Question
In: Chemistry
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...
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 2.80×10−2 mol of N2O5(g) in a volume of 2.2 L .
How many moles of N2O5 will remain after 6.0 min ?
How many minutes will it take for the quantity of N2O5 to drop to 1.6×10−2 mol ?
What is the half-life of N2O5 at 70∘C?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
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...
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 2.0 L .
1. How many moles of N2O5 will remain after 4.0 min ?
2. How many minutes will it take for the quantity of N2O5 to
drop to 1.6×10−2 mol ?
3. 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 70C is 6.82x10^-3 s^-1....
the first order rate constant for the decomposition of N2O5,
2N2O5(g)->4NO2(g)+O2(g)
at 70C is 6.82x10^-3 s^-1. suppose we start with 3.00x10^-2 mol
of N2O5(g) in a volume of 2.3L
A) how many moles of N2O5 will remain after 3.0 min?
B) how many minutes will it take for the quantity of N2O5 to
drop to 1.7x10^-2 mol?
C) what is the half-life of N2O5 at 70C?
The decomposition of N2O5 is described by the following equation. 2N2O5(g) → 4NO2(g) + O2(g) If...
The decomposition of N2O5 is described by the following
equation. 2N2O5(g) → 4NO2(g) + O2(g) If the rate constant is 4.50 ×
10−4 s−1, what is the half-life of this reaction? × 10 s in
scientific notation
The reaction 2A → B is second order with a rate constant of
51.0/M·min at 24°C. (a) Starting with [A]0 = 9.30 × 10−3 M, how
long will it take for [A]t = 2.90 × 10−3 M? min (b) Calculate the
half-life of...
The rate constant for the 1st order decomposition of N2O5 in the reaction 2N2O5 (g) ...
The rate constant for the 1st order decomposition of N2O5 in the
reaction 2N2O5 (g) 4NO2 (g) + O2 (g) is k=3.38x 10-5 s-1 at
25oC.
a. What is the half-life of N2O5?
b. What will be the total pressure, initially 88.3 kPa for the pure
N2O5 vapor, (1) 10s and
(2) 10 min after initiation of the reaction?
(Hint: partial pressure is proportional to concentration).
The specific rate constant for the first-order decomposition of N2O5(g) to NO2(g) and O2(g) is 7.48×10−3s−1...
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 0.150 atm .
B. 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 .
C. Find...
The specific rate constant for the first-order decomposition of N2O5(g) to NO2(g) and O2(g) is 7.48×10−3s−1...
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.
1. Find the length of time required for the total pressure in a
system containing N2O5 at an initial pressure of 0.110 atm to rise
to 0.220 atm .
The specific rate constant for the first-order decomposition of N2O5(g) to NO2(g) and O2(g) is 7.48×10−3s−1...
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.
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
0.220 atm .
The specific rate constant for the first-order decomposition of N2O5(g) to NO2(g) and O2(g) is 7.48×10−3s−1...
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.
Part 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 0.155 atm .
Express your answer using two significant figures.
t=_______ s
Part B
Find the length of time required for the total pressure in a
system containing N2O5 at an initial pressure...
The specific rate constant for the first-order decomposition of N2O5(g) to NO2(g) and O2(g) is 7.48×10−3s−1...
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.
1)Find the length of time required for the total pressure in a
system containing N2O5 at an initial pressure of 0.110 atm to rise
to 0.150 atm .
2)Find the length of time required for the total pressure in a
system containing N2O5 at an initial pressure of 0.110 atm to rise
to 0.200 atm .
use the steady state approximation 2N2O5 (g) → 4NO2 (g) + O2 (g) The mechanism is based on: N2O5 →...
use the steady state approximation
2N2O5 (g) → 4NO2 (g) + O2 (g)
The mechanism is based on:
N2O5 → NO2 +
NO3 ka
NO2 + NO3 →
N2O5 k'a
NO2 + NO3 → NO2 +
O2 +NO kb
NO + N2O5 → NO2 + NO2 +
NO2 kc
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