Question

The first order constant is 4.82 x 10^{-3}
s^{-1} at 70C for the decomposition of the following
reaction: 2N_{2}O_{5} (g) -> 4NO_{2} +
O_{2} (g)

Suppose that you start with .0175M of N_{2}O_{5}
(g)

a.) What is the molarity of N_{2}O_{5} that
remains after 15 minutes (note: the rate constant is in
seconds)

b.) How many seconds will it take for the quantity of
N_{2}O_{5} to drop to .015M?

c.) What is the half life of N_{2}O_{5} at
70C?

Answer #1

a) K = (2.303 /t) log [A] / [A]

[A_{0}] = 0.0175 M , [A] = ?

t = 15 min = 900 s

K = 4.82 x 10^{-3} s^{-1}

4.82 x 10^{-3} = (2.303 / 900) log [0.0175] /
[A]

1.88 = - 1.76 - log [A]

log [A] = -3.64

**[A] = 0.00023 M**

b) [A] = 0.015 M , t = ?

4.82 x 10^{-3} = (2.303 / t) log [0.0175] /
[0.015]

4.82 x 10^{-3} = (2.303 /t) 0.067

2.303 / t = 0.072

**t = 32 s**

c) for first order reaction

t_{1/2} = 0.693 / K = 0.693 / 0.00482

**t _{1/2} = 143.8
s**

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 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
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How many minutes will it take for the quantity of N2O5 to drop
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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,
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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 rate constant for the first-order decomposition of
N2O5 by the reaction
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?

The following data are obtained for the decomposition of N2O5 at
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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 decomposition of hydrogen peroxide (H2O2) is a first order
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(a) What is the half life (in hours) for the reaction at
20°C?
(b) What is the molarity of H2O2 after four half lives if the
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(c) How many hours will it take for the concentration to drop to
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*Help please!!!*

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
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c.Calculate the concentration of
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