 at 9:29pm by PsyDAG
Organic chemistry: dehydrohalogenation
DrBob has essentially covered it. It is not that easy to generalise, you need to consider each halide looking for steric influences, stabilisation of a carbocation and stability of the product. Some general points: E1 is a two-step process of elimination ionization and ...
Wednesday, October 10, 2007 at 11:21pm by Dr Russ
Chemistry - Kinetics
When a reaction is catalyzed: a) Is the catalyst involved in the reaction? (State your evidence) b) Has the catalyst been consumed when the reaction is complete?
Tuesday, November 13, 2007 at 1:04pm by Dick Rogers
Chemistry - Kinetics
a) Yes, you can probably tell because the activation energy gets lower and thus allow the reaction to speed up way faster than without a catalyst... it's kind of dumb to ask if in catalyst is involved in a CATALYZED reaction... b) No, the catalyst will get recycled at the end ...
Tuesday, November 13, 2007 at 1:04pm by Jake
Chemistry - Kinetics
a)Yes, the catalyst enters into the reaction. b) Although the catalyst enters into the reaction, it is regenerated in a subsequent step; the net effect is that none of it is consumed. Here is a site that gives some examples. http://en.wikipedia.org/wiki/Catalyst
Tuesday, November 13, 2007 at 1:04pm by DrBob222
Hey; I'm currently in a kinetics class and I am trying to do a prelab for a lab that we haven't learned the material for yet and I'm really stuck, and we unfortunately don't have a textbook for the class so I was hoping someone could help. We have the compound m-xylene and it ...
Monday, February 11, 2008 at 8:29pm by Tracy
I'm really struggling to understand this chapter in chem class, partly due to an inadequate math background. does anyone have any tips for learning kinetics? i'm starting to fall behind.
Monday, February 25, 2008 at 11:41pm by Gabe
The kinetics of the catalytic decomposition of NH3 into N2 and H2 on a hot tungsten filament at 1100 °C was investigated by Kunsman. He measured the times (t1/2) required for half of NH3 to decompose at different initial NH3 pressures, as shown below: P (torr) t1/2 (minutes) ...
Monday, May 3, 2010 at 11:34am by Teddy
Dinitrogen tetraoxide, N2O4, decomposes to nitrogen dioxide, NO2, in a first-order process. If k = 2.5 x 103 s-1 at -5° Cand k = 3.5 x 104 s-1 at 25° C, what is the activation energy for the decomposition? 0.73 kJ/mol 58 kJ/mol 140 kJ/mol 580 kJ/mol I am having massive ...
Saturday, September 25, 2010 at 10:04pm by lucylu
I have been studying a journal, and their objective is to find the ignition temperature, which can shift a reaction from being kinetics-controlled to being diffusion-controlled. What is the advantage of a reaction being diffusion-controlled over a reaction being kinetics-...
Tuesday, May 8, 2012 at 8:26pm by Namie
Decomposition of an organic compound A follows first order kinetics. Initial concentration of A is 2 M. If rate constant of the decomposition is 3.58 × 10^−6 min^-1 , calculate the rate after 3 hours.
Thursday, May 24, 2012 at 1:03am by swa