Question
In: Chemistry
Dinitrogen Pentoxide (N2O5) decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition...
Dinitrogen Pentoxide (N2O5) decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition is first order with a rate constatnt at 50 degrees Celcius 1.75 x 10-5 s-1. Calculate the partial pressure of O2 produce from 1.00L of 0.500 M N2O5 solution at 50 degrees celcius over a period of 18.0 hours if the gas collected in a 10.0L container. (Assume that the products do not dissolve in chloroform.)
Solutions
Expert Solution
Activation energy plays no role in this problem. It would be of
interest if you want to evaluate rates of reaction on different
temperature levels.
From the given information you can calculate the change of reactant
concentration with time. From this you get the change of
concentration and subsequently the number of moles of reactant,
which have reacted away. The amount of product formed is
proportional to that. Then use ideal gas law to calculate the
partial pressure.
How it works in detail:
We've got a first order reaction. i.e.
d[N?O?]/dt = - k?[N?O?]
Solving this differential equation with initial concentration
[N?O?]? leads to the integrated rate law:
ln[N?O?] = - k?t + ln[N?O?]?
From this you can calculate the concentration of nitrogen pentoxide
after 18h = 64800s
ln[N?O?] = - k?t + ln[N?O?]?
<=>
ln( [N?O?] / [N?O?]? ) = - k?t
<=>
[N?O?] = [N?O?]? ? e^(- k?t)
= 0.5M ? e^(-1.75
queen_honey_blossom answered 1 year agoRelated Solutions
Dinitrogen pentoxide (N2O5) decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition...
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 0.659 M N2O5 solution at 45
∘C over a period of 24.2 h if the gas is collected in a 12.4-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...
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 1.47 L of
0.605 M N2O5 solution at 45 ∘C over a period of 18.5 h if the gas
is collected in a 11.4-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...
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 oC of 1.0 x 10–5 s–1. Calculate the partial
pressure (in atm) of O2 produced from 1.00 L of 0.600 M N2O5
solution at 45 oC over a period of 20.0 h if the gas is collected
in a 10.0-L container. (assume that the products do not dissolve in
chloroform.)
The decomposition of n2o5 is a first order reaction. N2o5 decomposes to yield no2 and o2....
The decomposition of n2o5 is a first order reaction. N2o5
decomposes to yield no2 and o2.
At 48deg C the rate constant for the reaction is 1.2x10^-5s^-1.
Calculate the partial pressure of no2 produced from 1.0L of 0.700M
n2o5 solution at 48deg C over a period of 22 hours if the gas is
collected in a 10.0L container. Show work please.
1. The activation energy for the gas phase decomposition of dinitrogen pentoxide is 103 kJ. N2O5---------...
1. The activation energy for the gas phase
decomposition of dinitrogen pentoxide is
103 kJ.
N2O5---------
NO2 + 1/2 O2
The rate constant at 314 K is
2.76×10-4 /s. The rate constant will be
1.49×10-3 /s at -----------k
2. The activation energy for the gas phase
decomposition of dinitrogen pentoxide is
103 kJ.
N2O5-----------2
NO2 + 1/2 O2
The rate constant at 305 K is
8.40×10-5 /s. The rate constant will be
------- /s at 345 K.
In the reaction of gaseous N2O5 to yield NO2 gas and O2 gas as shown below...
In the reaction of gaseous N2O5 to yield
NO2 gas and O2 gas as shown below the
following data table is obtained:
2 N2O5 (g) → 4 NO2 (g) +
O2 (g)
Data Table #1
Time (sec)
[N2O5]
[O2]
0
0.200 M
0
300
0.182 M
0.009 M
600
0.166 M
0.017 M
900
0.152 M
0.024 M
1200
0.140 M
0.030 M
1800
0.122 M
0.039 M
2400
0.112 M
0.044 M
3000
0.108 M
0.046 M
Complete the...
Dinitrogen pentoxide decomposes in the gas phase to form nitrogen dioxide and oxygen gas. The reaction...
Dinitrogen pentoxide decomposes in the gas phase to form
nitrogen dioxide and oxygen gas. The reaction is first order in
dinitrogen pentoxide and has a half-life of 2.81 h at 25 ∘C.
If a 1.5-L reaction vessel initially contains 760 torr of N2O5
at 25 ∘C, what partial pressure of O2 is present in the vessel
after 225 minutes?
Dinitrogen pentoxide decomposes in the gas phase to form nitrogen dioxide and oxygen gas. The reaction...
Dinitrogen pentoxide decomposes in the gas phase to form
nitrogen dioxide and oxygen gas. The reaction is first order in
dinitrogen pentoxide and has a half-life of 2.81 h at 25 ∘C.
If a 1.7-L reaction vessel initially contains 760 torr of N2O5
at 25 ∘C, what partial pressure of O2 is present in the vessel
after 205 minutes?
The specific rate constant for the first-order decomposition of N2O5(g) to NO2(g) and O2(g) is 7.48×10−3s−1...
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 0.150 atm .
B. 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 .
C. Find...
The specific rate constant for the first-order decomposition of N2O5(g) to NO2(g) and O2(g) is 7.48×10−3s−1...
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.
1. Find the length of time required for the total pressure in a
system containing N2O5 at an initial pressure of 0.110 atm to rise
to 0.220 atm .
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