Thursday
April 17, 2014

Search: kinetics

Number of results: 173

Kinetics
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

Physics
Kinetics is linked to dynomics by a) Velocity b) distance c) time d) acceleration I am not so sure but I have a feeling it is D acceleration, does anyone know anything about kinetics lol
Wednesday, January 27, 2010 at 8:09pm by euro

Reaction Kinetics
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

chemistry kinetics
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

chemistry
I looked for and count not find a good diagram. Finally I succeeded. http://www.kentchemistry.com/links/Kinetics/PEDiagrams.htm You can see that 40 + 30 = total = 70 for exothermic and equally you see that 100 = total = 20 + 80 http://www.kentchemistry.com/links/Kinetics/...
Friday, December 30, 2011 at 5:16pm by DrBob222

CHEM- KINETICS
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

Chemical Kinetics
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

chemistry
Here is your answer. http://www.chm.davidson.edu/vce/kinetics/integratedratelaws.html
Wednesday, April 6, 2011 at 1:57pm by DrBob222

chemistry
That's much better, although the solubility of NaCl is not much higher at 100 C than it is at 0 C. http://www.kentchemistry.com/links/Kinetics/SolubilityCurves.htm
Tuesday, February 21, 2012 at 9:11pm by DrBob222

Chemistry
Scroll down about half way to "Determining the rate law ...." Graph the data to determine which order. http://www.sparknotes.com/chemistry/kinetics/ratelaws/section2.rhtml
Saturday, July 17, 2010 at 2:36pm by DrBob222

Chemistry
HELP! we just started kinetics and i have no clue how to solve this problem. For the reaction between reactants A and B below, if 4.925 moles of A is placed into a flask with excess B it is found that the amount of A remaining after 6.85 seconds is 2.737 moles. 2A (g) + B (g...
Wednesday, February 20, 2008 at 2:44pm by Jonathan

Chemistry
http://www.chm.davidson.edu/vce/kinetics/IntegratedRateLaws.html
Saturday, November 14, 2009 at 8:04pm by DrBob222

chemistry
http://www.kentchemistry.com/links/Kinetics/SolubilityCurves.htm
Tuesday, February 21, 2012 at 9:08pm by DrBob222

Organic Chem
According to the problem, the rate constant, k, has units of M/s which is moles/L*s and that is for a zero order equation. The equation then is r = k and the concns don't enter into the equation at all. You can read more about it here. http://www.chm.davidson.edu/vce/kinetics/...
Wednesday, November 9, 2011 at 2:50am by DrBob222

CP Biology
You will need the solubility curves for each. The two curves are shown here, http://www.kentchemistry.com/images/links/Kinetics/Solubi1.gif
Thursday, September 16, 2010 at 9:50pm by Dr Russ

Chemistry
Just like any other average. (A) changed from 0.670 to 0.100 or 0.570 M. That change took 352 sec; therefore, 0.570/352 = ?? http://www.chem.purdue.edu/gchelp/howtosolveit/Kinetics/CalculatingRates.html#AvgRate
Saturday, July 16, 2011 at 3:37pm by DrBob222

kinetics
nigga
Thursday, March 8, 2012 at 5:54pm by Yolo

chemistry; kinetics
8.0x10-4
Saturday, May 29, 2010 at 5:04am by Hatsu

chemistry; kinetics
wrong 8.0x10-4
Saturday, May 29, 2010 at 5:04am by Jay

Kinetics Problem II
No data.
Wednesday, January 30, 2013 at 12:51am by DrBob222

CHEM- KINETICS
Can't you use the Arrhenius equation?
Saturday, September 25, 2010 at 10:04pm by DrBob222

Kinetics Problem I
Use the Arrhenius equation.
Wednesday, January 30, 2013 at 12:51am by DrBob222

Chemistry- Kinetics
BECAUSE THE MINUS SIGN WAS REMOVED IN THE EQUATION
Saturday, April 7, 2012 at 10:14pm by ASMA

PHYSICS
http://dwb.unl.edu/teacher/nsf/c09/c09links/www.kobold.demon.co.uk/kinetics/maxboltz.gif
Saturday, July 21, 2012 at 9:18pm by bobpursley

Chemical kinetics (chemistry)
I think endothermic is the word you are looking for.
Monday, March 5, 2012 at 3:04pm by DrBob222

Chemistry
https://www.colby.edu/NSF_AIRE/Kinetics.pdf
Monday, March 4, 2013 at 7:11am by DrBob222

chemistry, chemical kinetics
Thanks bro, atleast I know the second question can be right.
Friday, July 2, 2010 at 8:33pm by student

college kinetics chem
what is the rate law for 2OF2 yeilds O2 + 2F2
Saturday, October 9, 2010 at 3:27pm by Anonymous

CHEM- KINETICS
I think you can simply substitute into ln(Po/P) = kt and solve for p.
Sunday, September 26, 2010 at 12:01am by DrBob222

chemistry
You need to read about chemical kinetics in your text. Then post what you think your approach should be.
Wednesday, August 6, 2008 at 12:20am by DrBob222

Chemical kinetics (chemistry)
if the activation energy is larger from the perspective of the reactants than the products, the reaction is ?
Monday, March 5, 2012 at 3:04pm by Rose Bud

Chemical kinetics (theory)
Explain why a dust is much more explosive than is a stalk of grain.
Monday, March 5, 2012 at 3:17pm by Rose Bud

CHEM- KINETICS
thanks again DR BOB! this whole chemistry thing is a kick in the pants when you just cant get your head around it!
Saturday, September 25, 2010 at 9:53pm by lucylu

Impossible chemistry problem
Perhaps something here will give you some information: http://www.google.com/search?q=Kinetics+problem+tutorial&ie=utf-8&oe=utf-8&aq=t&rls=org.mozilla:en-US:official&client=firefox-a Sra
Friday, January 8, 2010 at 1:24am by SraJMcGin

Chemistry
what is the equation for activation energy in terms of chemical kinetics. i tried to look it up but i get something different every time
Tuesday, February 26, 2008 at 12:13am by Gabe

chemistry; kinetics
the spacing came out weird so just to clarify, the times are 0, 400, 800, 1200, and 1600 secs.
Saturday, May 29, 2010 at 5:04am by kris

Chemistry
After 79 mins 20.0% of a compound has decomposed. What is the half life of this reaction assuming first-order kinetics?
Saturday, July 16, 2011 at 7:06pm by Josh

chemistry
After 56.0 min, 25.0% of a compound has decomposed. What is the half-life of this reaction assuming first-order kinetics?
Tuesday, February 14, 2012 at 3:13pm by Anonymous

Chemistry
After 53.0 min, 14.0% of a compound has decomposed. What is the half-life of this reaction assuming first-order kinetics?
Monday, November 11, 2013 at 3:41pm by Shardai

chem: study of kinetics
I don't know what you plotted on Excel but slope is slope.
Saturday, October 16, 2010 at 2:20pm by DrBob222

chemistry
how do you find the rate of production when you already know the rate of consumption? kinetics questions
Tuesday, January 25, 2011 at 5:23pm by ashley

chemistry-chemical kinetics
by what factor is the rate of detoxification changed if a liver enzyme lowers the activation energy of the reaction by 5 kJ/mol at 37 degree celsius?
Saturday, December 15, 2012 at 9:45pm by eiry

Chemistry
Please can someone help explain the following: Explain the kinetics of combustion as a complex free radical process using hydrogen fuel.
Saturday, May 5, 2012 at 11:53am by Kitty

Chemistry
I need to perform a chemical demonstration on thermochemistry or kinetics or colligative properties for chemistry class. However I cannot have demonstrations involving fire.
Tuesday, January 12, 2010 at 8:14am by alex

chemistry
What is the half-life of a compound if 69 percent of a given sample of the compound decomposes in 59 min? Assume first-order kinetics.
Sunday, January 31, 2010 at 11:28pm by danielle

Chemistry
10% of a sample reacts in 25 s. If the reaction follows first order kinetics, how long would it take for half the sample to react?
Monday, May 3, 2010 at 9:44pm by mandy

chem
I think you are on the right track. It's a matter of rate of reaction. Think kinetics. Think activation energy.
Thursday, March 11, 2010 at 5:45pm by DrBob222

gen chem 2
In the chemical kinetics experiment, determine the dilution of the stock bleach solution. The bleach used will be around 5.5% (weight/volume). Convert this to molarity
Tuesday, February 8, 2011 at 6:59pm by jen

chemistry
The reaction x products follows Ist order kinetics in 40 minutes the concetration of x changes from 0.1M to 0.025M then the rate of reaction when conc of x is 0.01
Friday, April 26, 2013 at 5:04am by ameer

Chemistry.. kinetics
Typically, initial rate is the highest. Instaneneous rate is the unit in the differential equation that solves the rate law.
Tuesday, July 21, 2009 at 5:39pm by bobpursley

chemistry
the chapter is about chemical kinetics Reaction mechanisms: What does it mean by mechanism of a reaction? What is an elementary step? what is the molecularity of a reaction?
Thursday, July 15, 2010 at 2:12am by Jin

Kinetics Problem II
The data below were collected for the following reaction: 2NO2 (g) + F2 (g) ->2NO2F(g) A: Calculate the value of the rate constant, k. B: What is the overall order of the reaction?
Wednesday, January 30, 2013 at 12:51am by Amy

college chemistry
If gaseous H2 and O2 are carefully mixed and left alone, they can remain intact for millions of years. Is this “stability” a function of thermodynamics or of kinetics? Give a valid reason to support your choice.
Wednesday, April 28, 2010 at 1:04pm by Stephanie

chemistry, chemical kinetics
calculate the ratio of rate constants for two thermal reactions that have the same arrhenius preexponential,but with activation energies that differ by 1,10, and 30 kJ/mol for T= 298K
Friday, July 2, 2010 at 8:33pm by Anonymous

chemistry, chemical kinetics
calculate the ratio of rate constants for two thermal reactions that have the same arrhenius preexponential,but with activation energies that differ by 1,10, and 30 kJ/mol for T= 298K
Friday, July 2, 2010 at 8:33pm by Anonymous

Chemistry Kinetics
well i guess I need the negative sense it's the reactant -d[H2 + I2]/dt = k[H2]^x[I2]^y is this correct?
Wednesday, December 1, 2010 at 10:42pm by Kate

chem: study of kinetics
he gave us an example of what the slope might be in class and it was -1.3x10^2 but my slop is completely different, was i supposed to do calculations? or just get the one from excel? what do i put in the 2 blanks?
Saturday, October 16, 2010 at 2:20pm by chem

thermodynamics and kinetics
One mole of an ideal gas undergoes an isothermal reversible expansion, doing 1 kJ of work and doubling the volume. What is its final temperature? How much heat was added to the gas?
Friday, October 12, 2012 at 1:36pm by Dorota

Chemistry- Kinetics
Worked! Thank you! - Why is it ln(No/N) = kt though? The formula I have in my notes for first order reactions is ln(N1/No) = -kt
Saturday, April 7, 2012 at 10:14pm by Tasneem

chemistry
follows first-order kinetics and has an activation energy of 244 kJ mol-1. At 684 K, k = 0.00000508 s-1. What is the half-life (min) for this reaction at 427 °C ? Round your answer to 3 significant figures. I really dont know what to do
Friday, November 19, 2010 at 4:42pm by bobjahng2

Enzyme Kinetics-Km values
Hi guys, I don't quite understand why a lower Km value means more effective binding? Sincerely, Sandy
Saturday, January 31, 2009 at 2:08pm by Sandy

Physics
dynamics means motion. Kinetics means the physics of motions caused by forces. So d is the best answer, but really, it is a very poor question.
Wednesday, January 27, 2010 at 8:09pm by bobpursley

Chemical Kinetics
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

Chemistry.. kinetics
Initial rate Average rate instanteneous rate Which of these would have the highest value? Explain Please? Which one of these is typically used to determine the rate law for a reaction?
Tuesday, July 21, 2009 at 5:39pm by Sunshine

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

chem lab
I agree that you are confused. Apparently this was a potassium permanganate solution and you are doing some kind of experiment on chemical kinetics; however, you haven't given any other details (and those I had to guess). One possibility is that 1/T might be 1/time and not 1/...
Saturday, October 16, 2010 at 9:08am by DrBob222

Chemistry
may i plz get help ...regarding the statement of rate law..4rm the topic of chemical kinetics..i am unable to find the exact law statement..:( and i need it before mon.. i hope to get assissted soon! thankyou..!
Saturday, April 18, 2009 at 1:21pm by humaira

Chem
The National Institute of Science and Technology (NIST) kinetics database lists the rate constant, k, of a particular gaseous reaction as 5.78× 10–10 cm3·molecule^–1·s^–1 at 298 K. Convert this constant, k, to torr^-1 X S^-1.
Wednesday, February 27, 2013 at 5:59pm by Ann

chemistry
the concentration of a chemical degrades in water according to order kinetics. the degradation constant is 0.2 day^-1. if the initial concentration is 100.0 mg/L, how may days are required for the concentration to reach 0.14 mg/L?
Saturday, January 15, 2011 at 4:34pm by Maria

chemistry
The concentration of a chemical degrades in water according to order kinetics. the degradation constant is 0.2 day^-1. if the initial concentration is 100.0 mg/L, how many days are required for the concentration to reach 0.14 mg/L?
Saturday, January 15, 2011 at 4:34pm by Maria

Chemistry
The given reaction, 2N2O5 4NO2 + O2, follows first-order kinetics and has an activation energy of 103 kJ mol-1. At 298 K, k = 0.0000354 s-1. What is the half-life (min) for this reaction at 338 K ? Round your answer to 3 significant figures.
Thursday, November 11, 2010 at 4:53am by Kyo

chemistry
In fact, a rule of thumb in the kinetics business is that reaction rate can be doubled for every 10 degrees T. Since this ratio k2/k1 = about 2.05 I would guess T2 would be close to 365 or something like that.
Tuesday, March 25, 2014 at 11:21pm by DrBob222

Chemistry (kinetics)
None of the orders in this reaction were 0 order; however, reactions can be 0 order. Using the idea of a reaction mechanism and rate limiting step, explain how a reaction can be 0 order for a substance.
Wednesday, December 5, 2012 at 9:44pm by Shruti

Chemistry
Cyclopropane rearranges to form propene: CH2CH2CH2 --> CH2=CHCH3 by first-order kinetics. The rate constant is k = 2.74 x 10-3 s-1. The initial concentration of cyclopropane is 0.290 M. What will be the concentration of cyclopropane after 100 seconds?
Sunday, February 17, 2013 at 5:01am by Marcus

chemistry
N2O undergoes thermal decomposition at 730°C to nitrogen (N2) and oxygen (O2) via first-order kinetics with a half-life of 3.58 x 103 minutes. Calculate the time required for 90% of a sample of N2O to decompose at 730°C.
Monday, December 5, 2011 at 4:18pm by Cece

chem
Radioactive substances decay by first-order kinetics. How many years would be required for a sample containing strontium-90 to decrease to 58.32% of its initial activity? The half-life of strontium-90 is 2.88e1 years.
Saturday, February 22, 2014 at 6:36pm by sara

CHEM- KINETICS
The rate constant for a reaction is 4.65 L mol-1s-1. The overall order of the reaction is: zero first second third I am having trouble with the order of reactions. I dont understand this question. this is an assignment question but i have no idea how to do it.
Saturday, September 25, 2010 at 9:53pm by lucylu

Chemical Kinetics
a). NH3== N2 + H2 BAlance: 2NH3 == N2 + 3H2 -r= kC(NH3)2 >> Therefore th order of rxn is 2nd order
Monday, May 3, 2010 at 11:34am by Anonymous

chemistry kinetics
1. Statement-I : Fractional order reactions are not elementary reactions. Statement-II : For an elementary reaction, order must be same as molecularity. are these statements true? give reason.
Thursday, May 24, 2012 at 1:06am by swa

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

kinetics
a. KE = 0.5m*V^2 = 0.1*(20)^2 = 40 Joules. b. hmax = (V^2-Vo^2) / 2g. hmax = (0-(20)^2) / -19.6 = 20.41 m. c. V = Vo = 20 m/s.
Friday, March 16, 2012 at 6:12am by Henry

Inorganic chemistry
The decopostion of formic acid follows first-order kinetics. HCO2H(g)==>CO2(g) + H2(g) The half-life for the reaction at 550 degrees Celsius is 24 seconds. How many seconds does it take for the formic acid concentration to decrease by 75%?
Tuesday, May 12, 2009 at 6:03pm by Steve

chemistry kinetics
The reaction SO2Cl2(g) → SO2(g) + Cl2(g) is a first order reaction carried out at constant volume at 600 K whose t1/2 is 4.1 hr. The initial pressure of SO2Cl2 is 1.25 atm. What will be the total pressure of the system after 1 hour?
Thursday, May 24, 2012 at 1:04am by swa

chemistry
The given reaction, cyclopropane propene (isomerization), follows first-order kinetics. The half-live was found to be 4.57 min at 796 K and rate constant was found to be 0.0328 s-1 at 850 K. Calculate the activation energy (in kJ/mol) for this reaction. Round your answer to 3 ...
Tuesday, November 23, 2010 at 4:09pm by bobjahng2

chemistry
is this right? For first order kinetics: ln[A) = -kt + ln[Ao] ln[A) = - (6.29 x 10^-4 1/s)(1000. s) + ln (0.00100) ln[A) = -0.629 - 6.91 = -7.54 [A) = e^-7.54 = 5.33 x 10^-4
Sunday, October 24, 2010 at 9:51pm by jack ross

thermodynamics and kinetics
One mole of an ideal gas at 25C and 1 bar is allowed to expand adiabatically against a constant external pressure of 1.00 bar from 1.00 dm^3 to 10.00 dm^3. Calculate the final temperature, q, w, delta_U and delta_H.
Friday, October 12, 2012 at 1:36pm by Dorota

Kinetics Problem I
A reaction has a rate constant of 1.23×10-4 s at 28 degrees C and 0.235 s at 79 degrees C. A: Determine the activation barrier for the reaction. B: What is the value of the rate constant at 15 degrees C?
Wednesday, January 30, 2013 at 12:51am by Amy

chemistry. am i doing this right?
1.) One of the trials in this week's experiment in chemical kinetics was determined to be 10.60 seconds. Evaluate log10(rate). log10(rate) = Would I just plug 10.60 in for the rate?
Monday, September 10, 2012 at 10:37am by JJ

CHEM- KINETICS
this is a text book question that i cannot figure out. the decomposition of dimethyl ether at 510 degrees is a first-order process with a rate constant of 6.8*10^-4. (CH3)2O(g)--> CH4(g) + H2(g) + CO(g) if the partial pressure of (CH3)20 is 18kPa, what is its partial ...
Sunday, September 26, 2010 at 12:01am by lucylu

Chemistry- Kinetics
I assume you can do a from your text or notes. Look it up if you have doubts. b. ln(No/N) = kt No = 10.0g N = unknown k = 1.9E-4 sec^-1 (but this must be converted to hours or the time below into seconds). t = 2.8 hours. Solve for N to find how much remains, then subtract from...
Saturday, April 7, 2012 at 10:14pm by DrBob222

chem
this question is also based on the reaction above. The concentration of I2(g) is increased to 1.5 M, disrupting equilibrium. Calculate the new ratio of products to reactants with this higher concentration of iodine. Assume that the reaction has not yet regained equilibrium. ...
Wednesday, November 14, 2012 at 3:24pm by byke

Chemical kinetics (theory)
Everything you ever wanted to know about dust explosions. http://en.wikipedia.org/wiki/Dust_explosion
Monday, March 5, 2012 at 3:17pm by DrBob222

chemistry kinetics
Statement-I : For an endothermic reaction, the activation energy is less than the change in enthalpy. Statement-II: Activation energy of a reaction, at a given temperature can never be greater than its change in enthalpy are these statements true? give reason
Thursday, May 24, 2012 at 1:05am by swa

Chemistry
using kinetics explain: a.the increasing of concentration of reactants increases the rate of reaction. b.the addition of a catalyst increases the rate at which a reaction will take place. c.and increase in temperature increases reaction rate. d.a catalyst grounded into powder ...
Monday, March 3, 2008 at 8:58pm by Chuck

Kinetics Problem II
Here is the data. I am sorry that I forgot to list it: Initial Rate [NO2](M) [F2](M) Initial Rate (M/s) 0.100 0.100 0.026 0.200 0.100 0.051 0.200 0.200 0.103 0.400 0.400 0.411
Wednesday, January 30, 2013 at 12:51am by Amy

chemistry, chemical kinetics
For #2, the reaction is 1st order with respect to NO and 1st order with respect to Cl2 which makes it 1+1 = 2 = 2nd order overall. Cutting Cl2 in half is also true. Doubling NO is not true. The molecularity of the first step is not 1. Both steps are termolecular is not true.
Friday, July 2, 2010 at 8:33pm by DrBob222

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

Chemistry- Kinetics
2. At 600 K the decomposition of gas ohase nitroethane (CH3CH2NO2) is first order with a rate constant of 1.9*10^-4 s^-1. CH3CH2NO2 --> C2H4 + HNO2 a) Write out the differential and integrated rate laws for this reaction. b) If a 10.0g sample of nitroethane is heated to ...
Saturday, April 7, 2012 at 10:14pm by Tasneem

chemical kinetics
at 100C the gaseous reaction A==2B+C is observed to be first order.on starting with pure A it is found that at the end of 10min,the total pressure of the system is 176mmHg,and after a long time the total pressure of the system is 270mmHg.a).determine the initial pressure of A...
Friday, December 9, 2011 at 1:29am by Anonymous

Chemistry Kinetics
If I had the equation H2 + I2 --> 2HI could I write the rate of reaction as d[H2 + I2]/dt = k[H2]^x[I2]^y were x is the order of reaction with respect to x and y is just the order of reaction with respect to y thanks
Wednesday, December 1, 2010 at 10:42pm by Kate

Pages: 1 | 2 | Next>>

Search
Members