Question

Ethyl chloride vapor decomposes by the first-order reaction C2H5Cl→C2H4+HCl The activation energy is 249 kJ/mol and the frequency factor is 1.6×1014s−1

The value of the specific rate constant at 720 K is k= 1.4x10^-4 s^-1

1) Find the fraction of the ethyl chloride that decomposes in 19 minutes at this temperature.

2) Find the temperature at which the rate of the reaction would be twice as fast.

Answer #1

1) For a first order reaction,

ln[A] = ln[Ao] - kt

[A] = fraction of ethyl chloride remaining

[Ao] = initial concentration of ethyl chloride

k = 1.4 x 10^-4 s-1

t = 19 x 60 = 1140 s

Feed values,

ln([A]/[Ao]) = -1.4 x 10^-4 x 1140

[A]/[Ao] = 0.852

fraction of ethyl alcohol decomposed = 1 - 0.852 = 0.148

2) Temperature at which rate would be twice fast

ln(k2/k1) = Ea/R[1/T1 - 1/T2]

k2/k1 = 2

Ea = 249 kJ/mol

R = gas constant

T1 = 720 K

T2 = ?

we get,

ln(2) = 249000/8.314 (1/720 - 1/T2)

T2 = 732.20 K

Is the temperature required

Ethyl chloride vapor decomposes by the first-order reaction
C2H5Cl→C2H4+HCl The activation energy is 249 kJ/mol and the
frequency factor is 1.6×1014s−1.
Find the fraction of the ethyl chloride that decomposes in 19
minutes at this temperature.
Express your answer using one significant figure.

Find the temperature at which the rate of the reaction would be
twice as fast.Ethyl chloride vapor decomposes by the first-order
reaction
C2H5Cl→C2H4+HCl
The activation energy is 249 kJ/mol and the frequency factor is
1.6×1014s−1.
Part A Find the value of the specific rate constant at 700 K
.
Part B
Find the fraction of the ethyl chloride that decomposes in 20
minutes at this
temperature.[C2H5Cl]0−[C2H5Cl]t[C2H5Cl]0[C2H5Cl]0−[C2H5Cl]t[C2H5Cl]0
Part C= Find the temperature at which the rate of the reaction
would be...

The activation energy of a certain reaction is 35.1 kJ/mol . At
25 ∘C , the rate constant is 0.0160s−1. At what temperature in
degrees Celsius would this reaction go twice as fast?
Given that the initial rate constant is 0.0160s−1 at an initial
temperature of 25 ∘C , what would the rate constant be
at a temperature of 200. ∘C for the same reaction
described in Part A?

1.a)The activation energy of a certain reaction is 46.3 kJ/mol .
At 30 ∘C , the rate constant is 0.0180s−1. At what temperature in
degrees Celsius would this reaction go twice as fast?
b) Given that the initial rate constant is 0.0180s−1 at an
initial temperature of 30 ∘C , what would the rate constant be at a
temperature of 140 C for the same reaction described in Part A?

A)The activation energy of a certain reaction is 33.8 kJ/mol .
At 30 ∘C , the rate constant is 0.0170s−1. At what
temperature in degrees Celsius would this reaction go twice as
fast?
B)Given that the initial rate constant is 0.0170s−1 at an
initial temperature of 30 ∘C , what would the rate constant be at a
temperature of 200. ∘C for the same reaction described in Part
A?

Part A: The activation energy of a certain
reaction is 43.5 kJ/mol . At 23 ∘C , the rate constant is
0.0180s−1. At what temperature in degrees Celsius would this
reaction go twice as fast?
Part B: Given that the initial rate constant is
0.0180s−1 at an initial temperature of 23 ∘C , what would the rate
constant be at a temperature of 190. ∘C for the same reaction
described in Part A?

Part A: The activation energy of a certain reaction is 42.3
kJ/mol . At 29 ∘C , the rate constant is 0.0170s−1 . At what
temperature in degrees Celsius would this reaction go twice as
fast?
Part B: Given that the initial rate constant is 0.0170s−1 at an
initial temperature of 29 ∘C , what would the rate constant be at a
temperature of 120. ∘C for the same reaction described in Part
A?

Part A:
The activation energy of a certain reaction is 42.8 kJ/mol . At
28 ∘C , the rate constant is 0.0190s−1. At what temperature in
degrees Celsius would this reaction go twice as fast?
Part B:
Given that the initial rate constant is 0.0190s−1 at an initial
temperature of 28 ∘C , what would the rate constant be
at a temperature of 150 ∘C for the same reaction
described in Part A?

A certain reaction has an activation energy of 66.0 kJ/mol and a
frequency factor of A1 = 8.30×1012 M−1s−1 .
What is the rate constant, k, of this reaction at 27.0 ∘C
?
An unknown reaction was observed, and the following data were
collected:
T
(K)
k
(M−1⋅s−1)
352
109
426
185
Determine the activation energy for this reaction.

A. The activation energy of a certain reaction is 42.0 kJ/mol .
At 29 ∘C , the rate constant is 0.0190s-1. At what
temperature in degrees Celsius would this reaction go twice as
fast? Express your answer with the appropriate units.
B. Given that the initial rate
constant is 0.0190s-1 at an initial temperature of 29 C
, what would the rate constant be at a temperature of
120. ∘C for the same reaction described in Part
A?
Express your answer...

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