Question

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*=*A**e*−*E*a/*R**T*

where *k* is the rate constant, *A* is the
frequency factor, *E*a is the activation energy,
*R*=8.314 J/(mol⋅K) is the universal gas constant, and
*T* is the absolute temperature.

__________________________________________________

A certain reaction has an activation energy of 66.0 kJ/moland a
frequency factor of *A*1 = 2.20×10^{12} M−1s−1 .
What is the rate constant, *k*, of this reaction at 26.0 ∘C
?

Express your answer with the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot (asterisk) or a dash. Enter your answer using dimensions of rate constant units for second-order reaction.

Answer #1

A certain reaction has an activation energy of 64.0 kJ/mol and a
frequency factor of A1 = 5.70×1012 M−1s−1 .
What is the rate constant, k , of this reaction at 20.0 ∘C
?
Express your answer with the appropriate units. Indicate the
multiplication of units explicitly either with a multiplication dot
(asterisk) or a dash.
Part B
An unknown reaction was observed, and the following data were
collected:
T
(K )
k
(M−1⋅s−1 )
352
109
426
185
Determine...

A certain reaction has an activation energy of 60.0 kJ/mol and a
frequency factor of A1 = 2.80×1012 M−1s−1 . What is the rate
constant, k, of this reaction at 30.0 ∘C ?
I tried k = Ae^(-Ea/RT) but it's giving me 1.26E2 M^-1s^-1 which
is wrong on my online homework, I did convert C to K and kJ/mol to
J.

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...

± 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 shows the relationship between the rate constant
k and the temperature Tin kelvins and is
typically written as
k=Ae−Ea/RT
where 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
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 temperatures
(T1and...

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.

± 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 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.

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...

explain a procedure/analysis to measure activation energy (Ea)
experimentally by using the Arrhenius expression for the
temperature dependence of the rate constant k
k(T)=Ae-Ea/RT

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