Question

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

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...

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.

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...

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"

± 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...

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...

The energy of activation for the reaction 2 HI → H2 + I2 is 180.
kJ·mol−1 at 556 K. Calculate the rate constant using the equation k
= Ae^(−Ea/RT). The collision diameter for HI is
3.5 ✕ 10−8 cm. Assume that the pressure is 1.00 atm.

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...

The activation energy, Ea for a particular reaction is
13.6 kj/mol. If the rate constant at 754 degrees celsius is
24.5/min at egat temperature in celsius will the rate constant be
12.7/min? r= 8.314j/mol • K

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