Question

The rate constant for the decomposition of N2O5 is 7.78 × 10−7 at 273 K and 3.46 × 10−5 at T2. If the activation energy is 1027 kJ/mol, what is the final temperature? 2 N2O5(g) → 4 NO2(g) + O2(g)

Answer #1

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 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

Values of the rate constant for the decomposition of N2O5 at
four different temperatures are as follows: T(K) k(s^-1) 658 2.14 x
10^5 673 3.23 x 10^5 688 4.81 x 10^5 703 7.03 x 10^5 Determine the
activation energy of the decomposition reaction: _____kJ/mol
Calculate the value of the rate constant at 300 K. _____s^-1

The decomposition of NO2(g) occurs by the
following bimolecular elementary reaction.
2 NO2(g) → 2 NO(g) +
O2(g)
The rate constant at 273 K is 2.3 ✕ 10-12 L/mol · s,
and the activation energy is 111 kJ/mol. How long will it take for
the concentration of NO2(g) to decrease from an
initial partial pressure of 4.0 atm to 2.4 atm at 451 K? Assume
ideal gas behavior.

For the decomposition of gaseous dinitrogen pentoxide
(shownbelow), the rate constant is k = 2.8 10-3 s-1 at 60°C. The
initialconcentration of N2O5 is 2.31 mol/L. 2 N2O5(g) 4NO2(g) +
O2(g) (a) What is [N2O5] after 5.00 min? _____mol/L (b) What
fraction of the N2O5 has decomposed after 5.00 min?

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.
If the initial concentration of...

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.

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 ?

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?

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