Question

The
Arrhenius equation shows the relationship between the rate constant
k and the temperature Tin kelvins and is
typically written as
R is the gas constant (8.314 J/mol⋅K), Ais
a constant called the frequency factor, and Ea is
the activation energy for the reaction.
However, a more practical form of this equation is
ln
ln k1 and k2 are the rate constants for a
single reaction at two different absolute temperatures
(T1and T2). |
The activation energy of a certain reaction is 45.6 kJ/mol . At 30 ∘C , the rate constant is 0.0160s−1. At what temperature in degrees Celsius would this reaction go twice as fast? Express your answer with the appropriate units.
Submit
Given that the initial rate constant is 0.0160s−1 at an initial temperature of 30 ∘C , what would the rate constant be at a temperature of 170. ∘C for the same reaction described in Part A? Express your answer with the appropriate units.
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Answer #1

± The Arrhenius Equation
The Arrhenius equation shows the relationship between the rate
constant k and the temperature T in kelvins and
is typically written as
k=Ae−Ea/RT
where R is the gas constant (8.314 J/mol⋅K), A
is a constant called the frequency factor, and Ea
is the activation energy for the reaction.
However, a more practical form of this equation is
lnk2k1=EaR(1T1−1T2)
which is mathmatically equivalent to
lnk1k2=EaR(1T2−1T1)
where k1 and k2 are the rate constants for a
single reaction...

± The Arrhenius Equation
The Arrhenius equation shows the relationship between the rate
constant k and the temperature T in kelvins and
is typically written as
k=Ae−Ea/RT
where R is the gas constant (8.314 J/mol⋅K), A is
a constant called the frequency factor, and Eais
the activation energy for the reaction.
However, a more practical form of this equation is
lnk2k1=EaR(1T1−1T2)
which is mathmatically equivalent to
lnk1k2=EaR(1T2−1T1)
where k1 and k2 are the rate constants for a
single reaction at...

The Arrhenius equation shows the relationship between the rate
constant k and the temperature T in kelvins and is typically
written as k=Ae−Ea/RT where R is the gas constant (8.314 J/mol⋅K),
A is a constant called the frequency factor, and Ea is the
activation energy for the reaction. However, a more practical form
of this equation is lnk2k1=EaR(1T1−1T2) which is mathmatically
equivalent to lnk1k2=EaR(1T2−1T1) where k1 and k2 are the rate
constants for a single reaction at two different absolute...

A. The Arrhenius
equation shows the relationship between the rate constant
k and the temperature T in kelvins
and is typically written as
k=Ae−Ea/RT
where R is the gas constant (8.314 J/mol⋅K), A
is a constant called the frequency factor, and Ea
is the activation energy for the reaction.
However, a more practical form of this equation is
lnk2k1=EaR(1T1−1T2)
which is mathematically equivalent to
lnk1k2=EaR(1T2−1T1)
where k1 and k2 are the rate constants for a
single reaction at two different...

The Arrhenius Equation is typically written as
k=Ae−Ea/RT
However, the following more practical form of this equation also
exists:
lnk2k1=EaR(1T1−1T2)
where k1 and k2 are the rate constants for a
single reaction at two different absolute temperatures
(T1and T2).
Part A
The activation energy of a certain reaction is 32.1 kJ/mol . At
20 ∘C, the rate constant is 0.0130 s−1. At what temperature would
this reaction go twice as fast?
Express your answer numerically in degrees Celsius
Part B...

A certain reaction has an activation energy of 31.40 kJ/mol. At
what Kelvin temperature will the reaction proceed 6.50 times faster
than it did at 293 K?
Use the Arrhenius equation
ln (k2/k1) = Ea/R [(1/T1)-(1/T2)]
Where R=8.3145 J/(molxK)

The following data show the rate constant of a reaction measured
at several different temperatures.
Temperature (K)
Rate constant (1/s)
300
6.50×10−2
310
0.191
320
0.527
330
1.36
340
3.34
Part A. Use an Arrhenius plot to determine the activation
barrier (Ea) for the reaction.
Part B. Use an Arrhenius plot to determine the frequency factor
(A) for the reaction.

There are several factors that affect the rate of a reaction.
These factors include temperature, activation energy, steric
factors (orientation), and also collision frequency, which changes
with concentration and phase. All the factors that affect reaction
rate can be summarized in an equation called the Arrhenius
equation:
k=Ae−Ea/RT
where k is the rate constant, A is the
frequency factor, Ea is the activation energy,
R=8.314 J/(mol⋅K) is the universal gas constant, and
T is the absolute temperature.
__________________________________________________
A certain...

The rate constant of a chemical reaction increased from 0.100
s−1 to 2.60 s−1 upon raising the temperature from 25.0 ∘C to 45.0
∘C .
I solved
(1T2−1T1) =
−2.11×10−4
K−1
In (k1/k2) = -3.26
But, I'm having problems on this question:
What is the activation energy of the
reaction?
Express your answer numerically in kilojoules per
mole.
It would be great if you could show all of your work. I've been
trying to figure out this problem for a...

The rate constant of a chemical reaction increased from 0.100
s−1 to 3.10 s−1 upon raising the temperature from 25.0 ∘C to 51.0
∘C .
Part A
Calculate the value of (1/T2−1/T1) where
T1 is the initial temperature and T2 is the final
temperature.
Express your answer numerically.
Part B
Calculate the value of ln(k1/k2) where
k1 and k2 correspond to the rate constants at the
initial and the final temperatures as defined in part A.
Express your answer numerically....

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