Question

Answer the following based on the reaction. At 313 K, the rate constant for this reaction is 1.09×102 /s and at 564 K the rate constant is 6.62×106 /s.

cyclopentane → 1-pentene

1. Determine the activation energy (EA) (in kJ/mol) for this reaction.

2. Determine the pre-exponential factor, A (in /s) for this reaction.

3. Determine the rate constant (in /s) for this reaction at 1218 K.

Answer #1

Determine the activation energy (EA) (in kJ/mol) for this reaction.

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

ln ( 6.62×10^{6} / 1.09×10^{2}) = -Ea / 8.314
[1/564-1/313]

Ea 1.710 e-4 = 11.014

**Ea (**activation energy) **= 6.441 x
10 ^{4}**

2. Determine the pre-exponential factor, A (in /s) for this reaction.

k=Ae^{−Ea/RT}

ln k = ln A - Ea/RT

ln 6.62×10^{6} = ln A - 6.441 x
10^{4} / 8.314 x 564

**ln A = 15.70 + 13.7363 = 29.4419**

**A (pre-exponential factor) = 6.08354 x 10 ^{12}
S^{-1}**

3. Determine the rate constant (in /s) for this reaction at 1218 K.

rate constant (in /s) for this reaction at 1218 K

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

ln (K2 /6.62×106 ) = -6.441 x 10^{4} / 8.314 [1/1218 -
1/564]

ln K2 = 23.08

**K2 = 1.0524812872 x 10 ^{10} /S**

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The frequency factor and activation energy for a chemical
reaction are A = 8.08 x 10–12 cm3/(molecule·s) and Ea = 15.0 kJ/mol
at 368.4 K, respectively. Determine the rate constant for this
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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 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

The rate constant for the reaction below was determined to be
3.241×10-5 s–1 at 800 K. The activation energy of the reaction is
215 kJ/mol. What would be the value of the rate constant at
9.10×102 K? N2O(g) --> N2(g) + O2(g)
I'm having trouble calculating the rate constant with the
arrhenius equation that deals with two temps, could you show me the
step by step how to do this?

A reaction has a rate constant of 0.393 at 291 K and 1.41 at 345
K. Calculate the activation energy of this reaction in kJ/mol.

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 table below gives the values for the rate constant, k, of
the reaction between potassium hydroxide and bromoethane in ethanol
at a series of temperatures. Use these data to determine the
activation energy of the reaction.
Explain your answer in brief.
T/K 305.0 313.0 323.1 332.7 343.6 353.0
k/M-1 s-1 0.182 0.466 1.35 3.31 10.2 22.6
A 80J
B 90J
C 80 J mol-1
D 80 kJ mol-1
E 90 kJ mol-1

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...

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