Question

**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.**

Answer #1

Arrhenius equation states

k = A e^{-Ea/RT}

where k = rate constant

A = preexponential factor

Ea = Activation energy

R = gas constant = 8.31 JK^{-1}mol^{-1}

T = temperature in Kelvin

ln k = -Ea/RT + ln A

so

ln(k1/k2) = Ea/R (T1-T2/T1T2)

ln(6.7 x 10^{-3}/k2) = 33600/8.31 x (298 - 348 /298 x
348)

ln(6.7 x 10^{-3}/k2) = 33600/8.31 x (4.821 x
10^{-4})

ln(6.7 x 10^{-3}/k2) = -1.949

(6.7 x 10^{-3}/k2) = e^{-1.949}

(6.7 x 10^{-3}/k2) = 0.1424

k2 = (6.7 x 10^{-3}/0.1424

k2 = 4.7 x 10^{-2}

The rate constant at 75 ^{o}C is **4.7
E-2**

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 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.

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.

A certain first-order reaction has a rate constant of
2.30×10−2 s−1 at 25 ∘C . What is the value of k
at 63 ∘C if Ea = 74.0 kJ/mol ?
Express your answer using two significant figures.
Part B
Another first-order reaction also has a rate constant of
2.30×10−2 s−1 at 25 ∘C . What is the value of k
at 63 ∘C if Ea = 128 kJ/mol ?
Express your answer using two significant figures.

Part A
A certain first-order reaction has a rate constant of
3.00×10−2 s−1 at 25 ∘C . What is the value of k
at 69 ∘C if Ea = 77.0 kJ/mol ?
Express your answer using two significant figures.
Part B
Another first-order reaction also has a rate constant of
3.00×10−2 s−1 at 25 ∘C . What is the value of k
at 69 ∘C if Ea = 115 kJ/mol ?
Express your answer using two significant figures.

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 rate constant of a first-order reaction is 3.20 × 10−4 s−1
at 350.°C. If the activation energy is 135 kJ/mol, calculate the
temperature at which its rate constant is 9.15 × 10−4 s−1.

If the rate constant increases from 0.40 M
–1 s –1 at 25°C to 0.80 M
–1 s –1 at 35°C, what is the activation
energy in kJ/mol for this reaction?

If a first order reaction has a rate constant of 4.15 X
10-2 s-1 at a temperature of
24.5oC, what would the value of k be if the reaction
temperature was changed to 52oC given that the
activation energy is 67.8 kJ/mol?

The first order rate constant for a reaction at 790
oC is 4.05e-03 s-1. If the activation energy
for the reaction is 255 kJ/mol, what is the rate constant at 890
oC?
k = s-1

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