Using experimental results to determine the order of a chemical reaction and the rate constant from your understanding of chemical kinetics and species half life.

A reaction is defined by the following scheme:

X à Y

When the concentration of X in a solution is 1.02 M, the half-life (t1/2) is 160 seconds.

When the concentration of X in solution is 2.05 M, the half-life (t1/2) is 80 seconds.

The above information applies when the reaction takes place at 25 degrees Celsius.

(a) What is the order of the reaction?
(b) Calculate the rate constant for the reaction.

Solution Preview

Please note that the attached file contains a complete solution to the question.

PART ONE: What is the order of the reaction?
To answer this question, we will consider the equations used to calculate half-life (t1/2) for zero order, first order, and second order reactions. In each case, [X]o=concentration of X at time zero; k = rate constant.
For a zero order reaction, t1/2 = [X]o/(2k)
For a first order reaction, t1/2 = 0.693/k
For a second order reaction, t1/2 = (k*[X]o)-1
Considering the equations shown above, it is clear that for a first order reaction, the half-life is independent of the ...

1) Explain the concept of chemicalkineticsandthe various factors that influence reaction states.
2) Relate experimental measurements to reactionrates andtherate laws.
3) Determinetheorder of reaction, therate law, therateconstant, andtherate of concentrations.
4) Solve first-orderrate problems.

After applying 2,4-D to turf, an experiment was conducted measuring the concentration of 2,4-D that was present over time. The 2,4-D concentration was 80 ppm on day zero, 45 ppm on day 14, and 6 ppm on day 56.
a. Do a first order kinetic plot to determinetherateconstant for the disappearance of 2,4-D.
b. What is thehalf

Thereaction A produces B + C is known to be zero order in A and to have a rateconstant of 5.0 x 10 superscript-2 mol/L x sec. @ 25 degrees C. An experiment was run at 25 degrees C where [A]0 = 1.0 x 10 superscript-3 M.
a) Write the integrated law for this reaction
b) Calculate thehalf-life for this reaction
c) Calculate

Question:
CA [mm] 4.40 3.55 2.98 2.57 2.26 2.01 1.81 1.65
t [s] 0 100 200 300 400 500 600 700
Use the method of half-life to find theorderandtheconstant of speed.

The 1st order composition of hydrogen peroxide has a rateconstant of 7.30 X 10-4 s^-1 at 25 degrees C. Determinethe percent of hydrogen peroxide that has decomposed after the first 500 seconds?
Since I do not have the initial concentration, I was going to use thehalf life equation and take the percentage of that. The miss

Please can you provide an explanation for the following questions:
For therate law, Rate = k[A]2[B], which of the following is false about thechemicalreaction having this rate law?
A) Doubling [A] quadruples therate.
B) Thereaction is third order overall.
C) Thechemicalreaction must be: 2 A + B â?' C.
D) Do

In an aqueous solution, glucose decomposed according to theresults shown below.
(a) Demonstrate that thereaction is first order.
(b) Calculate therateconstant for the decomposition process.
(c) Calculate thehalf-life (t1/2) for glucose under the specified conditions.
Glucose decomposition results:
Time (min), Glucose

See the attached file.
1. Now consider the following reactionand data:
H 2 +2BrCl→2HCl+Br 2
Time (s)
Br 2 concentration (M)
5 1.35
15 1.65
Part A
What is the average rate of formation of Br 2 ?Express your answer to three decimal places and include the appropriate units.
2. Consider thereaction: A(g)+1 2 B(

Knowing therateconstant is 3.46 X 10^-5 s^ at 298 and that energy activation is 1.60 x 10^5 J-mol ^-1. Determinethe temperature at which thehalf life for the 1st order decomposition of dinitrogen pentoxide in carbon tetrachloride to dinitrogen tetroxide and oxygen is 2 hours.