1mol of an organic compound requires 3mol of oxygen gas

AI Thread Summary
The discussion centers on identifying the formula of an organic compound that requires 3 moles of oxygen gas for complete oxidation, interpreted as combustion. Participants confirm that complete oxidation refers to combustion processes. The organic compounds listed for consideration include CH3CHO, CH3CH2OH, CH3CH3, and CH3CO2H. The focus is on understanding the stoichiometry involved in combustion reactions. The conclusion emphasizes the need to analyze the molecular structure of each compound to determine which one fits the oxidation requirement.
elitewarr
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Homework Statement


For complete oxidation, 1mol of an organic compound requires 3mol of oxygen gas
What could be the formula?
a) CH3CHO
b) CH3CH2OH
c) CH3CH3
d) CH3CO2H


Homework Equations





The Attempt at a Solution


What does it mean by complete oxidation? Is it combustion?
 
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elitewarr said:

Homework Statement


For complete oxidation, 1mol of an organic compound requires 3mol of oxygen gas
What could be the formula?
a) CH3CHO
b) CH3CH2OH
c) CH3CH3
d) CH3CO2H


Homework Equations





The Attempt at a Solution


What does it mean by complete oxidation? Is it combustion?

Yes it is combustion.
 


chemisttree said:
Yes it is combustion.

Thank you.
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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