Question

**A.** The Arrhenius
equation shows the relationship between the rate constant
*k* and the temperature *T* in kelvins
and is typically written as

*k*=*A**e*−*E*a/*R**T*

where *R* is the gas constant (8.314 J/mol⋅K), *A*
is a constant called the *frequency factor*, and *E*a
is the *activation energy* for the reaction.

However, a more practical form of this equation is

ln*k*2*k*1=*E*a*R*(1*T*1−1*T*2)

which is mathematically equivalent to

ln*k*1*k*2=*E*a*R*(1*T*2−1*T*1)

where *k*1 and *k*2 are the rate constants for a
single reaction at two different absolute temperatures (*T*1
and *T*2).

**Part 1:** The
activation energy of a certain reaction is 43.9 kJ/mol . At
28 ∘C , the rate constant is 0.0130s−1. At what
temperature in degrees Celsius would this reaction go twice as
fast?

Express your answer with the appropriate units.

**Part 2:** Given
that the initial rate constant is 0.0130s−1 at an initial
temperature of 28 ∘C , what would the rate constant be
at a temperature of 100. ∘C for the same reaction
described in Part A?

Express your answer with the appropriate units.

**B.** A reaction
occurs by a two-step mechanism, shown below. Step 1: AX2(g) → AX(g)
+ X(g) Step 2: AX2(g) + X(g) → AX + X2(g) The intermediate in this
reaction is ________, and the molecularity of the second step is
________. Enter your answers separated by a comma.

*** The answer is NOT AX and 2**

Answer #1

To
convert Kelvin to Celsius.

C+ 273= 313.4 K

Temperature in degree Celsius = 313.4 - 273 = 40.4 deg C

Please post the remaining question as a new question

Update

B)

A reaction intermediate is transient species within a multi-step reaction mechanism that is produced in the preceding step and consumed in a subsequent step to ultimately generate the final reaction product.

So X which is formed in Step 1 and consumed in step 2 to produce the product X2 is the intermediate.

Molecularity is the number of molecules that come together to react in an elementary reaction and is equal to the sum of stoichiometric coefficients of reactants in this elementary reaction.

Molecularity of the second step is 1+1= 2

The answer is X and 2

± 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 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 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 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 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...

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...

The following data show the rate constant of a reaction measured
at several different temperatures.
Temperature (K)
Rate constant (1/s)
300
6.50×10−2
310
0.191
320
0.527
330
1.36
340
3.34
Part A. Use an Arrhenius plot to determine the activation
barrier (Ea) for the reaction.
Part B. Use an Arrhenius plot to determine the frequency factor
(A) for the reaction.

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?

Rate constants for the reaction
NO2(g)+CO(g)?NO(g)+CO2(g)
are 1.3M?1s?1 at 700 K and 23.0M?1s?1 at 800 K.
Part A
What is the value of the activation energy in kJ/mol?
Ea =
134
kJ/mol
SubmitMy AnswersGive
Up
Correct
Part B
What is the rate constant at 770K ?
Express your answer using two significant figures.
k =
/(M?s)

Part A
The activation energy of a certain reaction is 43.9 kJ/mol . At
28 ∘C , the rate constant is 0.0130s−1. At what
temperature in degrees Celsius would this reaction go twice as
fast?
Express your answer with the appropriate units.
Part B
Given that the initial rate constant is 0.0130s−1 at an initial
temperature of 28 ∘C , what would the rate constant be
at a temperature of 100. ∘C for the same reaction
described in Part A?
Express your answer...

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