Question
In: Chemistry
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 .
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
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.
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 .
The decomposition of n2o5 is a first order reaction. N2o5 decomposes to yield no2 and o2....
The decomposition of n2o5 is a first order reaction. N2o5
decomposes to yield no2 and o2.
At 48deg C the rate constant for the reaction is 1.2x10^-5s^-1.
Calculate the partial pressure of no2 produced from 1.0L of 0.700M
n2o5 solution at 48deg C over a period of 22 hours if the gas is
collected in a 10.0L container. Show work please.
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 following reaction is first order in N2O5: N2O5(g)→NO3(g)+NO2(g) The rate constant for the reaction at...
The following reaction is first order in N2O5:
N2O5(g)→NO3(g)+NO2(g)
The rate constant for the reaction at a certain temperature is
0.053/s.
A. Calculate the rate of the reaction when [N2O5]=
5.9×10−2 M.
B. What would the rate of the reaction be at the same
concentration as in Part A if the reaction were second order?
(Assume the same numerical value for the rate constant
with the appropriate units.)
C. What would the rate of the reaction be at the same...
The following reaction is first order in N2O5: N2O5(g)?NO3(g)+NO2(g) The rate constant for the reaction at...
The following reaction is first order in N2O5:
N2O5(g)?NO3(g)+NO2(g)
The rate constant for the reaction at a certain temperature is
0.053/s.
A)
Calculate the rate of the reaction when [N2O5]= 5.4
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 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?
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