Question

The decomposition of N2O5 is first order reaction. N2O5(g) decomposes to yield NO2 (g) and O2(g). At 48 deg C the rate constant for the reaction is 1.2x10^-5 s^-1. Calculate the partial pressure of NO2(g) produced from 1.0L of 0.700M N2O5 solution at 48 degC over a period of 22 hours if the gas is collected in a 10.0L container

Answer #1

Formula for first order reaction: k = (2.303/t)*log(a/(a-x)

k is rate constant, t is time, a is initial concentration, and x is change.

t = 22 h =22*60*60 = 7.92*10^4 /s

a = 1.0 L*0.700 M = 0.700 mol

1.2*10^-5 /s = (2.303/7.92*10^4 /s)*log(0.700/(0.700-x)

log(0.700/(0.700-x)) = 0.52

0.700/(0.700-x) = 3.28

3.28x = 1.6

x = 0.49 mol

Balanced equation: 2N2O5 ------>4NO2 + O2

mol ration of N2O5 to NO2 = 2:4 = 1:2

So, 2x = 0.98 moles of NO2 produced.

Ideal gas equation: PV = nRT

P is pressure, V is volume, n is number of moles, R is constant, and T is temperature

T = 48+273.15 = 321.15 K

P = (nRT)/V

= (0.98 mol*0.0821 atm L/mol K*321.15)/10.0 L

= 2.58 atm

So, the partial pressure of NO2 is **2.58 atm**

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

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...

The rate constant for the first-order decomposition of
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2 N2O5 (g) 4 NO2(g) + O2(g) is k, = 3.38 x 10-5 s
-1 at 25 C. What is the half-life of N2O5?
What will be the partial pressure, initially 500 Torr, at ( a) 50
s; (b) 20 min, (c) 2 hr
after initiation of the reaction?

Hydrogen peroxide decomposes to yield water and oxygen. The
decomposition is first order with a rate constant at 46°C of 1.6 ×
10-4 s-1. Calculate the partial pressure of
the oxygen produced from 1.25 L of a 0.750 M
H2O2 solution at 46°C over a period of 24.0
hours if the gas is collected in a 13.0 L container.
Please show all work! Thanks in advance!

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.

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.
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to come to equilibrium, what are the equilibrium partial pressures
of NO(g) and O2(g)?

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