Question

What is the rate constant for a reaction based on the following experimental information?

Experiment | Rate (M/s) | [A] (M) | [B] (M) | [C] (M) |

1 | 1.444 | 0.27 | 0.75 | 0.8 |

2 | 1.444 | 0.459 | 0.75 | 0.8 |

3 | 1.4584 | 0.27 | 1.35 | 0.8 |

4 | 1.4584 | 0.459 | 0.75 | 3.28 |

Answer #1

First we have to write the rate equation = Rate =
k[A]^{m}[B]^{n}[C]^{p}

Let us find the order of the reaction then we can find Rate constant,k

From the table

Take (1) and (2) rows and plug in those values in the rate equation as shown below

here we cancel like terms

Here 1 can also be written as (1.7)^{0}

m=0

Order with respect to [A] = 0

Now take rows (1) and (3) to find the order of [B]

here we cancel like terms

here 1.01 which is almost 1

n=0

Order of the reaction with respect to [B] = n= 0

Let us take rows (2) and (4)

here we cancel like terms

p=0

Order of the reaction with respect to [C] = p =0

Now let us find the rate constant, k by plugging the any row values into reate equation

Rate = k[A]^{m}[B]^{n}[C]^{p}

Here i am taking first row values

1.444 =
k[0.27]^{0}[0.75]^{0}[0.8]^{0}

1.444 = k

Rate constant k = 1.444 M/s

What is the rate constant for a reaction based on the following
experimental information?
Experiment
Rate (M/s)
[A] (M)
[B] (M)
[C] (M)
1
0.4416
0.6
0.58
0.54
2
1.9672
1.26
0.58
0.54
3
0.4549
0.6
1.856
0.54
4
5.857
1.26
0.58
1.674

What is the rate constant for a reaction based on the following
experimental information?
Experiment
Rate (M/s)
[A] (M)
[B] (M)
1
0.1172
0.32
0.56
2
0.3389
0.544
0.56
3
0.1741
0.32
0.84

What is the rate constant for a reaction based on the following
experimental information?
Experiment
Rate (M/s)
[A] (M)
[B] (M)
1
1.4125
0.73
0.38
2
2.7685
1.46
0.38
3
1.3984
0.73
1.178

What is the rate constant for a reaction based on the following
experimental information?
Experiment
Rate (M/s)
[A] (M)
[B] (M)
1
0.7082
0.39
0.39
2
1.216
0.663
0.39
3
0.694
0.39
0.897

Answer the following based on the reaction. At 313 K, the rate
constant for this reaction is 1.09×102 /s and at 564 K the rate
constant is 6.62×106 /s.
cyclopentane → 1-pentene
1. Determine the activation energy (EA) (in kJ/mol) for this
reaction.
2. Determine the pre-exponential factor, A (in /s) for this
reaction.
3. Determine the rate constant (in /s) for this reaction at 1218
K.

Based on the kinetic data below, what is the rate constant for
this reaction?
A + 2 B => C
[A], mol/L
[B], mol/L
Initial Rate, mol L-1 s-1
1.0 x 10-4
2.0 x 10-4
0.276
2.0 x 10-4
1.0 x 10-4
0.069
1.0 x 10-4
1.0 x 10-4
0.069
Based on the kinetic data below, what is the rate constant for
this reaction?
A + 2 B => C
[A], mol/L
[B], mol/L
Initial Rate, mol L-1 s-1
1.0...

With the experimental data given for the kinetic study of the
reaction
A + 2B == AB2, answer the following two questions
Experiment [A] 0 M [B] 0 M Initial velocity formation rate of
AB2 (M / min)
1 0.5 1.5 4.2x10-3
2 1.5 1.5 1.3x10-2
3 3.0 3.0 5.2 x10-2
11.-Determine the law of speed for the reaction
Answer: ___________________________
12.- Calculate the value of the kinetic constant
Answer: __________________

Question # 3: Algorithmic Questions.
A. A particular first-order reaction has a rate constant of 1.35
×102 s-1 at 25.0 °C. What is the magnitude of k at 75.0 °C if Ea =
85.6 kJ/mole?
B. The rate constant for a second-order reaction is 0.13 M-1s-1.
If the initial concentration of reactant is 0.26 mole/L, how much
it will take for the concentration to decrease to 0.13 mole/L?

For a first-order reaction, the half-life is constant. It
depends only on the rate constant k and not on the reactant
concentration. It is expressed as t1/2=0.693k For a second-order
reaction, the half-life depends on the rate constant and the
concentration of the reactant and so is expressed as
t1/2=1k[A]0
Part A
A certain first-order reaction (A→products) has a rate constant
of 4.20×10−3 s−1 at 45 ∘C. How many minutes does it take
for the concentration of the reactant, [A],...

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...

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