Question

If the rate constant k of a reaction doubles when the temperature increases from 121 °C to 279 °C, what is the activation energy of the reaction in units of kJ/mol? Do not enter units with your numerical answer. Do not use scientific notation.

Answer #1

The rate constant of a reaction is 6.7 ×
10−3 s−1 at
25°C, and the activation energy is
33.6 kJ/mol.
What is k at 75°C? Enter your
answer in scientific notation.

By what factor does the rate constant increase when the
temperature increases from 200. K to 400. K for a reaction with an
activation energy of 845 J/mol?

the rate constant of a reaction is 4.0x10^-3 s^-1 at 25 degrees
C, and the activation energy is 33.6 kJ/mol. What is k at 75
degrees C? Enter in scientific notation

If the rate of a reaction increases by a factor of 2.8 when the
temperature is raised from 20 ∘C to 30 ∘C, what is the value of the
activation energy in kJ/mol?
By what factor does the rate of this reaction increase when the
temperature is raised from 130 ∘C to 140 ∘C?

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...

what is the activation energy(Ea) of a first order reaction is
the reaction rate constant(k) increases from 0.0300 min to 0.500
min as the temperature increases from 20.0 C to 45.0 C?

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 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 rate constant of a reaction is 8.05 ×
10−5 L/mol·s at 195°C and 3.20 ×
10−3 L/mol·s at 258°C. What is the
activation energy of the reaction? Enter your answer in scientific
notation.

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.

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