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September 3, 2015

Search: A zero-order reaction has a constant rate of 1.70×10−4 . If after 80.0 seconds the concentration has dropped to 6.00×10−2 , what was the initial concentration?

Number of results: 88,719

CHEMISTRY!
A zero-order reaction has a constant rate of 3.4010−4 M/s. If after 80.0 seconds the concentration has dropped to 6.0010−2 M, what was the initial concentration?
February 25, 2009 by Reese

Chemistry
A zero-order reaction has a constant rate of 3.2010^−4 M/s. If after 35.0 seconds the concentration has dropped to 9.0010^2M , what was the initial concentration?
April 30, 2010 by D.Walker

Chemistry
The decomposition of hydrogen iodide on a gold surface at 150 oC HI(g) H2(g) + I2(g) is zero order in HI. In one experiment, when the initial concentration of HI was 0.206 M, the concentration of HI dropped to 3.71E-2 M after 898 seconds had passed. Based on these data, ...
March 22, 2014 by kait

chemistry
1) The activation energy of a certain reaction is 35.3 kJ/mol. At 20 degrees C, the rate constant is 0.0130 s^-1. At what temperature would this reaction go twice as fast? Answer in units of degrees Celsius. i think the answer is around 34, but i keep in getting it screwed up...
January 29, 2008 by Evets

chemistry-rate of reaction
The fictitious compound, arrhenium fluoride (AhF), reacts with itself to form a dimer with the formula Ah2F2. The reaction is second order in AhF. The value of the rate constant is 3.59110−3 M−1s−1. What is the initial rate of reaction in a reactor filled ...
December 2, 2012 by Ron

Chemistry
In a given 1st order reaction A ---> products, the initial concentration of A is 0.40 M. What will be the concentration of A after 15 seconds if the half-life of the reaction is 3 seconds? I found the concentration to be 1.25 x 10-2 M But then how do I find the rate ...
February 18, 2013 by Marcus

Chemistry
The fictitious compound, arrhenium fluoride (AhF), reacts with itself to form a dimer with the formula Ah2F2. The reaction is second order in AhF. The value of the rate constant is 4.09110−3 M−1s−1. What is the initial rate of reaction in a reactor filled ...
November 29, 2012 by Odesa

chemistry
The fictitious compound, arrhenium fluoride (AhF), reacts with itself to form a dimer with the formula Ah2F2. The reaction is second order in AhF. The value of the rate constant is 2.59110−3 M−1s−1. What is the initial rate of reaction in a reactor filled ...
November 29, 2012 by mike

chemistry
The fictitious compound, arrhenium fluoride (AhF), reacts with itself to form a dimer with the formula Ah2F2. The reaction is second order in AhF. The value of the rate constant is 5.59110−3 M−1s−1. What is the initial rate of reaction in a reactor filled ...
November 30, 2012 by maliya

Science
The fictitious compound, arrhenium fluoride (AhF), reacts with itself to form a dimer with the formula Ah2F2. The reaction is second order in AhF. The value of the rate constant is 1.09110−3 M−1s−1. What is the initial rate of reaction in a reactor filled ...
December 5, 2012 by Shelly

chemistry
The fictitious compound, arrhenium fluoride (AhF), reacts with itself to form a dimer with the formula Ah2F2. The reaction is second order in AhF. The value of the rate constant is 2.09110−3 M−1s−1. What is the initial rate of reaction in a reactor filled ...
December 8, 2012 by Anonymous

chemistry
The fictitious compound, arrhenium fluoride (AhF), reacts with itself to form a dimer with the formula Ah2F2. The reaction is second order in AhF. The value of the rate constant is 6.091×10−3 M−1s−1. What is the initial rate of reaction in a reactor ...
November 29, 2012 by NIK

chemistry
The fictitious compound, arrhenium fluoride (AhF), reacts with itself to form a dimer with the formula Ah2F2. The reaction is second order in AhF. The value of the rate constant is 6.091×10−3 M−1s−1. What is the initial rate of reaction in a reactor ...
November 29, 2012 by sveta

Chemistry
The rate constant for a certain reaction is = 4.3010−3 s^-1. If the initial reactant concentration was 0.400 M , what will the concentration be after 19.0 minutes? Rate would be first order therefore I used. A=A initial*e^-kt I keep getting .0030 M but supposely I am ...
January 31, 2010 by Joanna

Chemistry
The reaction 2NO2--->2NO+O2 has the rate constant k= 0.68 m-1s-1. If the initial concentration of NO2 is 9.3010−2 M, how long it would take for the concentration to decrease to 2.0010−2 M ? please answer and show the steps
February 9, 2012 by Jeremy

Chemistry!
The rate constant for a certain reaction is k = 5.0010−3 s-1 . If the initial reactant concentration was 0.950 M , what will the concentration be after 8.00 minutes?
February 25, 2009 by Reese

Chemistry
The rate constant for a certain reaction is = 8.0010−3 . If the initial reactant concentration was 0.400 , what will the concentration be after 16.0 minutes?
September 29, 2012 by Dab353

Chemistry
The rate constant for a certain reaction is k=8.9010^−3 s^-1. If the initial reactant concentration was 0.400M, what will the concentration be after 13.0 minutes?
October 22, 2012 by Tasnim

college chem
Determine the rate of consumption of I− if the initial concentration of IO3− was 0.6634 M and decreased to 0.5745 M after 0.3964 hours. Use the reaction below. IO3− + 5I− + 6H+ ↔ 3I2 + 3H2O
February 22, 2014 by hershi

Chemistry
Consider the reaction A ==> B. If the reaction is first-order in A with the initial concentration A being 6.048M, what is the concentration of A after 1.986 seconds if the rate constant is 0.483s-1? Error tolerance: 0.5% Can someone explain how to do this? Thanks ln(Ao/A...
February 6, 2007 by Marisol

Chemistry
The decomposition of hydrogen iodide on a gold surface at 150 oC HI(g) H2(g) + I2(g) is zero order in HI with a rate constant of 1.20E-4 Ms-1. If the initial concentration of HI is 0.575 M, the concentration of HI will be 0.116 M after seconds have passed.
March 22, 2014 by kait

Chemistry
The decomposition of hydrogen iodide on a gold surface at 150 oC HI(g) H2(g) + I2(g) is zero order in HI with a rate constant of 1.20E-4 Ms-1. If the initial concentration of HI is 0.575 M, the concentration of HI will be 0.116 M after how many seconds have passed?
March 22, 2014 by kait

chemistry
In a reaction A to products, ,4.40 min after the reaction is started concentration of A is 0.588M. The rate of reaction at this point is rate= -change in concentration of A/change in time=2.2x10^-2Mmin^-1. Assume that this rate remains constant for a short period of time. A. ...
January 18, 2014 by Temmi

chemistry
The rate constants for a first order decay reaction are found to be: k287.3∘C=1 x 10−4 s−1 k327.4∘C=19.2 x 10−4 s−1 a) Determine the value, in s-1 of k250∘C (b) How long will it take, at 350 ∘C, for the reactant to decay to 1% of...
January 11, 2013 by Anonymous

Chemistry
The rate constants for a first order decay reaction are found to be: k287.3∘C=1 x 10−4 s−1 k327.4∘C=19.2 x 10−4 s−1 (a) Determine the value, in s-1 of k250∘C (b) How long will it take, at 350 ∘C, for the reactant to decay to 1% ...
January 11, 2013 by selly

Chemistry
At a given temperature, a first-order reaction has a rate constant of 3.5 103 s1. How long will it take for the reaction to be 24% complete? A chemical reaction that is first-order in X is observed to have a rate constant of 2.20 102 s1. If the initial concentration of...
November 17, 2014 by Juli

chemistry
The reactant concentration in a second-order reaction was 0.790 after 200 and 8.8010−2 after 740 . What is the rate constant for this reaction?
May 20, 2012 by Anonymous

Chemistry
Determine the rate constant for the following second-order reaction: A=C+2D given that the initial concentration of A is .3 M and that the concentration of C increase to .01 M in 200 seconds. Express the result in terms of the rate law for the loss of A.
March 14, 2014 by Anonymous

Chemistry
Determine the rate constant for the following second-order reaction: A=C+2D given that the initial concentration of A is .3 M and that the concentration of C increase to .01 M in 200 seconds. Express the result in terms of the rate law for the loss of A.
March 16, 2014 by Anonymous

Chemistry
What would be the concentration of dinitrogen pentoxide after 6.00 X 10(2) seconds and how long would it take for the concentration of N2O2 to decrease to 10.0% of its initial value in the following equation... N2O5 to NO2 and O2 initial concentration is 1.65 X 10-2mol/L rate ...
January 20, 2013 by Chris

chem
Butadiene can undergo the following reaction To form a dimer(two butadiene molecules hooked together). 2c4h8---->c8h12. The half life for the reaction at a given temperature is 5.92x10-2 sec. The reaction kinetics are second order. 1. If the initial concentration of c4h8 is...
March 25, 2012 by court

Chemistry
At 2000 ∘C the equilibrium constant for the reaction 2NO(g)←−→N2(g)+O2(g) is Kc=2.4103. The initial concentration of NO is 0.220M . What is the equilibrium concentration of NO? What is the equilibrium concentration of N2? What is the equilibrium ...
June 6, 2015 by Braxten

calculus
The Voltage v , Current I and Resistance R are related by the equation V=IR. Suppose that V is increasing at a rate of 2 volt/sec, while I is decreasing of the rate of 1/5 (amp/sec ). Let t denote time in seconds. Find the rate at which R is changing when V=40volts and 1=2 amp .
November 7, 2014 by Maria

calculus
The Voltage v , Current I and Resistance R are related by the equation V=IR. Suppose that V is increasing at a rate of 2 volt/sec, while I is decreasing of the rate of 1/5 (amp/sec ). Let t denote time in seconds. Find the rate at which R is changing when V=40volts and 1=2 amp .
November 8, 2014 by maria

Chemistry
In a given 1st order reaction A ---> products, the initial concentration of A is 0.40 M. What will be the concentration of A after 15 seconds if the half-life of the reaction is 3 seconds?
February 17, 2013 by Marcus

Chemistry
The fictitious compound, arrhenium fluoride (AhF), reacts with itself to form a dimer with the formula Ah2F2. The reaction is second order in AhF. The value of the rate constant is 8.591x10-3 M-1s-1. What is the initial rate of reaction in a reactor filled with AhF to a ...
December 10, 2012 by Please Help Me!!!!!!!!

chemistry
The following data were obtained at 25 C for the reaction [1+2+2] C2H5Br + OH- C2H5OH + Br- Determine the rate law for the reaction from these data. [C2H5Br] [OH-] Rate 0.150 0.200 4.8 x 10-5 0.300 0.200 9.6 x 10-5 0.450 0.200 14.4 x 10-5 0.300 0.600 28.8 x 10-5 (ii) The ...
February 8, 2012 by ranu

Chemistry
The gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g) 2 NO2(g) + O2(g) is first order in N2O5. During one experiment it was found that when the initial concentration of N2O5 was 0.218 M, the concentration of N2O5 dropped to 2.96E-2 M after 282 s had passed. ...
January 24, 2014 by Breauna

chemistry
HCOOH(aq) <-----> H^+ (aq)+ HCOO^-(aq) The equilibrium constant (Ka) for Reaction 3 at 25 C is 1.80 10−4 mol dm−3. Calculate the equilibrium concentration of hydrogen ions if the concentration of formic acid at equilibrium is 0.00500 mol dm−3
February 10, 2013 by Mark

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.
May 24, 2012 by swa

science
The equilibrium constant (Ka) for Reaction 3 at 25 C is 1.80 10−4 mol dm−3. Calculate the equilibrium concentration of hydrogen ions if the concentration of formic acid at equilibrium is 0.00500 mol dm−3. (Show all of your working and give your answer to ...
February 10, 2013 by Mark

Chemistry
A reaction of the form aA-----products is second-order with a rate constant of 0.225 L/(mol/s). If the initial concentration of A is 0.293 mol/L, what is the molar concentration of A after 35.6 secs?
September 26, 2010 by Yesenia

Chemistry
The reaction 2B--->C + 2D is found to be zero order when run at 990 degrees C. If it takes 3.3X110^2 s for an initial concentration of B to go from 0.50 M to .20 M what is the rate constant for the reaction? what is the half life of the reaction under these conditions?
February 29, 2008 by Lauren

CHEMISTRY
A second-order reaction has a rate constant of 1.65 M1 s1. If the initial reactant concentration is 1.0 M, calculate the time (in seconds) required for the reaction to become 90% complete. i got 0.06734 seconds but thats incorrect i have no idea what i am doing wrong! HELP!!!!
March 28, 2012 by Maya

Chemistry
H6P6: Urbium Oxide First Part of the Question: Urbium (Ur) is an upscale element found in big cities. Its oxide (UrO2) is not very stable and decomposes readily at temperatures exceeding 66∘ C. The figure below shows how the rate of reaction varies with the concentration...
November 29, 2012 by Odesa

CHEMISTRY HELP NEEDED!!
Given info: Reaction: 3A+2B--->2C+D {A] (mol/L) 1.0 10^-2 1.0 10^−2 2.0 10^−2 2.0 10^−2 3.0 10^−2 [B] (mol/L) 1.0 3.0 3.0 1.0 3.0 Rate of appearance of C (mol/L-hr) 0.3010^−6 8.1010^−6 3.2410^−5 1.2010^−6 7.3010^&#...
March 11, 2012 by Kelly

Second order half life
At 100 degrees C , a certain substance undergoes second-order decomposition with a half-life of 26 minutes. If the initial concentration of the substance is 3.910−2M , what is the value of the rate constant at 100degrees C? So I put in (1560seconds) 1/2 = 1/ k (3.910&#...
September 21, 2010 by Sar

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?
February 17, 2013 by Marcus

Chemistry
The following rearrangement reaction is first order: C3H6 CH3CH=CH2 The rate constant for this reaction is 6.7 ~ 10−4. How many minutes will it take for the concentration of C3H6 to drop to 11.75% of its initial value? How do I calculate this step by step. My answer ...
March 20, 2011 by Alex

Chemistry
Given info: A] (mol/L) [B] (mol/L) Rate of appearance of C (mol/L-hr) 1.0 10^-2 1.0 0.3010^−6 1.0 10^−2 3.0 8.1010^−6 2.0 10^−2 3.0 3.2410^−5 2.0 10^−2 1.0 1.2010^−6 3.0 10^−2 3.0 7.3010^−5 Reaction: 3A+2B--->...
March 11, 2012 by Kelly

Bio Help Please
1)How can you indicate that the bacteria have taken up the plasmid? 2)What is the purpose of the LB/amp(-) plate? Should there be bacterial growth on the plate? 3) Why would one compare plates LB/amp (-) and LB/amp (+)?
March 30, 2013 by Melissa

Bio Help Please!!!
1)How can you indicate that the bacteria have taken up the plasmid? 2)What is the purpose of the LB/amp(-) plate? Should there be bacterial growth on the plate? 3) Why would one compare plates LB/amp (-) and LB/amp (+)?
March 31, 2013 by Melissa

Rate Laws
If the initial concentration of AB is 0.210 M, and the reaction mixture initially contains no products, what are the concentrations of A and B after 75 s? The reaction is in the second order: rate=k[AB]^2 The rate constant is k=5.4*10^2 M*s I don't understand how to find A and...
February 20, 2010 by Kyle

Chem8
The decomposition of XY is second-order in XY and has a rate constant of 0.00895 M-1s-1 at a certain temperature. If the initial concentration of XY is 0.194 M, how long (in seconds) will it take for the concentration to decrease to 0.047 M?
May 2, 2011 by Ryan

Chem10
The decomposition of XY is second-order in XY and has a rate constant of 0.00599 M-1s-1 at a certain temperature. If the initial concentration of XY is 0.174 M, how long (in seconds) will it take for the concentration to decrease to 0.054 M?
May 2, 2011 by Ryan

Calculus
Recall that the average velocity between times t1and t2 is calculated using vave = y(t2) − y(t1)/t2 − t1. We are given that y = 14t − 1.86t^2. Evaluating at t = 1, we have y(1) = 14(1) − 1.86(1)2 = 12.14. Thus, the average velocity between times 1 and 1...
October 8, 2011 by Prater

Calc
Recall that the average velocity between times t1and t2 is calculated using vave = y(t2) − y(t1)/t2 − t1. We are given that y = 14t − 1.86t^2. Evaluating at t = 1, we have y(1) = 14(1) − 1.86(1)2 = 12.14. Thus, the average velocity between times 1 and 1...
September 4, 2013 by P

Chemistry
The decomposition of N2O5(g) --> NO2(g) + NO3(g) proceeds as a first order reaction with a half-life of 30.0 seconds at a certain temperature. If the initial concentration [N2O5]0 = 0.400 M, what is the concentration after 120 seconds?
February 17, 2013 by Marcus

chemistry - (Dr. Bob222)
The rate constant for a second order reaction has the value of 2.5 x 103 Lmol1s1. If the initial concentration of reactant is 3.5 molL-1, what will be the molar concentration of the reactant after 2.5 minutes?
April 16, 2014 by Ana

biology
Given the part of the molecule shown below, can the underlined atom participate in a hydrogen bond with an approriate bonding partner? −O−−−H −C−H−− −N−−−H −O−H−− −C−&#...
March 12, 2013 by selly

CHEMISTRY
Urbium (Ur) is an upscale element found in big cities. Its oxide (UrO2) is not very stable and decomposes readily at temperatures exceeding 66∘ C. The figure below shows how the rate of reaction varies with the concentration of UrO2 at 75∘ C. The rate r is in units...
November 29, 2012 by OLEG

chemistry
Urbium (Ur) is an upscale element found in big cities. Its oxide (UrO2) is not very stable and decomposes readily at temperatures exceeding 66∘ C. The figure below shows how the rate of reaction varies with the concentration of UrO2 at 75∘ C. The rate r is in units...
December 1, 2012 by lisa

chemistry ASAP please!!
The reaction of CO(g) + NO(g) is second-order in NO2 and zero-order in CO at temperatures less than 500K. (a) Write the rate law for the reaction. (b) How will the reaction rate change if the NO2 concentration is halved? (c) How will the reaction rate change is the ...
March 15, 2011 by Maria

chemistry
Benzoic acid reacts with water to form the benzoate ion by the following reaction C6H5COOH(aq) + H2O(l) ⇀↽ C6H5COO−(aq) + H3O +(aq) The equilibrium constant for this reaction is 6.4 x 10−5 . In a 0.1 M solution of benzoic acid, what is the concentration...
February 7, 2015 by Anonymous

Algebra
1.Solve 2x = 5x2 for x. A. 2.322 B. 0.431 C. 0 and 2.322 D. 0 and 0.431 2.Which of these is a factor of 2x100 − x7 − 1? A. x B. x − 2 C. x + 1 D. x − 1 3.If P(x) is a polynomial with P(6) = 1.12 and P(5) = 0.6 then which of the following must be true...
May 5, 2012 by nash

Chemistry(Please check)
1) The reaction A + B + C = products has a rate law rate = k times A times C squared. Which of the following will result in an increase in the rate constant for the reaction? #1 - increasing the temperature #2 - adding a catalyst #3 - doubling the concentration of reactant C I...
February 19, 2012 by Hannah

chemistry
What would be the concentration of dinitrogen pentoxide after 6.00 X 10(2) seconds and how long would it take for the concentration of N2O2 to decrease to 10.0% of its initial value in the following equation... N2O5 to NO2 and O2 initial concentration is 1.65 X 10-2mol/L rate ...
January 21, 2013 by Chris

Chemistry
The rate law of a reaction, A-> B+C is given by the expression: Rate=k, where k=0.0113 mol/L min. If the initial concentration of the reactant is 0.225 mol/L, how long does it take for the concentration to decrease to 0.180 mol/L? I know i have to find the order of the ...
September 14, 2010 by James

chemistry
In the presence of a tungsten catalyst at high temperature, the decomposition of ammonia to nitrogen and hydrogen is a zero order process. If the rate constant at a particular temperature us 3.7x10^-6 mol. How long will it take for an ammonia concentration to drop from an ...
March 26, 2012 by court

AP CHEMISTRY
A voltaic cell is constructed that uses the following half-cell reactions. Cu+(aq) + e− -> Cu(s) I2(s) + 2 e− -> 2 I−(aq) The cell is operated at 298 K with [Cu+ ] = 2.7 M and [I− ] = 2.7 M. (a) Determine E for the cell at these concentrations. (b...
April 6, 2012 by MIKE

AP CHEMISTRY
A voltaic cell is constructed that uses the following half-cell reactions. Cu+(aq) + e− -> Cu(s) I2(s) + 2 e− -> 2 I−(aq) The cell is operated at 298 K with [Cu+ ] = 2.7 M and [I− ] = 2.7 M. (a) Determine E for the cell at these concentrations. (b...
April 14, 2012 by DAN

chemistry
20 mL of 0.125 M potassium iodide solution is mixed with 10 mL of 0.1 g L1 sodium thiosulfate solution and 0.2 g of solid iodine indicator is added. To this solution is added 20 mL of 0.025 M peroxodisulfate solution. After 46 seconds a blue colour appears, indicating that ...
May 9, 2014 by dan

biology
Which bacterial plates control for: 1) If the E. coli cells were transferred correctly: 2) If the E. coli cells can grow on LB: 3) If the Ampicillin is working correctly: 4) If the stock E. coli cells were contaminated with plasmid: Possible choices for each number are: "-"...
July 18, 2009 by Jenn

ap chem
Under certain conditions, the reaction 3 A + 4 B → 5 C is observed to proceed at a rate of 0.0106 M s−1. What is the corresponding rate of change in product C? 1. 0.0318 M s−1 2. 0.0106 M s−1 3. 0.00353333 M s−1 4. −0.00212 M s&#...
October 30, 2014 by john

chemistry
The reaction A -> B + C is 1st order w/ respet to A. It's rate const k is equal to 0.343 M/s at 273K. The initial concentration of A was 0.399 M. Calculate the concentration of B after 0.185 secs have passed.
February 18, 2012 by bernard

Chemistry
For the following reaction 2NO2 -> 2NO +O2 is second order reaction. If the initial concentration of NO2 is 0.098M and the initial rate of disappearance is 2.72e-3 M/sec , what is the value of the rate constant?
February 9, 2015 by Cole

chemistry
The reaction Cl(g)+ O3(g) --> ClO(g)+ O2(g) is the first-order in both reactants. Determine the pseudo-first-order and second-order rate constants for the reaction from the data in the table below if the initial ozone concentration was ..0000000000825 M or 8.25*10^-11 M. ...
October 15, 2012 by Brun

chemistry
The reaction Cl(g)+ O3(g) --> ClO(g)+ O2(g) is the first-order in both reactants. Determine the pseudo-first-order and second-order rate constants for the reaction from the data in the table below if the initial ozone concentration was ..0000000000825 M or 8.25*10^-11 M. ...
October 15, 2012 by Brun

Chem2
A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C. If the concentration of C is increased by a factor of 4.95 (and all other concentrations are held constant), how much will the rate of reaction increase?
May 2, 2011 by Ryan

Chemistry
Calculate the half-life (in s) of a first-order reaction if the concentration of the reactant is 0.0655 M 18.4 s after the reaction starts and is 0.0173 M 41.2 s after the reaction starts. I got 25.6 Suppose the half-life is 23.7 s for a first order reaction and the reactant ...
January 31, 2013 by Anonymous

Chemistry
In a reversible reaction, chemical equilibrium is attained when ? 1. Rate of the forward reaction is greater than the rate of the reverse reaction. 2. Rate of the reverse reaction is greater than the rate of the forward reaction, 3. Concentration of the reactants reaches zero ...
March 9, 2011 by Jazmin F.

chem
The rate data from a chemical reaction shows that doubling the concentration of A with the concentration of B remaining constant causes the rate to increase by a factor of four. What is the reaction order for [A]? a. 0 b. 0.5 c. 1 d. 2 e. 3
February 10, 2008 by Anonymous

MATH
what is a constant rate of change? That means the velocity changes over time in the same manner. 4,800 +3,700 =4,500 Rate of Change Is Constant You can increase or decrease the amount or concentration of a species by a constant value using a zero order rule. For example, the ...
January 9, 2007 by Austin

Chemistry
Determine the rate constant for each of the following first-order reactions. In each case, write the rate law for the rate of loss of A. (a) 2 A B + C, given that the concentration of A decreases to one-fourth its initial value in 57 min (b) 2 A B + C, given that A0 = 0.036 ...
June 28, 2013 by Sara

Chemistry
Cyclopropane is converted to propene in a first-order process. The rate constant is 5.4 10-2 hr-1. If the initial concentration of cyclopropane is 0.150 M, what will its concentration be after 22.0 hours?
December 10, 2009 by Ericka

Concentration and Reaction
The rate of the following reaction: Radioactive decay of 90Sr, is characterized by the rate constant k = 0.024 year-1. What is the half-life (in years) for this reaction at the same conditions when the initial concentrations are 0.0356 M? (Round your answer to 3 significant ...
November 20, 2010 by Confused

Chemistry
A reaction of the form aA---> Products is second order with a rate constant of 0.169 L/(mol*s). If the intial concentration of A is 0.159 mol/L, how many seconds would it taje for the concentration of A to decrease to 6.07X10^-3 mol/L
February 23, 2008 by Sam

Chemisty
A reaction of the form aA---> Products is second order with a rate constant of 0.169 L/(mol*s). If the intial concentration of A is 0.159 mol/L, how many seconds would it taje for the concentration of A to decrease to 6.07X10^-3 mol/L
February 24, 2008 by Sam

calculus-changing voltage
V = IR V is increasing at the rate of 1 volt/sec while I is decreasing at the rate of 1/3 amp/sec. Let t = time in sec What is dV/dt? What is dI/dt? Find the rate at which R is changing when V = 12 volts and I = 2 amp. Thanks. Please ignore this. I got the answer.
December 9, 2006 by Jen

Chemistry
Cyclopropane, C3H6, is converted to its isomer propylene, CH2=CHCH3, when heated. The rate law is first order in cyclopropane, and the rate constant is 6.0 10^-4 /s at 500C. If the initial concentration of cyclopropane is 0.0238 mol/L, what is the concentration after 719 s?
February 7, 2012 by Keigan

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)...
November 18, 2010 by ben

Chemistry(Please check)
The initial concentration of a reactant in a first order reaction is 0.620 molar. What will be its concentration after 3 half-lives? I did 0.620 -> 0.31 ->0.155 0.155M will be the concentration. Is this correct?
February 19, 2012 by Hannah

Physics
A 60 watt light bulb in a household circuit at 120 V carries a current of 0.500 amp. (An amp was defined in class as a way to measure charge movement. One amp is one coulomb per second.) How many electrons move through this light bulb in five minutes?
March 7, 2011 by Anonymous

physics
Four charges −8 10^−9 C at (0 m, 0 m), −7 10^−9 C at (5 m, 1 m), −1 10^−9 C at (−2 m, −3 m), and 2 10^−9 C at (−2 m, 4 m), are arranged in the (x, y) plane as shown. Find the magnitude of the resulting force ...
January 29, 2014 by sarah

Chemistry
The rate constant for a second-order reaction is 0.54 M-1s-1. What is the half-life of this reaction if the initial concentration is 0.27 M
December 9, 2014 by anonymous.

chemistry
The rate constant for the following equation is 0.00454 M−1 s −1 . We start with 0.134 mol C2F4 in a 4 liter container, with no C4F8 initially present. 2 C2F4 → C4F8 What will be the concentration of C2F4 after 2 hours? Answer in units of M.
May 8, 2015 by Anonymous

chemistry
If it takes 30 seconds for a reactant concentration to decrease from 1.0 M to 0.5 M in a first-order chemical reaction, then what is the rate constant for the reaction? A. 43 s1 B. 0.046 s1 C. 0.023 s1 D. 0.033 s1
March 25, 2015 by Cortney

chemistry
calculate the half-life of a first- order reaction if the concentration of the reactant is 0.0396 M at 12 seconds after the reaction starts and is 0.00579 M at 47 after the reaction starts. How long does it take for the reactant concentration to decrease to 0.00269 M
November 18, 2011 by saud

chemistry
calculate the half-life of a first- order reaction if the concentration of the reactant is 0.0396 M at 12 seconds after the reaction starts and is 0.00579 M at 47 after the reaction starts. How long does it take for the reactant concentration to decrease to 0.00269 M
November 18, 2011 by saud

math
(4 − 2x)−2 x=-2 y=4 z=-3 how do you solve this? i have solved it and gotten 6 for my answer many times and it says it's wrong. other equations are (y − z)−3 and (x − 5y)0. i cant get them right
March 1, 2012 by krysta

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