Question
In: Chemistry
consider the reaction 4NO2(g) + O2(g) ---> 2N2O5(g) At a particular time during the reaction, nitrogen...
consider the reaction 4NO2(g) + O2(g) ---> 2N2O5(g) At a particular time during the reaction, nitrogen dioxide is being consumed at the rate of 0.0013 M/s. At what rate is molecular oxygen being consumed?
Solutions
Expert Solution
Rate eq for the reaction:
4NO2(g) + O2(g) ---> 2N2O5(g)
-1/4d[NO2]/dt = -d[O2]/dt = +d[N2O5]/dt
From here:
rate of consumption of molecular oxygen: d[O2]/dt = 1/4d[NO2]/dt
= 0.0013/4
= 0.000325 = 3.25 x 10-4 M/s
queen_honey_blossom answered 2 years agoRelated Solutions
For 2N2O5(g) = 4NO2(g) + O2(g) 1. Determine, by making the appropriate graphs, whether this decomposition reaction...
For 2N2O5(g) = 4NO2(g) +
O2(g)
1. Determine, by making the appropriate graphs,
whether this decomposition reaction is zero, first, or second order
with respect to N2O5
I found by makin the graph in excel that it was a first order
reaction
Now here are my questions
2. The stoichiometric coefficient for N205 in the reaction
equation is 2. Depending on your answer to Problem 1, explain why
the reaction order you obtained in Problem 1 is also 2, or explain...
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...
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
In the gas phase, N2O5 decomposes according to the following reaction 2N2O5 (g) --> 4NO2 (g)...
In the gas phase, N2O5 decomposes according to the following
reaction
2N2O5 (g) --> 4NO2 (g) + O2 (g)
We put some N2O5 (g) in a container and it has a pressure of
0.154 atm. After the reaction proceeds for 103 seconds, the total
pressure has increased to 0.260 atm. Assuming constant temperature
and volume, the average rate of disappearance of the N2O5 (g)
during this time interval is
answer is: 1.0 x 10^-3 atm/s
Please show work :D
Consider the reaction 2N2O(g) + 3O2 (g) ⇌ 4NO2 (g). Exactly 0.0560 mol of O2 and...
Consider the reaction 2N2O(g) + 3O2 (g) ⇌ 4NO2 (g). Exactly
0.0560 mol of O2 and 0.020 mol of N2O were placed into a 500 mL
flask. The equilibrium concentration of NO2 was 0.020 M. What is
the value of Kc for this reaction? Report your answer to the
correct number of significant figures.
For the reaction 3O2(g) + 4NO(g)-->2N2O5(g) the rate of change in concentration of O2, delta[O2]/deltat =...
For the reaction 3O2(g) + 4NO(g)-->2N2O5(g)
the rate of change in concentration of O2, delta[O2]/deltat =
0.057 mol/L.sec. What is the rate of change of NO and what is the
rate of change of N2O5? Show your calculations.
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 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?
Consider this reaction: H2(g) + O2 (g) à H2O (g)  
Consider this reaction:
H2(g) +
O2 (g) à
H2O (g)
dHo = __________
Balance the equation and put the correct number of moles in the
equation above. (1 point)
Classify the forward reaction as (1) Combustion, (2)
Decomposition, (3) Single replacement, (4) Double replacement, (5)
Neutralization, (6) Synthesis. Circle the correct answer. (1
point)
In this reaction did Hydrogen get oxidized or reduced? Circle
the correct answer. (1 point)
Based on your answer above is Hydrogen an...
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