Question

The following data were obtained at 25C for a reaction:

aA + bB = cC

Initial Concentrations Initial Reaction Rate

Reaction [A] [B] M/s or mol/Ls

1 0.100 M 0.200 M 5.00x10^-4

2 0.150 M 0.200 M 7.50x10^-4

3 0.150 M 0.600 M 6.75x10^-3

What is the order of the reaction with respect to A?

What is the order of the reaction with respect to B?

What is the rate constant, k, for the reaction?

Answer #1

Learning Goal: To understand reaction order and rate constants.
For the general equation aA+bB?cC+dD, the rate law is expressed as
follows: rate=k[A]m[B]n where m and n indicate the order of the
reaction with respect to each reactant and must be determined
experimentally and k is the rate constant, which is specific to
each reaction. Order For a particular reaction, aA+bB+cC?dD, the
rate law was experimentally determined to be
rate=k[A]0[B]1[C]2=k[B][C]2 This equation is zero order with
respect to A. Therefore, changing...

Consider the following reaction and associated equilibrium
constant: aA(g)+bB(g)⇌cC(g), Kc = 3.0 Part A Find the equilibrium
concentrations of A, B, and C for a=1, b=1, and c=2. Assume that
the initial concentrations of A and B are each 1.0 M and that no
product is present at the beginning of the reaction. Express your
answer using two significant figures. Enter your answers separated
by commas. [A], [B], [C] = m M

Consider the following reaction and associated equilibrium
constant: aA(g)+bB(g)⇌cC(g), Kc = 5.0
a.) Find the equilibrium concentrations of A, B, and C for
a=1, b=1, and c=2. Assume that the
initial concentrations of A and B are each 1.0 M and that no
product is present at the beginning of the reaction.
Express your answer using two significant figures. Enter your
answers separated by commas.
b.) Find the equilibrium concentrations of A, B, and C for
a=1, b=1, and c=1....

Using the initial rates of reaction for the following
reaction:
A + 3B → 2C
[A] (mol/L)
[B] (mol/L)
Initial Rate (mol/L∙s)
0.210
0.150
3.41x10-3
0.210
0.300
1.36x10-2
0.420
0.300
2.73x10-2
What is the order of the reaction with respect to A?
What is the order of the reaction with respect to B?
The overall rate expression?___________________
Calculate the rate constant including the units.

Consider the following reaction and associated equilibrium
constant: aA(g)⇌bB(g), Kc = 2.1
A. Find the equilibrium concentrations of A and B for
a=1 and b=1. Assume that the initial
concentration of A is 1.0 M and that no B is present at the
beginning of the reaction.
[A], [B] =?
B. Find the equilibrium concentrations of A and B for
a=2 and b=2. Assume that the initial
concentration of A is 1.0 M and that no B is present at...

Consider the following reaction and associated
equilibrium constant:
aA(g)⇌bB(g),
Kc = 3.8
PART A
Find the equilibrium concentrations of A and B for a=1 and
b=1. Assume that the initial concentration of A is 1.0 M
and that no B is present at the beginning of the reaction.
PART B
Find the equilibrium concentrations of A and B for a=2 and
b=2. Assume that the initial concentration of A is 1.0 M
and that no B is present at the...

The following data were obtained for the chemical reaction: A +
B ---> products
Exp.
Initial A
(mol/L)
Initial B
(mol/L)
Init. Rate of Formation
of products (M s-1)
1
0.040
0.040
9.6 x 10-6
2
0.080
0.040
1.92 x 10-5
3
0.080
0.020
9.6 x 10-6
(a) Determine the rate law for this reaction.
(b) Find the rate constant.
(c) What is the initial rate of reaction when [A]o =
0.12 M and [B]o = 0.015

For the reaction, A(g) + B(g) => 2 C(g), the following data
were obtained at constant temperature.
Experiment
Initial [A], mol/L
Initial [B], mol/L
Initial Rate, M/min
1
0.10
0.10
2 x 10-4
2
0.30
0.30
5.4 x 10-3
3
0.10
0.30
1.8 x 10-3
4
0.20
0.40
6.4 x 10-3
Which of the following is the correct rate law for the
reaction?
1.
Rate = k[A][B]
2.
Rate = k[A]2[B]
3.
Rate = k[A]2[B]2
4.
Rate = k[A]
5....

Determine (a) the rate equation and (b) the rate constant for
the hypothetical reaction A + B C given the following initial
concentrations and initial rate data. Run # (1) (2) (3) [A]0
(mol/L) 0.100 0.100 0.200 [B]0 (mol/L) 0.100 0.200 0.200 Initial
Rate (mol/L·s) 0.18 0.36 1.44

For the following combination reaction,
2 NO2(g) + F2(g) = 2 NO2F(g)
The initial rates of this reaction were determined for several
concentrations of the reactants. All of the data is summarized via
the following table:
Experiment
[NO2] (M)
[F2] (M)
Rate (M/s)
1
0.100
0.100
0.026
2
0.200
0.100
0.051
3
0.200
0.200
0.103
4
0.400
0.400
0.411
a) Determine the rate law for this reaction based on the data
above.
b) Calculate the rate constant, with appropriate units.

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