13. The kinetics of the oxidation of ethanol (C2H5OH) with dichromate (Cr2O72-) in acidic medium (H+) was studied. The table below summarizes the initial rates in four separate reactions where different initial concentrations of the reactants were used. What is the rate law for this reaction? (5 points) Cr₂0 + 3 C2H5OH + 8H+ → 2 Cr3+ + 3 CH3CHO + 7 H₂O ->>> [Cr₂0]/M [C2H5OH]/M [H+]/M (rate), /Ms-1 0.273 0.404 0.375 3.26 0.819 0.404 0.375 9.77 0.273 0.808 0.375 13.0 0.273 0.404 0.750 6.52 a) rate = = k[C₂H5OH][Cr2O7²¯][H+] b) rate = k[C₂H5OH]2[Cr₂O,²¯][H+] c) rate = k[C₂H5OH][Cr₂07²-]² [H+] d) rate = k[C₂H5OH]² [Cr₂O,²-] e) rate = = k [Cr₂07²¯]² [H+]²
13. The kinetics of the oxidation of ethanol (C2H5OH) with dichromate (Cr2O72-) in acidic medium (H+) was studied. The table below summarizes the initial rates in four separate reactions where different initial concentrations of the reactants were used. What is the rate law for this reaction? (5 points) Cr₂0 + 3 C2H5OH + 8H+ → 2 Cr3+ + 3 CH3CHO + 7 H₂O ->>> [Cr₂0]/M [C2H5OH]/M [H+]/M (rate), /Ms-1 0.273 0.404 0.375 3.26 0.819 0.404 0.375 9.77 0.273 0.808 0.375 13.0 0.273 0.404 0.750 6.52 a) rate = = k[C₂H5OH][Cr2O7²¯][H+] b) rate = k[C₂H5OH]2[Cr₂O,²¯][H+] c) rate = k[C₂H5OH][Cr₂07²-]² [H+] d) rate = k[C₂H5OH]² [Cr₂O,²-] e) rate = = k [Cr₂07²¯]² [H+]²
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Chapter13: Rates Of Reaction
Section: Chapter Questions
Problem 13.51QP: In experiments on the decomposition of azomethane. CH3NHCH3(g)C2H6(g)+N2(g) the following data were...
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![13. The kinetics of the oxidation of ethanol (C2H5OH) with dichromate (Cr2O72-) in acidic medium
(H+) was studied. The table below summarizes the initial rates in four separate reactions where
different initial concentrations of the reactants were used. What is the rate law for this reaction?
(5 points)
Cr₂0 + 3 C2H5OH + 8H+ → 2 Cr3+ + 3 CH3CHO + 7 H₂O
->>>
[Cr₂0]/M
[C2H5OH]/M
[H+]/M
(rate), /Ms-1
0.273
0.404
0.375
3.26
0.819
0.404
0.375
9.77
0.273
0.808
0.375
13.0
0.273
0.404
0.750
6.52
a) rate = = k[C₂H5OH][Cr2O7²¯][H+]
b) rate = k[C₂H5OH]2[Cr₂O,²¯][H+]
c) rate = k[C₂H5OH][Cr₂07²-]² [H+]
d) rate = k[C₂H5OH]² [Cr₂O,²-]
e) rate = = k [Cr₂07²¯]² [H+]²](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff15267d6-b61d-436d-a58e-82820b6d50d3%2Fa266b917-de01-4014-9114-4a9fab6142e3%2F0wu0uv_processed.jpeg&w=3840&q=75)
Transcribed Image Text:13. The kinetics of the oxidation of ethanol (C2H5OH) with dichromate (Cr2O72-) in acidic medium
(H+) was studied. The table below summarizes the initial rates in four separate reactions where
different initial concentrations of the reactants were used. What is the rate law for this reaction?
(5 points)
Cr₂0 + 3 C2H5OH + 8H+ → 2 Cr3+ + 3 CH3CHO + 7 H₂O
->>>
[Cr₂0]/M
[C2H5OH]/M
[H+]/M
(rate), /Ms-1
0.273
0.404
0.375
3.26
0.819
0.404
0.375
9.77
0.273
0.808
0.375
13.0
0.273
0.404
0.750
6.52
a) rate = = k[C₂H5OH][Cr2O7²¯][H+]
b) rate = k[C₂H5OH]2[Cr₂O,²¯][H+]
c) rate = k[C₂H5OH][Cr₂07²-]² [H+]
d) rate = k[C₂H5OH]² [Cr₂O,²-]
e) rate = = k [Cr₂07²¯]² [H+]²
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