Question
In: Chemistry
The decomposition of N2O5(g) —> NO2(g) + NO3(g) proceeds as a first order reaction with a...
The
decomposition of N2O5(g) —> NO2(g) + NO3(g) proceeds as a first
order reaction with a half life 30.0s at a certain temperature.
If the initial concentration [N2O5]0 = 0.400 M, what is the
concentration after 120 seconds?
A)0.050
B)0.200
C)0.025
D)0.100
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
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 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 reaction: N2O5 (g) NO3 (g) + NO2 (g) a. Determine the rate order by plotting...
The reaction: N2O5 (g)
NO3 (g) +
NO2 (g)
a. Determine the rate order by plotting the data.
(Hint: Which plot gives a straight line? Conc vs time, ln(conc)
vs time, or 1/conc vs time)
b. Predict the concentration of N2O5 at 250 seconds.
Time (s) [N2O5]
0 1.00
25 0.822
50 0.677
100 0.557
125 0.458
150 0.377
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...
A proposed mechanism for the reaction N2O5-->2NO2 +1/2O2 N2O5 k1--> NO2+NO3 <---k_1-- NO2 +NO3 --k2--> NO...
A proposed mechanism for the reaction N2O5-->2NO2 +1/2O2
N2O5 k1--> NO2+NO3 <---k_1-- NO2 +NO3 --k2--> NO +O2
+NO2 NO +NO3 - k3-->2NO2
Applying the steady-state approximation to show that the overall
reaction rate is -d[N2 O5 ]/dt=k[N2 O5 ] In this process you should
evaluate K in terms of K1, K_1, K2 and K3
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).
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