Question

A certain reaction has an activation energy of 64.0 kJ/mol and a
frequency factor of *A*1 = 5.70×10^{12} 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 the activation energy for this reaction.

Answer #1

Given the activation energy, Ea = 64.0 KJ/mol = 64000 J/mol

Frequency factor, A1 = 5.70x10^{12}
M^{-1}s^{-1}

Temperature, T = 20 C = 20+273 = 293 K

Rate constant can be calculated from the following formulae

k = A x (exp)^{(-Ea/RT)} = (5.70x10^{12}
M^{-1}s^{-1}) x (exp)^{(- 64000 J/mol / 8.314
J.K-1.mol-1 x 293K)} = 22.17 M^{-1}s^{-1}
(answer)

Part - B:

T1 = 352 K, k1 = 109 M^{-1}s^{-1}

T2 = 426 K, k2 = 185 M^{-1}s^{-1}

ln(k1 / k2) = - (Ea / R)x(1/T1 - 1/T2) = - (Ea / R)x(T2 - T1) / T1T2

=> ln(109 M^{-1}s^{-1} / 185
M^{-1}s^{-1} ) = - (Ea / R)x(426K - 352K) /
352Kx426K

=> Ea = 8912 J = 8.91 KJ/mol (answer)

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 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.

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 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...

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...

1) A first order reaction has an activation energy of 66.6
kJ/mol and a frequency factor (Arrhenius constant) of 8.78 x
1010 sec -1. Calculate the rate constant at
19 oC. Use 4 decimal places for your answer.
2) A first order reaction has a rate constant of 0.988 at 25
oC and 9.6 at 33 oC. Calculate the value of
the activation energy in KILOJOULES (enter answer to one decimal
place)

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

A certain reaction has an activation energy of 65.39 kJ/mol. At
what Kelvin temperature will the reaction proceed 3.50 times faster
than it did at 337 K?

A certain reaction has an activation energy of 64.28 kJ/mol. At
what Kelvin temperature will the reaction proceed 4.50 times faster
than it did at 329 K?

A certain reaction has an activation energy of 53.03 kJ/mol. At
what Kelvin temperature will the reaction proceed 7.00 times faster
than it did at 365 K?

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 8 minutes ago

asked 8 minutes ago

asked 19 minutes ago

asked 19 minutes ago

asked 34 minutes ago

asked 43 minutes ago

asked 44 minutes ago

asked 52 minutes ago

asked 52 minutes ago

asked 56 minutes ago

asked 1 hour ago

asked 1 hour ago