Question

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 temperatures (T1 and T2).

A.

The activation energy of a certain reaction is 32.9 kJ/mol . At 23 ∘C , the rate constant is 0.0160s−1. At what temperature in degrees Celsius would this reaction go twice as fast?

B.

Given that the initial rate constant is 0.0160s−1 at an initial temperature of 23 ∘C , what would the rate constant be at a temperature of 140. ∘C for the same reaction described in Part A?

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 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. 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...

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...

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

Explain the Arrhenius Equation, k = Ae-Ea/RT, in your own words.
How does the Arrhenius Equation relate to the iodine clock
reaction? Please explain in one well-developed paragraph.

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)

For a Reaction that has positive activation energy, would you
expect increasing the temperature to increase or decrease the
reaction rate? Please explain your answer in using
"rate=K[A]^x[B]^y" and "K=Ae*-Ea/rT"

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