Question

The gas phase reaction

2N2O5(g)->4NO2(g)+O2(g)

has an activation energy of 103 kJ/mole, and the first order rate constant is 1.16x10^-8 min^-1 at 231 K. what is the rate constant at 211K?

Answer #1

ARRHENIUS EQUATION CALCULATIONS The activation energy for the
gas phase decomposition of dinitrogen pentoxide is 103 kJ. N2O52
NO2 + 1/2 O2 The rate constant at 319 K is 5.59×10-4 /s. The rate
constant will be 6.37×10-3 /s at ______ K.
PART 2 The activation energy for the gas phase isomerization of
isopropenyl allyl ether is 123 kJ.
CH2=C(CH3)-O-CH2CH=CH2CH3COCH2CH2CH=CH2 The rate constant at 432 K
is 2.68×10-4 /s. The rate constant will be______ /s at 474 K.

The rate constant for the reaction 2N2O5(g) → 4NO2(g) + O2(g) is
equal to 3.41 x 10–5 s–1 at 30 ºC. If the initial concentration of
N2O5 is 0.446 M what concentration of NO2 will be observed after
175 minutes? Assume that initially no NO2 was present in the
reaction vessel.

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...

The first-order rate constant for
the decomposition of N2O5,
2N2O5(g)?4NO2(g)+O2(g),
at 70?C is 6.82×10?3s?1. Suppose we start with 2.90×10?2
mol of N2O5(g) in a volume of 1.5 L .
a) How many moles of N2O5 will remain after 5.0 min ?
b) How many minutes will it take for the quantity of N2O5 to
drop to 2.0×10?2 mol?
c) What is the half-life of N2O5 at 70?C?

The first-order rate constant for the decomposition of N2O5,
2N2O5(g)→4NO2(g)+O2(g) at 70∘C is 6.82×10^−3 s−1. Suppose we start
with 2.60×10^−2 mol of N2O5(g) in a volume of 2.4 L . How many
moles of N2O5 will remain after 4.0 min ? How many minutes will it
take for the quantity of N2O5 to drop to 1.9×10^−2 mol ? What is
the half-life of N2O5 at 70∘C?

The first-order rate constant for the decomposition of N2O5,
2N2O5(g)→4NO2(g)+O2(g)
at 70∘C is 6.82×10−3 s−1. Suppose we start with
2.30×10−2 mol of N2O5(g) in a volume of 1.8 L .
a) How many moles of N2O5 will remain after 6.0 min ?
b) How many minutes will it take for the quantity of N2O5 to
drop to 1.6×10−2 mol ?
c) What is the half-life of N2O5
at 70∘C?

The first-order rate constant for the decomposition of N2O5,
2N2O5(g)→4NO2(g)+O2(g)
at 70∘C is 6.82×10−3 s−1. Suppose we start with
2.10×10−2 mol of N2O5(g) in a volume of 1.8 L .
How many minutes will it take for the quantity of N2O5 to drop
to 1.6×10−2 mol ?

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 gas-phase association reaction between F2 and IF5 is
first-order in each of the reactants. The energy of activation for
the reaction is 58.6 kJ mol−1. At 65°C the rate constant is
7.84 ✕ 10−3 kPa−1 s−1. Calculate the entropy of activation at 65°C.
Please show all work and report answer in J/k*mol to multiple sig
figs.

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...

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