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Question
Nitrogen dioxide reacts with carbon monoxide to produce nitrogen monoxide and carbon dioxide.
NO2(g) + CO(g) NO(g) + CO2(g)
A proposed mechanism for this reaction is
2 NO2(g) 
NO3(g) + NO(g) (fast, equilibrium)
NO3(g) + CO(g) NO2(g) + CO2(g) (slow)
What is a rate law that is consistent with the proposed mechanism?
A.rate = k[NO2]2[CO] [NO]-1
B.rate = k[NO2]2[CO]
C.rate = k[NO2][CO]
D.rate = k[NO3][CO]
E.rate = k[NO2]2
Answer
This answer is hidden. It contains 2 characters.
Related questions
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H2O2(aq) H2O() + 1/2 O2(g)
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What is the distance, in atomic radii, along any edge of a body-centered unit cell?
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Which equation represents the number of atoms in a body-centered cubic unit cell?
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Q:
The solubility product equilibrium constant, Ksp, of silver bromide is 5.4 10-13 at 298 K.
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Q:
What is the equilibrium constant for reaction below at 25 C? (R = 8.314 J/Kmol)2 NO(g) + O2(g) 2 NO2(g)given DfG [NO(g)] = +86.6 kJ/mol and DfG [NO2(g)] = +51.2 kJ/mol.A.3.9 10-13B.1.0C.2.6 1012D.1.6 106E.3.8 1028
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All of the following relationships are true EXCEPT
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Q:
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Q:
If a chemical reaction is exothermic, but not spontaneous, which of the following must be true?
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B.DrG < 0, DrS > 0 and DrH > 0
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