Question

1) Use the integrated rate law to calculate the concentration of tert-butyl chloride at t =...

1) Use the integrated rate law to calculate the concentration of tert-butyl chloride at t = ( 1.5) X (half life) if half life is 23.5 seconds

2) Explain why the rate can't be determined simply examining the balanced equation?

3) propose an experiment to determine the activation energy of this reaction

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

2. rate can not be determined simply examining the balanced equation becoz , rate of a reaction is dependent on time and concentration. from balanced chemical equation we never get any information about reaction time , so for this reason rate can not be determined simply examining the balanced equation .

3. We have to do an experiment where we have to find different rate constant for a reaction at two different temperature , then when we get this we will have to put the known equation ,

ln (K2/K1) = - (Ea/RT) ( T1-T2/T1T2)

we know here all the parameter except the Ea which is activation energy .

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The integrated rate law allows chemists to predict the reactant concentration after a certain amount of...
The integrated rate law allows chemists to predict the reactant concentration after a certain amount of time, or the time it would take for a certain concentration to be reached. The integrated rate law for a first-order reaction is: [A]=[A]0e−kt Now say we are particularly interested in the time it would take for the concentration to become one-half of its initial value. Then we could substitute [A]02 for [A] and rearrange the equation to: t1/2=0.693k This equation calculates the time...
The integrated rate law allows chemists to predict the reactant concentration after a certain amount of...
The integrated rate law allows chemists to predict the reactant concentration after a certain amount of time, or the time it would take for a certain concentration to be reached. The integrated rate law for a first-order reaction is: [A]=[A]0e−kt Now say we are particularly interested in the time it would take for the concentration to become one-half of its inital value. Then we could substitute [A]02 for [A] and rearrange the equation to: t1/2=0.693k This equation caculates the time...
Integrated Rate Laws: Working with First Order Reactions When formic acid is heated, it decomposes to...
Integrated Rate Laws: Working with First Order Reactions When formic acid is heated, it decomposes to give hydrogen and carbon dioxide. This first order decay is shown below: HCOOH (g) → CO2 (g) + H2 (g) At 535.0° C, the half life for this reaction is 23.5 min. How many seconds are needed for the initial concentration of HCOOH to decrease by a factor of 10? seconds
Learning Goal: To understand how to use integrated rate laws to solve for concentration. A car...
Learning Goal: To understand how to use integrated rate laws to solve for concentration. A car starts at mile marker 145 on a highway and drives at 55 mi/hr in the direction of decreasing marker numbers. What mile marker will the car reach after 2 hours? This problem can easily be solved by calculating how far the car travels and subtracting that distance from the starting marker of 145. 55 mi/hr×2 hr=110 miles traveled milemarker 145−110 miles=milemarker 35 If we...
1.If the rate law for the clock reaction is: Rate = k [ I-] [ BrO3...
1.If the rate law for the clock reaction is: Rate = k [ I-] [ BrO3 -] [H+] A clock reaction is run with the following initial concentrations: [I-] [BrO3-] [H+] [S2O32-]                                                                                                    0.002 0.008 0.02 0.0001 The reaction time is 25.4 seconds Calculate k in the rate law. A clock reaction is run at 18 ºC with the following initial concentrations [I-]               [BrO3-]            [H+]                         [S2O32-] 0.002                  0.008              0.02                          0.0001   Then the experiment is...
1) If the rate law for the clock reaction is:     Rate = k [ I-]...
1) If the rate law for the clock reaction is:     Rate = k [ I-] [ BrO3-] [H+] A clock reaction is run with the following initial concentrations: [I-]               [BrO3-]            [H+]                         [S2O32-] 0.002                   0.008                   0.02                          0.0001   The reaction time is 29 seconds Calculate k in the rate law: 2)If the rate law for the clock reaction is:     Rate = k [ I-] [ BrO3-] [H+] A clock reaction is run...
1)A second order reaction has a rate constant of 3.7 M-1min-1. if the initial concentration of...
1)A second order reaction has a rate constant of 3.7 M-1min-1. if the initial concentration of the reactant is 0.0100M, what is the concentration remaining after 15 min? a) .0099M b) .0056M c) .0025M d) .0064M 2) the rate constant for the first order decomposition of A at 500 degrees Celsius is 9.2 x 10 to the negative 3rd powers s-1. How long will it take for 90.8 % of a 0.500M sample of A to decompose a) 2.5 x...
Rate Law: Iodination of Acetone Experiment X trial   initial [A] initial [B] Rate (M/s) #1    1.00...
Rate Law: Iodination of Acetone Experiment X trial   initial [A] initial [B] Rate (M/s) #1    1.00 x 10-3 0.25 x 10-3 0.26 x 10-9 #2   1.00 x 10-3 0.50 x 10-3 0.52 x 10-9 #3   1.00 x 10-3 1.00 x 10-3 1.04 x 10-9 #4    2.00 x 10-3 1.00 x 10-3 4.16 x 10-9 #5    3.00 x 10-3 1.00 x 10-3 9.36 x 10-9 #6    4.00 x 10-3 1.00 x 10-3 16.64 x 10-9 Determine the rate law and calculate...
The first-order decomposition of a colored chemical species, X, into colorless products is monitored with a...
The first-order decomposition of a colored chemical species, X, into colorless products is monitored with a spectrophotometer by measuring changes in absorbance over time. Species X has a molar absorptivity constant of 5.00x103 cm–1M–1 and the path length of the cuvette containing the reaction mixture is 1.00 cm. The data from the experiment are given in the table below. [X] (M) Absorbance (A) Time (min) ? 0.600 0.0 4.00 x 10-5 0.200 35.0 3.00 x 10-5 0.150 44.2 1.50 x...
1. Which of the following balanced molecular equations represent reactions for which the rate law expression...
1. Which of the following balanced molecular equations represent reactions for which the rate law expression could likely be determined via time to turbidity determinations? Select all that apply. a. 3 SrCl2 (aq) + 2 Li3PO4 (aq) ---> Sr3(PO4)2 (s) + 6 LiCl (aq) b. 2 HBr (aq) + Ca(OH)2 (aq) ---> 2 H2O (l) + CaBr2 (aq) c. FeS (s) + HCl (aq) ---> FeCl2 (aq) + H2S (g) d. 2 NO (g) + 5 H2 (g) ---> 2...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT