Question
In: Chemistry
At 700 K acetaldehyde decomposes in the gas phase to methane and carbon monoxide. The reaction...
At 700 K acetaldehyde decomposes in the gas phase to methane and
carbon monoxide. The reaction
isCH3CHO(g)?CH4(g)+CO(g)
A sample of CH3CHO is heated to 700 K and the pressure is measured
as 0.20 atm before any reaction takes place. The kinetics of the
reaction are then followed by measurements of total pressure and
these data are obtained:
| t(s) | 0 | 1000 | 3000 | 7000 |
| PTotal (atm) | 0.20 | 0.22 | 0.24 | 0.28 |
Rate law --> Rate=??PCH3CHO?t=4.510?4atm?1?s?1PCH3CHO2
Find total pressure after 1.17104s
Solutions
Expert Solution
The reaction is:
CH3COH(g) ? CH4(g) + CO(g)
At t=0: 0.2 atm 0 0
A t=t: 0.2 -x x x
Ptotal= P(CH3COH) + P(CH4) +P(CO)= 0.2 - x + x + x = 0.2 + x
x = Ptotal -0.2 (atm)
At t=0 s: x = 0 atm ?P(CH3COH) = 0.2 atm
At t = 1000 s: x = 0.02 atm ?P(CH3COH) = 0.18 atm
At t = 3000 s: x = 0.04 atm ?P(CH3COH) = 0.16 atm
At t = 3000 s: x = 0.08 atm ?P(CH3COH) = 0.12 atm
The rate law of the reaction is: rate = r = -d{P(CH3COH)/dt = k
queen_honey_blossom answered 11 hours agoRelated Solutions
At 700 K acetaldehyde decomposes in the gas phase to methane and carbon monoxide. The reaction...
At 700 K acetaldehyde decomposes in the gas phase to methane and
carbon monoxide. The reaction is:
CH3CHO(g)→CH4(g)+CO(g)
A sample of CH3CHO is heated to 700 K and the pressure is measured
as 0.27 atm before any reaction takes place. The kinetics of the
reaction are then followed by measurements of total pressure and
these data are obtained:
t(s)
0
1000
3000
7000
PTotal (atm)
0.27
0.30
0.34
0.39
Find total pressure after 1.47×104 s .
At 700 K acetaldehyde decomposes in the gas phase to methane and carbon monoxide. The reaction...
At 700 K acetaldehyde decomposes in the gas phase to methane and
carbon monoxide. The reaction is: CH3CHO(g)→CH4(g)+CO(g) A sample
of CH3CHO is heated to 700 K and the pressure is measured as 0.11
atm before any reaction takes place. The kinetics of the reaction
are then followed by measurements of total pressure and these data
are obtained: t(s) 0 1000 3000 7000 PTotal (atm) 0.11 0.12 0.12
0.14
Find total pressure after 1.89×104 s .
Express your answer to...
At 700 K acetaldehyde decomposes in the gas phase to methane and carbon monoxide. The reaction...
At 700 K acetaldehyde decomposes in the gas phase to methane and
carbon monoxide. The reaction is:
CH3CHO(g)→CH4(g)+CO(g)
A sample of CH3CHO is heated to 700 K and the pressure is measured
as 0.47 atm before any reaction takes place. The kinetics of the
reaction are then followed by measurements of total pressure and
these data are obtained:
t(s)
0
1000
3000
7000
PTotal (atm)
0.47
0.55
0.65
0.75
a. Find the rate law.
1.
Rate=−ΔPCH3CHOΔt=6.0×10−4s−1PCH3CHO
2.
Rate=−ΔPCH3CHOΔt=3.0×10−4s−1PCH3CHO
3.
Rate=−ΔPCH3CHOΔt=9.0×10−4atm−1⋅s−1PCH3CHO2...
At 700 K acetaldehyde decomposes in the gas phase to methane and carbon monoxide. The reaction...
At 700 K acetaldehyde decomposes in the gas phase to methane and
carbon monoxide. The reaction is:
CH3CHO(g)→CH4(g)+CO(g)
A sample of CH3CHO is heated to 700 K and the pressure is measured
as 0.41 atm before any reaction takes place. The kinetics of the
reaction are then followed by measurements of total pressure and
these data are obtained:
t(s) 0 1000 3000 7000
PTotal (atm) 0.41 0.47 0.56 0.64
Find total pressure after 1.65×104 s .
At 700 K acetaldehyde decomposes in the gas phase to methane and carbon monoxide. The reaction...
At 700 K acetaldehyde decomposes in the gas phase to methane and
carbon monoxide. The reaction is:
CH3CHO(g)→CH4(g)+CO(g)
A sample of CH3CHO is heated to 700 K and the pressure is measured
as 0.43 atm before any reaction takes place. The kinetics of the
reaction are then followed by measurements of total pressure and
these data are obtained:
t(s)
0
1000
3000
7000
PTotal (atm)
0.43
0.50
0.59
0.68
Question:
Find total pressure after 1.39×104 s
.
Consider the decomposition of acetaldehyde (CH3CHO) into methane (CH4) and carbon monoxide (CO).
Consider the decomposition of acetaldehyde (CH3CHO)
into methane (CH4) and carbon monoxide (CO).CH3CHO → CH4 + COAn experiment is performed where the concentration of
acetaldehyde is measured at various time intervals, resulting in
the following data.Time (s)[CH3CHO] (M)0.00.24220.00.16840.00.12960.00.104(a) Using Excel (or similar software), graph the three types of
plots outlined below and enter the slope, y-intercept, and
R2 for each graph). Use the graph with the best linear
fit to determine the order of the reaction with respect to
CH3CHO....
At 700 K, CCl4 decomposes to carbon and chlorine. The Kp value for the decomposition is...
At 700 K, CCl4 decomposes to carbon and chlorine. The Kp value
for the decomposition is 0.76. Find the starting pressure of CCl4
at this temperature that produces a total pressure of 1.7 atm at
equilibrium.
Carbon monoxide reacts with steam to produce carbon dioxide and hydrogen. At 700 K the equilibrium...
Carbon monoxide reacts with steam to produce carbon dioxide
and hydrogen. At 700 K the equilibrium constant is 5.10. Calculate
the equilibrium concentrations of all species if 1.000 mole of each
component (reactants and products) is mixed in a 1.000 L flask.
(Note: Be sure to check Q to determine which way the reaction will
proceed to come to equilibrium). Please show step by step, I'm
lost. Thank you!
CO(g) + H2O(g) -> CO2(g) + H2(g)
Dinitrogen pentoxide decomposes in the gas phase to form nitrogen dioxide and oxygen gas. The reaction...
Dinitrogen pentoxide decomposes in the gas phase to form
nitrogen dioxide and oxygen gas. The reaction is first order in
dinitrogen pentoxide and has a half-life of 2.81 h at 25 ∘C.
If a 1.5-L reaction vessel initially contains 760 torr of N2O5
at 25 ∘C, what partial pressure of O2 is present in the vessel
after 225 minutes?
Dinitrogen pentoxide decomposes in the gas phase to form nitrogen dioxide and oxygen gas. The reaction...
Dinitrogen pentoxide decomposes in the gas phase to form
nitrogen dioxide and oxygen gas. The reaction is first order in
dinitrogen pentoxide and has a half-life of 2.81 h at 25 ∘C.
If a 1.7-L reaction vessel initially contains 760 torr of N2O5
at 25 ∘C, what partial pressure of O2 is present in the vessel
after 205 minutes?
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