Question

The following data are obtained for the decomposition of N2O5 at a certain temperature: 2N2O5(g) ↔ 4NO2(g) + O2(g) Time(s) 0 200 400 600 800 N2O5 (atm) 2.80 2.51 2.25 2.01 1.80 Find the rate constant kobs for this first-order decomposition reaction. (Enter in sec-1)

Answer #1

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.

Please include all steps and significant digits and units.
2N2o5 (g) --> 4No2 (g) + O2 (g)
The following data were obtained in a kinetic run from the
decomposition of gaseous dinitrogen pentoxide at a set
temperature.
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 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 ?

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 decomposition of N2O5 can be described by
equation
2N2O5 (soln) = 4NO2 (soln) + O2 (g)
t (s) [N2O5](M)
0 ----- 2.62
215----2.29
506----1.91
795----1.59
given data for reaction at 45°C .
A).
interval 0-215s
reaction rate ? M/s
B).
interval 215-506s
reaction rate? M/s
C).
interval 506-795s
reaction rate? M/s

The specific rate constant for the first-order decomposition of
N2O5(g) to NO2(g) and O2(g) is
7.48×10−3s−1 at a given temperature.
A. Find the length of time required for the total pressure in a
system containing N2O5 at an initial pressure of 0.100 atm to rise
to 0.200 atm .
B. Find the total pressure after 110 s of reaction.

For the reaction 2N2O5(g) →
4NO2(g) + O2(g), the
following data were collected:
t (minutes)
[N2O5] (mol/L)
0
1.24 × 10–2
10.
0.92 × 10–2
20.
0.68 × 10–2
30.
0.50 × 10–2
40.
0.37 × 10–2
50.
0.28 × 10–2
70.
0.15 × 10–2
Reference: Ref 12-10
The half-life of this reaction is approximately

The first order constant is 4.82 x 10-3
s-1 at 70C for the decomposition of the following
reaction: 2N2O5 (g) -> 4NO2 +
O2 (g)
Suppose that you start with .0175M of N2O5
(g)
a.) What is the molarity of N2O5 that
remains after 15 minutes (note: the rate constant is in
seconds)
b.) How many seconds will it take for the quantity of
N2O5 to drop to .015M?
c.) What is the half life of N2O5 at
70C?

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