Question

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 ?

Answer #1

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 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?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,
given below, at 70°C is 6.82 10-3 s-1. Suppose we start with 0.0550
mol of N2O5(g) in a volume of 3.5 L. 2 N2O5(g) → 4 NO2(g) + O2(g)
(a) How many moles of N2O5 will remain after 3.0 min? mol (b) How
many minutes will it take for the quantity of N2O5 to drop to 0.005
mol? min (c) What is the half-life of N2O5 at 70°C? min

The first-order rate constant for the decomposition of N2O5,
given below, at 70°C is 6.82 10-3 s-1. Suppose we start with 0.0550
mol of N2O5(g) in a volume of 2.5 L. 2 N2O5(g) → 4 NO2(g) + O2(g)
(a) How many moles of N2O5 will remain after 2.5 min? mol (b) How
many minutes will it take for the quantity of N2O5 to drop to 0.005
mol? min (c) What is the half-life of N2O5 at 70°C? min

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?

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

"For the reaction 2 N2O5 --> 4 NO2 + O2 the rate constant is
6.82 x 10^-3 s^-1 at 70 degrees Celsius. The reaction is first
order overall. If you start with 0.350 mol of dinitrogen pentoxide
in a 2.0 L volume, how many miles will remain after 10 minutes? How
long will it take for you to have 0.125 moles of reactant left?
What is the half-life of dinitrogen pentoxide?"
*Please show all work.
* if it's out of...

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)

The rate constant for the reaction 2N2O5(g) → 4NO2(g) + O2(g) is
equal to 3.41 x 10–5 s–1 at 30 ºC. If the initial concentration of
N2O5 is 0.446 M what concentration of NO2 will be observed after
175 minutes? Assume that initially no NO2 was present in the
reaction vessel.

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