The Arrhenius equation relates reaction rates to temperature via the activation energy. Calculate the ratio of the rates at -30 degrees C (a typical stratospheric temperature) for two biomolecular reactions having the same Arrhenius A factor and initial concentrations , one of which is endothermic and has an activation energy of 54000 J /(mol) and the other of which is exothermic and has an activation energy of 7000 J /(mol).

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Arrhenius Equation:

k=A*exp(-Ea/R*T)

Where k is the rate coefficient, A is a constant, Ea is ...

Solution Summary

The solution involves the calculation of ratios for biomolecular reactions using Arrhenius equation reaction rates.

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The unimolecular decomposition of urea in aqueous solution
is measured at 2 different temperatures and the following data are observed:
Trial # Temp (C degrees) k (s-1)
1 60 1.2 X 10^-7
2 71.5 4.40 x 10^ -7
Determine the Arrhenius para

The rearrangement of cyclopropane to propene has been studied at various temperatures with the following results.
Rate constant, k (s-1) Temperature (K)
3.30 x 10-9 600
2.19 x 10-7 650
7.96 x 10-6 700
1.80 x 10-4 750
2.74 x 10-3 800
3.04 x 10-2 850
2.58 x 10-1 900
(a) From the appropriate plot of these data, determi

Chemists commonly use a rule of thumb that an increase of 10 K in temperature doubles the rate of a reaction. What must the activation energy be for this statement to be true for a temperature increase from 49 to 59°C?

Knowing the rate constant is 3.46 X 10^-5 s^ at 298 and that energy activation is 1.60 x 10^5 J-mol ^-1. Determine the temperature at which the half life for the 1st order decomposition of dinitrogen pentoxide in carbon tetrachloride to dinitrogen tetroxide and oxygen is 2 hours.

For the reaction:
H2 + C2H4 -> C2H6
In gaseous phase, the pre-exponential factor is 1.24*10^6 [M-1s-1] and the activation energy is 180 kJ/mol. find the entropy, the enthalpy and the gibbs free energy.
see attachment

The rate of a particular reaction triples when the temprature is increased from 25C to 35C. Calculate the activation energy for this reaction.
Also i just need to clearify the concept of ArrheniusEquation. What happened to Rate Constant(k) and the rate of reaction if:
a. there is a decrease in temperature
b. an increase in

Practice Exercise 13.9
The first-order rate constant for the reaction of methyl chloride (CH3Cl) with water to produce methanol (CH3OH) and hydrochloric acid (HCl) is 3.32 10-10s-1 at 25°C. Calculate the rate constant at 33°C if the activation energy is 116 kJ/mol.
My answer, which was incorrect was 3.17e-10. I used th

I need help understanding the meaning and units involved in the Arrhenius Law equation.
Assuming a first order reaction:
k = Ae^-Ea/RT
1) Can this be re-written as: logk = -Ea/RT + constant ? What is the constant?
2) In either case:
a) How do I determine or choose the activation energy Ea? Where would I find

A thermal process (in this example a large rotating dryer) operating at 1500 degrees F is said to have air emissions of 5 lbs/hr formaldehyde (from the presence of formic acid) and 2 lbs/hr acetaldehyde (from the presence of acetic acid). The air stream from the thermal process is quantified as 75,000 cu. ft. per minute.
The