Question

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.

Answer #1

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...

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...

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...

The hydrolysis of urea to ammonia plus CO2 normally has an
activation energy of 125 kJ/mol at 294 K, but when the urease
enzyme catalyzes the reaction it lowers the activation energy to 46
kJ/mol. By what factor does this increase the velocity of the
reaction? The rate constant equation might be helpful here, where k
= A·e(-ΔG°‡/RT) and A = 6.12 x 1012 s-1. Look at both kcat and
knon, finding the ratio between the two

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.

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)

The gas-phase reaction of NO with F2 to form NOF and F has an
activation energy of Ea = 6.30 kJ/mol and a frequency
factor of A = 6.00×108M−1⋅s−1 . The
reaction is believed to be bimolecular:
NO(g)+F2(g)→NOF(g)+F(g)
What is the rate constant at 695 ∘C ?
Express your answer to three significant digits with the
appropriate units. For compound units, place a multiplication dot
between units (e.g. J⋅mol−1⋅K−1).
(I got 2.74*10^8 M-1s-1 but it is wrong. I got a...

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.

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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