Question

In a series of experiments on the decomposition of dinitrogen
pentoxide, N_{2}O_{5}, rate constants were
determined at two different temperatures. At 35°C, the rate
constant was 1.4×10^{-4}/s; at 45°C, the rate constant was
5.0×10^{-4}/s.

(a) What is the activation energy for this reaction? | |

(b) What is the value of the
rate constant at 85°C? |

Answer #1

Dinitrogen pentoxide (N2O5) decomposes in chloroform as a
solvent to yield NO2 and O2. The decomposition is first order with
a rate constant at 45 ∘C of 1.0×10−5s−1.
Part A
Calculate the partial pressure of O2 produced from 1.44 L of
0.543 M N2O5 solution at 45 ∘C over a period of 15.0 h if the gas
is collected in a 12.6-L container. (Assume that the products do
not dissolve in chloroform.)

Dinitrogen pentoxide (N2O5) decomposes in chloroform as a
solvent to yield NO2 and O2. The decomposition is first order with
a rate constant at 45 ∘C of 1.0×10−5s−1.
Calculate the partial pressure of O2 produced from 1.15 L of
0.592 M N2O5 solution at 45 ∘C over a period of 24.3 h if the gas
is collected in a 12.1-L container. (Assume that the products do
not dissolve in chloroform.)

Dinitrogen pentoxide (N2O5) decomposes in chloroform as a
solvent to yield NO2 and O2. The decomposition is first order with
a rate constant at 45 ∘C of 1.0×10−5s−1.
Part A
Calculate the partial pressure of O2 produced from 1.69 L of
0.524 M N2O5 solution at 45 ∘C over a period of 16.2 h if the gas
is collected in a 11.6-L container. (Assume that the products do
not dissolve in chloroform.)
Answer Pressure in terms of atm

1) The gas phase decomposition of dinitrogen pentoxide at 335
K
N2O5(g) 2
NO2(g) + ½ O2(g)
is first order in
N2O5 with a rate constant of
4.70×10-3
s-1.
If the initial concentration of
N2O5 is
0.105 M, the concentration of
N2O5 will
be Mafter 391 s have
passed.
2) The gas phase decomposition of dinitrogen pentoxide at 335
K
N2O5(g)2
NO2(g) + ½ O2(g)
is first order in
N2O5 with a rate constant of
4.70×10-3
s-1.
If the initial concentration of...

Dinitrogen pentoxide (N2O5) decomposes in chloroform as a
solvent to yield NO2 and O2. The decomposition is first order with
a rate constant at 45 ∘C of 1.0×10−5s−1.
Calculate the partial pressure of O2 produced from 1.63 L of
0.589 M N2O5 solution at 45 ∘C over a period of 18.4 h if the gas
is collected in a 11.2-L container. (Assume that the products do
not dissolve in chloroform.)
I came up with .05757 atm but its telling me...

For the decomposition of gaseous dinitrogen pentoxide
(shownbelow), the rate constant is k = 2.8 10-3 s-1 at 60°C. The
initialconcentration of N2O5 is 2.31 mol/L. 2 N2O5(g) 4NO2(g) +
O2(g) (a) What is [N2O5] after 5.00 min? _____mol/L (b) What
fraction of the N2O5 has decomposed after 5.00 min?

The following data were obtained in a kinetic run from the
decomposition of gaseous dinitrogen pentoxide at a set
temperature.
2N2O5(g) = 4NO2(g) +
O2(g)
Time (s)
0
100
200
300
400
500
600
700
[N2O5]
0.0200
0.0169
0.0142
0.0120
0.0101
0.0086
0.0072
0.0061
a.Graphically determine the order of
the reaction.
b.Calculate the rate constant for
the reaction.
c.Calculate the concentration of
dinitrogen pentoxide in the reaction vessel after 350 seconds.

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.

Values of the rate constant for the decomposition of N2O5 at
four different temperatures are as follows: T(K) k(s^-1) 658 2.14 x
10^5 673 3.23 x 10^5 688 4.81 x 10^5 703 7.03 x 10^5 Determine the
activation energy of the decomposition reaction: _____kJ/mol
Calculate the value of the rate constant at 300 K. _____s^-1

Dinitrogen pentoxide, N2O5, decomposes by first-order kinetics
with a rate constant of 3.7 × 10–5 s–1 at 298 K.
a. What is the half-life, in hours, of N2O5 at 298 K?
b. If [N2O5]0 = 0.0648 mol·L–1, what will be the concentration
of N2O5 after 2.1 hours?
c. How much time, in minutes, will elapse before the N2O5
concentration decreases from 0.0648 mol·L–1 to 0.0246 mol·L–1?

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