Use the concentration and rate data presented in the table below to answer the f
ID: 791535 • Letter: U
Question
Use the concentration and rate data presented in the table below to answer the following questions about the hypothetic reaction:
A + 2B + 4C --> 2D + E
Line
[A] (Mol/L)
[B] (mol/L)
[C] (mol/L)
Rate (mol/L.s)
1
0.100
0.100
0.100
3.6 x 10-2
2
0.200
0.100
0.100
3.6 x 10-2
3
0.100
0.200
0.100
7.2 x 10-2
4
0.200
0.200
0.200
2.9 x 10-1
5
0.300
0.200
0.300
?
a) Based on the overall reaction, why is this a multi-step reaction?
b) What is the order of the reaction, respective to each reactant?
c) What is the overall order of the reaction?
d) What is the rate law equation?
e) How does the rate law equaiton justify that this reaction is a multi-step reaction?
f) Predict the rate for the "?"
g) Propose a reaction mechanism using the criteria presented in the lesson, with the third step as a rate-determining step.
h) Draw a potential energy diagram to illustrate this reaction mechanism, assuming that the overall reaction is endothermic. Label reaction intermediates with "R"I and activated complexes with "AC."
Line
[A] (Mol/L)
[B] (mol/L)
[C] (mol/L)
Rate (mol/L.s)
1
0.100
0.100
0.100
3.6 x 10-2
2
0.200
0.100
0.100
3.6 x 10-2
3
0.100
0.200
0.100
7.2 x 10-2
4
0.200
0.200
0.200
2.9 x 10-1
5
0.300
0.200
0.300
?
Explanation / Answer
from 1 to 2, we note that {A] has no effect on rate
from 1 to 3, we note that doubling [B] doubles the rate.... FIRST ORDER RELATIONSHIP
from 3 to 4, doubling [C] , quadrupled the rate.... SECOND ORDER
===============================
from 3 to 5, we fund that they cahnged [A] which has no effect
but because they tripled [C]
[3X's]^2 = should be 9 times faster
so
9X's faster than #3 =
6.48 e-1
so the rate for #5, rounded to 2 sig figs is 6.5 X 10^-1
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.