Question

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 reaction at 368.4 K.

Answer #1

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.

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.

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...

The activation energy of a reaction is 55.6 kJ/mol and the
frequency factor is 1.5×1011/s. Calculate the rate constant of the
reaction at 23 ∘C. Express your answer using two significant
figures.

1) A first order reaction has an activation energy of 66.6
kJ/mol and a frequency factor (Arrhenius constant) of 8.78 x
1010 sec -1. Calculate the rate constant at
19 oC. Use 4 decimal places for your answer.
2) A first order reaction has a rate constant of 0.988 at 25
oC and 9.6 at 33 oC. Calculate the value of
the activation energy in KILOJOULES (enter answer to one decimal
place)

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...

Calculate the rate constant, k, for a reaction at 65.0 °C that
has an activation energy of 87.1 kJ/mol and a frequency factor of
8.62 × 1011 s–1.

The activation energy of a certain uncatalyzed reaction is 64
kJ/mol. In the presence of a catalyst, the Ea is 55 kJ/mol. How
many times faster is the catalyzed than the uncatalyzed reaction at
400°C? Assume that the frequency factor remains the same.

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

a.)A certain reaction has an activation energy of 25.10 kJ/mol.
At what Kelvin temperature will the reaction proceed 7.00 times
faster than it did at 289 K?
b.A certain reaction has an enthalpy of ΔH = 39 kJ and an
activation energy of Ea = 51 kJ. What is the activation energy of
the reverse reaction?
c.)At a given temperature, the elementary reaction A<=> B in
the forward direction is the first order in A with a rate constant
of...

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