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April 23, 2014

Search: chemistry-rate of reaction

Number of results: 117,332

Chemistry
A + 2 B = C + D describes an elementary reaction, which takes place in a single step. Thus, the rate law must be a) rate = k (A)^2 b) rate = k (B)^2 c) rate = k (A) (B) d) rate = k (A) (B)^2 I think its D because there are 2 moles of B and 1 mole of A. Do you agree with my ...
Friday, February 24, 2012 at 2:34am by Mohamed

chemistry
(B) is not in the rate expression; therefore, changing (B) will not affect the rate. If the rate order for A is 1, the answers are the same. If the rate order of A is 0, the rate doesn't depend on A or B.
Thursday, November 18, 2010 at 1:23pm by DrBob222

chemistry
The equation A + 2 B = C + D describes an elementary reaction, which takes place in a single step. Thus, the rate law must be a. rate = k(A]2 b. rate = k(B]2 c. rate = k(A][B] d. rate = k(A][B]2 e. none of the above represents the rate law for this elementary reaction.
Friday, February 24, 2012 at 8:19pm by bob

chemistry
The equation A + 2 B = C + D describes an elementary reaction, which takes place in a single step. Thus, the rate law must be a. rate = k(A]2 b. rate = k(B]2 c. rate = k(A][B] d. rate = k(A][B]2 e. none of the above represents the rate law for this elementary reaction. help
Saturday, February 25, 2012 at 10:09am by bob

chemistry
What is the rate? You don't list the rate or rate constant and I don't see any way to calculate the rate.
Sunday, February 21, 2010 at 9:42pm by DrBob222

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- rate laws
rate for second order rxn = k(A)^2 0.1 = k(0.01)^2 Solve for k. Then substitute k into rate = k(A)^2 with A = 0.5 and solve for rate. The answer is 250 which i 2.5E2.
Tuesday, September 18, 2012 at 10:18am by DrBob222

Chemistry
The rate of a reaction A ---> B is expressed by the rate expression rate=k(A)2. If the molar concentration of A is tripled, the rate of the reaction should increase by a factor of some many?
Saturday, February 9, 2013 at 5:49pm by Marcus

Chemistry
rate 1 = k*(PCl3)^0(Cl2)^y rate 2 = k*(PCl3)^0(Cl2)^y The problem says rate increases by 4 when we double Cl2. So let's do that. Let's call rate 1 = 1 to make things simple; also, since (PCl3)^0 = 1 we can dispense with that, too. Then we will call (Cl2)= 1 with rate 1, again...
Wednesday, February 27, 2008 at 5:33pm by DrBob222

Chemistry
For the reaction, 2 XO + O2 = 2 X02, some data obtained from measurement of the initial rate of reaction at varying concentrations are given below. run # [XO] [O2] rate, mol L-ls-l 1 0.010 0.010 2.5 2 0.010 0.020 5.0 3 0.030 0.020 45.0 The rate law is therefore a. rate = k[XO]...
Monday, February 20, 2012 at 4:29pm by Hannah

Chemistry
For the reaction, 2 XO + O2 = 2 X02, some data obtained from measurement of the initial rate of reaction at varying concentrations are given below. run # [XO] [O2] rate, mol L-ls-l 1 0.010 0.010 2.5 2 0.010 0.020 5.0 3 0.030 0.020 45.0 The rate law is therefore a. rate = k[XO...
Monday, February 20, 2012 at 3:10pm by Hannah

Chemistry(Please check)
there is a difference between the rate constant, and the rate. Changing concentration affects rate.
Sunday, February 19, 2012 at 6:07pm by bobpursley

Chemistry
X + Y --> Q The reaction above has the rate law: rate = k[X]. When [X] is doubled the rate increases by a factor of ?
Wednesday, March 9, 2011 at 2:16pm by Anthony

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
O2 effuses at a rate that is _____ times that of Xe under the same conditions. rate 02/rate x2 = ?
Friday, June 21, 2013 at 4:11pm by Annie

chemistry
Determine the overall orders of the reactions to which the following rate laws apply: a) rate= k[NO2]^2 b) rate = k c) k [H2][Br2]^1/2 d) k [NO]^2[O2] is it.. a. 2 b. 0 c. 1 1/2 d. 3
Thursday, July 15, 2010 at 1:03am by Jin

chemistry
What is the rate of the following reaction (M/s) if the rate constant for the reaction is 0.500 Lmol-1s-1 and the concentration of each reactant is 0.0628 M. (The units for the rate constant depend upon the rate law). CO + NO2 --> CO2 + NO
Saturday, November 20, 2010 at 10:35pm by Confused

chemistry
Nitric oxide (NO) can be removed from gas-fired power-plant emissions by reaction with methane as follows: CH4(g) + 4NO(g) --> 2N2(g) + CO2(g) + 2H2O(g) Complete the equation relating the rates for each of the following: a) the rate of appearance of N2 to the rate of ...
Monday, October 15, 2012 at 6:56pm by Brun

chemistry
For the reaction, 2 XO + O2 = 2 X02, some data obtained from measurement of the initial rate of reaction at varying concentrations are given below. run # [XO] [O2] rate, mol L-l s-l 1 0.010 0.010 2.5 2 0.010 0.020 5.0 3 0.030 0.020 45.0 The rate law is therefore a. rate = k[XO...
Friday, February 17, 2012 at 9:18pm by steve

Chemistry
For the reaction, 2 XO + O2 = 2 X02, some data obtained from measurement of the initial rate of reaction at varying concentrations are given below. run # [XO] [O2] rate,mol L-l s-1 1 0.010 0.010 2.5 2 0.010 0.020 5.0 3 0.030 0.020 45.0 The rate law is therefore a. rate = k[XO]...
Tuesday, February 21, 2012 at 5:18pm by Kay

chemistry-rate of reaction
rection rate=rate constant * conc^2
Sunday, December 2, 2012 at 12:07am by qwerty

chemistry
Wouldn't the rate of disappearance for H2O2 be the same as the rate of appearance of I2? And the rate of disappearance of I^- would be 1/2 rate of I2? Check my thinking.
Friday, November 27, 2009 at 6:13pm by DrBob222

Chemistry
1) The rate expression for the reaction 2 SO2 + O --> 2 SO3 is given by rate = k [SO2]2[O2]. The overall order of this reaction is: first order 2)The rate reaction between A and B is expressed as rate = k [A][B]. To produce the greatest increase in the reaction rate: double...
Sunday, December 23, 2007 at 8:42am by Anonymous

chemistry
rate F2 = 3.632L/2.040 min = ? (?/rate UF4) = sqrt(molar mass UF4/2*19) Solve for rate UF4 gas, then rate = 3.632 L/min. You have rate and L, solve for min.
Tuesday, March 5, 2013 at 8:42pm by DrBob222

chemistry
I did 3 Experiments and got 3 rate as the following: Exp1: (S2O8)2-:0.05M; I-:0.05M rate:1.7x10^-5 M/s Exp2: (S2O8)2-:0.10M; I-:0.05M rate:3.4x10^-5 M/s Exp3:(S2O8)2-:0.05M; I-:0.10M rate:3.6x10^-5 M/s what effect does doubling [(S208)2-] have on the rate? By what factor does ...
Friday, October 1, 2010 at 1:07pm by Kimberly

Chemistry II
rate = k(A)(B)^2 rate = k(4)(7)^2 rate = k*4*49 you finish
Wednesday, September 30, 2009 at 1:35am by DrBob222

Chemistry
The reaction X + Y --> products was studied using the method of initial rates. The initial rate of consumption of X was measured in three different experiments. What is the value of the rate constant, k? *concentrations are in mol/L and initial rates are in molL-1s-1 Exp 1...
Wednesday, February 23, 2011 at 10:51am by Jamie

chemistry
3 CH3NH2 + 11 HNO3 ---> 3 CO2 + 13 H2O + 14 NO RATE OF DISAPPEARANCE OF NITRIC ACID IS 20M/min. what is the rate of reaction? at what rate is the concentration of carbon dioxide changing?
Sunday, December 5, 2010 at 1:17pm by candace

Chemistry
-rate A = -1/3 B = 1/2 C. Is that what you mean by "relative"? That means if A is disappearing at the rate of 0.480 M, then B is disappearing at the rate of 3*0.480M and C is appearing at the rate of 2*0.480M.
Saturday, July 16, 2011 at 2:09pm by DrBob222

Chemistry - Rate Law
The following example is given in my textbook: If a chemical equation is: NO2 (g) + CO (g) -> NO (g) + CO2 (g) The rate law is: Rate = k[NO2]^2 Usually you put in the reactants in their own sets of brackets, so why isn't the reactant CO involved in the rate law? I get it ...
Wednesday, January 31, 2007 at 4:44pm by Belinda

Chemistry(Please check)
I don't think so. rate = k(A)^3 so k = rate/(A)^3 Plug in mol/L*min for rate and plug in moles^3/L^3 for A^3 and go through the algebra.
Sunday, February 19, 2012 at 5:43pm by DrBob222

chemistry
The rate constant for this reaction was found to be 0.00550 s-1. What is the instantaneous rate of reaction when the concentration of dinitrogen pentoxide is 0.100 M? Rate = k[N2O5].
Thursday, April 26, 2012 at 5:15pm by Anonymous

Chemistry
Graham's Law predicts that the ratio of the rate of effusion of gas X to the rate of gas Y equals the square root of the INVERTED ratio of their molar masses: Rate of X/Rate of Y = SQRT(My/Mx) What is the ratio of rate of effusion of Helium to Nitrogen gas? Enter your answer ...
Sunday, October 28, 2012 at 8:20pm by Anonymous

Chemistry - Rate Determining Step
According to the Liebig law of "Minimum" and the Blackman law of limiting factors, the rate of a multi-step reaction is determined by the step which has the lowest rate or velocity. This step is called the Rate-Determining or Rate-limiting Step.
Tuesday, February 6, 2007 at 10:35pm by Hadi Farazdaghi

chemistry
For the reaction, A = B + C, the rate law is kA]. If it takes 80.0 seconds for 70.0% of a 10.0 gram sample of A to be transformed into products, what is the value of the rate constant? a. 0.00450 s-1 b. 0.0290 s 1 c. 0.00530 s-1 d. 0.0150 s-1 e. 5.40 s-1 chemistry - DrBob222, ...
Saturday, February 18, 2012 at 9:20pm by elvis

Chemistry
What is the correct rate law for the following reaction? 2 NO2(g) + F2(g) → 2 NO2F(g) rate = kf(NO)2 rate = -kf(NO2)2(F2) rate = kf(NO2)2(F2) rate = -kf(F2) Not enough information is available to determine the rate law.
Monday, May 16, 2011 at 9:52pm by dude

Chemistry
rate = -delta [N2O5]/delta time rate = (0.218-0.0296)/282 = ? Then rate = k[A]. Calculate k.
Friday, January 24, 2014 at 9:35pm by DrBob222

Chemistry
The rate equation is rate = k(CO)^x(O2)^y. Divide rate 2 by rate 1. 0.226/0.113 = 2 and 2 = (0.300)x(0.150)y/(0.150)x(0.150)y Note that 0.150y cancels with 0.150y and leaves just 2= (2)x and x must be 1. Do the same thing for rate 3 divided by rate 2 and determine y. You ...
Thursday, June 30, 2011 at 11:11pm by DrBob222

chemistry
(rate 1/rate 2) = sqrt(M2/M1) rate = 4.83/sec and 9.23/sec.
Wednesday, October 31, 2012 at 5:41pm by DrBob222

Chemistry
Choose a convenient volume such as 1 L. Then rate CO2 = 1L/200 s = ? rate unknown = 1L/280 s = (rate CO2/rate unk) = sqrt(MMunk/MMCO2) MM = molar mass. Solve for MM unk.l
Monday, February 18, 2013 at 11:56am by DrBob222

chemistry
disappearance of NO in ...- Help!!!? The following data were collected for the rate of disappearance of NO in the reaction 2 NO(g) + O2(g) 2 NO2(g). Run: [NO](M) [O2](M) Initail Rate (M/s) 1 .0126 .0125 1.41 X 10^-2 2 .0252 .0125 5.64 X 10^-2 3 .0252 .0250 1.13 X 10^-1 (a) ...
Wednesday, January 30, 2013 at 5:55pm by Hannah

Chemistry
1. How is the rate affected by doubling the concentratino? 2. Explain the effect of concentration on the rate of a reaction in terms of the "Collision Theory" of chemical reactions. 3. Considering that 1/Time is proportional to the rate of the reaction how is the rate of the ...
Sunday, November 18, 2007 at 3:05pm by Dick Rogers

Chemistry
I would make up a rate for the unknown gas and multiply that made up rate x 6.7 to find the rate of H2. Plug in those numbers. rate1/rate2 = sqrt(M2/M1) Solve for M (depending upon what you call rate 1 and rate2, M2 and M1.
Thursday, April 22, 2010 at 12:57pm by DrBob222

chemistry
Generally adding more (higher conc) acid will increase rate and lower M will decrease rate. Changing the volume up or down will not impact the rate assuming you have enough to begin with to have a reaction.
Wednesday, May 22, 2013 at 10:08pm by DrBob222

chemistry
There are different definitions for different subject areas. In chemistry, chemical equilibrium is when the rate of the forward reaction = rate of reverse direction.
Saturday, October 5, 2013 at 9:03am by DrBob222

chemistry-please help
I don't know how to find generic rates and how to find rate of production? Example: 2HgCl2+ C2O4 goes to 2Cl + 2CO2 + Hg2Cl2 Experiment 3: [HgCl2]=.052 [C204]=.300 the inital rate (M/min of Hg2Cl2) is 3.54E-5. What is the generic rate of the reaction and what is the rate of ...
Tuesday, February 24, 2009 at 12:46am by eliz

chemistry
What is the rate of disappearance of dinitrogen pentoxide between 100 s and 200 s? Is this rate higher or lower than the rate from 0 s to 100 s that you calculated in part c? As the reaction takes place, what happens to [N2O5]? In general, does a higher concentration of ...
Thursday, April 26, 2012 at 5:14pm by Anonymous

chemistry
At the instant oxygen is reacting at the rate 5.0 x 10-4 mol/L*s, at what rate is NO reacting and NO2 forming? this is a method of initial rate problem. i don't know what to do the chemical equation is 2 NO(g) + O2 (g) ---> 2 NO2 (g)
Saturday, September 8, 2007 at 6:26pm by Chris

che,istry
Isn't the rate for a first order reaction rate = k[A]?. rate = 0.5 Make A anything and solve for k. Then use rate = k[A]. you know k and [A] now is 1/2. Then 1/4. solve for rate for each. Check my thinking.
Sunday, July 6, 2008 at 11:12pm by DrBob222

chemistry
Determine the overall orders of the reactions to which the following rate laws apply: a. rate = k[NO2]^2 b. rate = k c. rate = k[H2][Br2]^1/2 d. rate = k[NO]^2[O2] I think the answers are: a. Second Order b. Zero Order c. First Order for H2 and One-half order for Br2 d. Second...
Sunday, July 18, 2010 at 9:58pm by Sara

Chemistry
For the reaction: 5A + 3B -> 6C + D, the following data is found: Time________A 0.00s .775 M 5.00s .200 M Find the rate of disappearance of A, the overall rate of reaction, and the reates of disapperance and appearance of B, C, and D. The answers I got were: Rate of ...
Wednesday, February 21, 2007 at 11:18am by Aletha

Chemistry
When 0.13 g of H2 and 0.18 g of I2 are confined to a 150. mL reaction vessel and heated to 700. K, they react by a second-order process (first order in each reactant), with k = 0.063 Lmol-1s-1 in the rate law (for the rate of formation of HI). (a) What is the initial reaction...
Friday, June 28, 2013 at 4:41pm by Sara

Chemistry
No volume is listed; let's make up a volume, say 2 L for He, then the rate is (2L/2sec) = 1 L/s. Then rate1/rate2 = sqrt(M2/M1) 1/rate 2 = sqrt(80.9/4) solve for rate 2, then rate = 2L/sec and solve for sec. Post your work if get stuck.
Tuesday, December 4, 2012 at 9:58pm by DrBob222

Chemistry
You can change the rate of the reaction by increasing OH or CH3Br (will increase rate) or decreasing OH or CH3Br (will decrease rate). Cooling the reaction mixture will decrease the rate; increasing T will increase rate.
Monday, April 16, 2012 at 2:05pm by DrBob222

AP Chem
RATES: If you double the concentration of reactant A in the reaction A + 2B C, what happens to the rate based on the rate law, rate = [A]2 [B]3? The rate would ___ by a factor of ___. increase, 2 increase, 4 decrease, 2 decrease, 4 I can't read some of the signs; however, ...
Tuesday, January 23, 2007 at 9:43pm by Chemwiz

chemistry
the rate law choices are: 1. rate in respect to net=k[NO][H2] 2. rate net=k[NO]^2[H2]^2 3. rate net=k([H2]^2[NO]^2)/[H2O] 4. rate net=k[NO]^2[H2] 5.rate net=k([N2][H2O]^2[H2]^2)/[NO]^2 please help! :)
Monday, January 10, 2011 at 10:04pm by Anonymous

chemistry
Consider the reaction below: Cgraphite(s) + F2(g) +1/2O2(g) → CF2O(g) Which of the following is a correct rate expression? 1. rate = −2∆[O2]/∆t 2. rate = −∆[CF2O]/∆t 3. rate =∆[F2]/∆t 4. rate = −∆[Cgraphite]/&#...
Tuesday, February 7, 2012 at 8:55pm by bob

chemistry
Give an arbitrary rate to the reaction at the 21.5C Lets say it is 100 moles/sec Then the rate at 35.6 is 160.3 M/s Now, take the natural log of each of those rates. Plot ln rate vs 1/tempinKelvins The slope of that line is Ea/R where R is the universal gas constant.
Sunday, March 23, 2008 at 8:59pm by bobpursley

Math interest rate
Please explian how to figure out the the initial interest rate of the ARM ? Given th these facts thanks :) Ben bought a home with an adjustable-rate mortgage. The margin on the loan is 2.7% and the rate cap is 7.2% The current index rate is 4.3%
Wednesday, November 14, 2007 at 2:21pm by Anonymous

Chemistry Lab
What would happen to the reaction rate of a solution if 10 mL or more of water is added? Will the reaction rate increase or decrease? The following reaction occurs without a change in the color 2A (g) + B2(g) --- 2AB (g) a) How could you monitor the concentration of the ...
Monday, July 20, 2009 at 11:07pm by Sunshine

Chemistry Lab
What would happen to the reaction rate of a solution if 10 mL or more of water is added? Will the reaction rate increase or decrease? The following reaction occurs without a change in the color 2A (g) + B2(g) --- 2AB (g) a) How could you monitor the concentration of the ...
Monday, July 20, 2009 at 11:08pm by Sunshine

Chemistry
1. Nitric oxide reacts with bromine gas at elevated temperatures according to the equation, 2 NO(g) + Br2(g) = 2 NOBr(g) The experimental rate law is rate = k[NO][Br2]. In a certain reaction mixture the rate of formation of NOBr(g) was found to be 4.50 x 10-4 mol L-l s-l. What...
Sunday, February 19, 2012 at 6:14pm by Hannah

chemistry
i see what your saying. so multiply the rate by two to get the rate of NO? but what is NO2 forming
Saturday, September 8, 2007 at 6:26pm by Chris

chemistry
The correct answer is D. At equilibrium, the forward rate equals the reverse rate.
Thursday, April 10, 2008 at 9:59pm by DrBob222

Chemistry
a car is traveling at a rate of 41.2 megameters/hr. what is the rate in cm/s?
Wednesday, September 15, 2010 at 7:16pm by Lisa

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
What are the units for the rate constant for a second and third -order rate law?
Tuesday, March 20, 2012 at 12:16am by Kaleen

chemistry
Is it possible for this equation 2C + D = E + F to have a rate law of rate = k [C]^2[D]^3
Tuesday, April 8, 2008 at 10:11pm by william

chemistry
Explain the difference between the rate of a reaction and its rate constant.
Thursday, October 13, 2011 at 6:40pm by chris

Chemistry
(rate O2/rate N2) = sqrt(28/32)
Thursday, October 4, 2012 at 1:25am by DrBob222

chemistry
How do I figure this out? If argon diffuses at a rate of 15, what rate does krypton diffuse at?
Thursday, February 26, 2009 at 5:32pm by kayla

chemistry(check my answer)
its kf,kr, the value of forward rate and reverse rate.
Friday, May 14, 2010 at 2:32am by Jay

chemistry
use the formula rection rate=rate constant * conc^2 and the answer is=0.050319
Friday, November 30, 2012 at 12:30am by amar chauhan

chemistry
The rate law of the overall reaction. A + B -> C is rate = k[ A ]^2 Which of the following not increase the rate of a chemical reaction? a) increasing the temperature of the reaction b)increasing the concentration of reaction A c)adding a catalyst for the reaction d)...
Thursday, November 18, 2010 at 1:23pm by ben

Chemistry 2
An industrial chemical reaction has a rate law: rate = k [C]. The activation energy for the reaction is 3.0000 x 10^4 J/mol and A = 2.000 x 10^-3. What must be the reaction temperature if a rate of 1.000 x 10^-9 M/s is required and [C] must be kept at 0.03000M. Hint: What must...
Monday, March 12, 2012 at 1:18pm by Jessica

Chemistry(Please check)
So wouldn't a catalyst just speed up the rate too and not the rate constant?
Sunday, February 19, 2012 at 6:07pm by Hannah

Chemistry
what is the rate of a first-order reaction that has a reactant concentration of 1.1M and a rate constant of 0.14/s?
Wednesday, May 1, 2013 at 1:59pm by George

chemistry
What must be known for the rate constant to be calculated from the rate law?
Saturday, March 10, 2012 at 7:42pm by princess

arts high enviromental science
birth rate death rate immigration rate emigration rate
Tuesday, March 9, 2010 at 7:27pm by Ms. Sue

Chemistry - Concentration and Time
1. How is the rate affected by doubling the concentratino? 2. Explain the effect of concentration on the rate of a reaction in terms of the "Collision Theory" of chemical reactions. 3. Considering that 1/Time is proportional to the rate of the reaction how is the rate of the ...
Saturday, November 17, 2007 at 8:59pm by Dick Rogers

Chemistry
i need help with a rate law question: The reaction is 2ClO2(aq) + 2OH -(aq)---> ClO3-(aq)+ ClO2-(aq) + H2O(l) Experiment 1: [ClO2]0= 0.0500 [OH-]0= 0.100 INITIAL RATE= 5.75*10^-2 Experiment 2: [ClO2]0= 0.100 [OH-]0= 0.100 INITIAL RATE= 2.30*10^-1 Experiment 3: [ClO2]0= 0....
Tuesday, June 2, 2009 at 6:49pm by Saira

chemistry 2
Meaning you want me to do all the thinking? rate 1 = rate oxygen = 2 liters/hour. rate 2 = rate unknown = (1/2)*2 = 1 liter/hour. Mol Weight 1 = mw oxygen = 32 mol wt 2 = mw unknown. (rate1/rate2) = sqrt (M2/M1). Substitute and solve for M2
Tuesday, February 16, 2010 at 10:22am by DrBob222

chemistry
A reaction has a rate law, rate = kA]B]^2 What is the overall order of the reaction? a. 2 b. 3 c. 0 d. 1 e. 4 chemistry - DrBob222, Friday, February 17, 2012 at 10:53pm The overall is the sum of the orders of each component. still dont get it but guessing A
Saturday, February 18, 2012 at 9:13pm by elvis

chemistry
I suppose you could work the 2-4 combinations out and memorize them; however, it's relatively easy to do one. For example, for the rate = k(x)^1(y)^2 for a third order reaction, you have k = rate/(x)^1(y)^2 = rate is M/t where M is molar and t is time. Tben k = (M/t)/(M)(M)2 k...
Sunday, December 12, 2010 at 5:41pm by DrBob222

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

chemistry
avg rate = (12.5-10)/50 min = ? mM/min. rate = k(NPP). You know NPP initially and the rate, solve for k. Plug all of this into the Arrhenius equation an solve for activation energy.
Saturday, April 12, 2014 at 5:33pm by DrBob222

chemistry
I don't remember all the posts you had yesterday. Did you read how to determine the rate law expression. Can you do that from these data? I seem to remember that it was zero with respect to C, 2nd order with respect to B and 1st order with respect to A. so the rate law ...
Saturday, February 18, 2012 at 9:18pm by DrBob222

Chemistry
Select the most likely rate law for the following: (CH3)3C-Br + OH- > (CH3)3C-OH + Br- a. Rate=k[(CH3)3C-Br] b. Rate=k[(CH3)3C-Br][OH-] c. Rate=k[(CH3)3C-Br][OH-]2 d. Rate=k[(CH3)3C-Br]2[OH-]2 e. Rate=k[(CH3)3C-Br]2[OH-] The correct is answer is "a" but I'm not sure why its...
Sunday, July 3, 2011 at 4:11am by Carole

chemistry
I have a problem like this: CHCl3 + Cl2 = CCl4 +HCL This is the rate table: CHCL3 Cl2 Initial Rate .010 .010 .0035 .020 .010 .0069 .020 .020 .0098 .040 .040 .027 They want me to find the rate constant and the rate law.
Saturday, February 23, 2013 at 10:18am by Nancy

Chemistry
I think the rate quoted is good as is; if any division/multiplication/etc are needed, they should have been done when quoting the rate.
Sunday, May 16, 2010 at 5:01pm by DrBob222

Chemistry
Sorry I typed it wrong i meant IF the rate of consumption of N2O4 (below) is .0221 what is the rate of production of NO2?
Sunday, January 23, 2011 at 1:58pm by Amber

chemistry
If the rate of disappearance of dinitrogen pentoxide is 0.0300 M/s, what is the rate of appearance of nitrogen dioxide? Use your equations from part a
Thursday, April 26, 2012 at 5:13pm by Anonymous

Chemistry
rection rate=rate constant * conc^2
Thursday, December 6, 2012 at 12:47pm by qwerty

Chemistry
rection rate=rate constant * conc^2
Tuesday, December 4, 2012 at 10:54pm by qwerty

Chemistry
rection rate=rate constant * conc^2
Tuesday, December 4, 2012 at 12:04am by qwerty

Chemistry
rection rate=rate constant * conc^2
Thursday, December 6, 2012 at 11:55pm by nenita

Chemistry
rection rate=rate constant * conc^2
Monday, December 10, 2012 at 1:31am by nenita

chemistry
rection rate=rate constant * conc^2
Friday, December 7, 2012 at 5:46am by nenita

chemistry
rection rate=rate constant * conc^2
Saturday, December 8, 2012 at 10:40am by nenita

Chemistry
Which of the following rate laws suggests that the reaction probably occurs in a single step? NO(g) + O2(g) → NO2(g) + O(g) rate = k[NO][O2] H2O2 + 3 I- + 2 H+→ I3- + 2 H2O rate= kl[H2O2][I-]+K2[H2O2][I-][H+] H2(g) + Br2(g) → 2 HBr(g) rate = k[H2][Br2]1/2 (...
Monday, May 16, 2011 at 9:55pm by dude

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