Question

For the reaction A + B → C the following data is obtained:

Trial | [A] | [B] | Rate_{A} |

1 | 0.2 M | 0.2 M | 1.2 x 10^{-3} M/min |

2 | 0.1 M | 0.2 M | 6.0 x 10^{-4} M/min |

3 | 0.2 M | 0.1 M | 1.2 x 10^{-3} M/min |

After you determine the rate law, what is the value of the rate
constant for the reaction using the given units? If you choose to
enter your answer in scientific notation you must enter it this way
1.2E-3 for 1.2 x 10^{-3}.

Answer #1

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....

For the reaction
A + 2 B + C → 3 D + 2 F
the following experimental data were obtained.
Experiment
[A] (M)
[B] (M)
[C] (M)
Rate (M/min)
1
0.10
0.10
0.10
2.0 x 10-5
2
0.10
0.10
0.30
6.0 x 10-5
3
0.20
0.10
0.10
8.0 x 10-5
4
0.10
0.40
0.10
2.0 x 10-5
Part #1:
Which represents the correct rate law?
A) Rate = k
[A]0[B]2[C]
B) Rate = k
[A]2[B]0[C]
C) Rate = k...

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

Determine the rate law, including the values of the orders and
rate law constant, for the following reaction using the
experimental data provided.
Q + X --> products
Trial
[Q]
[X]
Rate
1
0.12 M
0.10 M
1.5 x 10-3 M/min
2
0.24 M
0.10 M
3.0 x 10-3 M/min
3
0.12 M
0.20 M
1.2 x 10-2 M/min

1.) 2A → B + C
The above reaction is run and found to follow second order
kinetics with a rate constant of 1.30 x 10-3
M-1sec-1. If the initial concentration of A
is 1.33 M, what is the concentration after 164 seconds?
2.) 2A → B + C
Two trials of the above reaction are run with the same initial
concentration of A. The first trial is performed at 25oC
and the second at 35oC. If the rate constant...

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...

3. A certain reaction has the following general form: 2A > B
Concentration vs time data were collected for this reaction, at
50°C and an initial concentration of 0.0200 M. It is determined
that a plot of ln[A] vs. time resulted in a straight line with a
slope value of - 2.97 X 10-2 min-1.
A. Write the rate law.
B. Write the integrated rate law
C. What is k for this reaction (or what is the rate constant for...

Using the given data, calculate the rate constant of this
reaction: A+B ---> C+D
Trial
[A] (M) [B}
(M)
Rate (M/s)
1
0.230
0.330
0.0170
2
0.230
0.792
0.0979
3
0.276 0.330
0.0204

using the given data, calculate the rate constant of this
reaction. A+B yields C+D Trial: 1,2,3 [A](M): 0.370, 0.370, 0.592
[B](M):0.340, 0.782, 0.340 Rate(M/s): 0.0210, 0.111, 0.0336 K= ?
Please provide the units as well. Please show work so I can
understand the problem.

Given the data below for the reaction, 2 A + 2 B + 4 C => D +
E + 3 F,
Experiment
Initial conc of A, mol/L
Initial conc of B, mol/L
Initial conc of C, mol/L
Initial rate, mol/L.s
1
0.1
0.2
0.4
2 x 10-3
2
0.2
0.2
0.4
8 x 10-3
3
0.3
0.4
0.4
1.8 x 10-2
4
0.4
0.6
0.2
1.6 x 10-2
Calculate the value of k to 3 significant figures

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