Question
In: Chemistry
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?
Solutions
Expert Solution
half- life = 2.81 h
rate constant = k = 0.693 / t1/2 = 0.693 / 2.81
k = 0.247 h-1
initial pressure = 760 torr
t = 205 min = 205 / 60 = 3.42 hour
k = 1/t * ln (Po / Pt)
0.247 = 1/3.42 * ln (760 / Pt)
Pt = 326.6 torr
remaining pressure of N2O5 after 205 min
2N2O5 -----------------------> 4 NO2 + O2
760 0 0 ----------------> initial
760 -2x 4x x ---------------------> after 205 min
760 -2x = 326.6
x = 216.7
partial pressure of O2 = x = 216.7 torr
queen_honey_blossom answered 2 years agoRelated Solutions
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?
Nitrogen gas reacts with oxygen gas to form dinitrogen tetroxide. N2 (g) + 2 O2 (g)...
Nitrogen gas reacts with oxygen gas to form dinitrogen
tetroxide.
N2 (g) + 2 O2 (g) → N2O4 (g)
A 1.8 L reaction vessel, initially at 298 K, contains nitrogen
gas at a partial pressure of 337 mmHg and oxygen gas at a partial
pressure of 445 mmHg .
What is the pressure of N2O4 in the reaction vessel after the
reaction?
Enter your answer numerically, in terms of
mmHg.
Please show all work
Nitric acid (NO) reacts with oxygen gas to form nitrogen dioxide (NO2), a dark brown gas:...
Nitric acid (NO) reacts with oxygen gas to form nitrogen
dioxide (NO2), a dark brown gas:
2NO(g) + O2(g) →
2NO2(g)
In one experiment 0.886 mole of NO is mixed with 0.503 mol of
O2.
Calculate which of the two reactants is the limiting reagent.
(5 points)
Calculate also the number of moles of NO2 produced.
(5 points)
What reactant is left over and how much of it is left over?
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 nitrogen gas with oxygen gas to produce nitrogen oxide. What is the...
In the reaction of nitrogen gas with oxygen gas to produce
nitrogen oxide. What is the effect of adding more nitrogen gas to
the initial reaction mixture? N2+O2-2NO. A) the equilibrium shifts
to produce more N2 b) the temperature of the reaction is raised c)
extra catalyst is required to reach equilibrium d) the equilibrium
shifts to produce more NO e) the equilibrium Is not effected
Sulfur dioxide reacts with oxygen to produce sulfur trioxide in a gas-phase reaction. (a) A 1.500...
Sulfur dioxide reacts with oxygen to produce sulfur trioxide in
a gas-phase reaction.
(a) A 1.500 L flask was filled with 4.00 x 10^-2 moles of sulfur
dioxide and 2.00 x 10^-2 moles of oxygen, and the reaction is
initiated at 900K. At equilibrium, the flask contained 2.96 x 10^-2
moles of sulfure trioxide. What is the molarity of each substance
in the flask at equilibrium?
(b) Find K. Suppose that the 1.500 L flask was initially filled
with 4.00...
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 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.)
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.)
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