Solving a Chemistry Problem: Moles of Oxygen Required to Burn Octane

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To determine the moles of oxygen required to burn 5.00 moles of octane (C8H18), the balanced equation shows that 2 moles of octane react with 50 moles of oxygen. Therefore, for 5.00 moles of octane, 125 moles of oxygen are needed. The discussion includes a check on whether the oxygen is balanced in the equation, confirming that it is indeed balanced. Participants express confusion over their calculations, indicating a need for clarity in stoichiometric relationships. Understanding these relationships is crucial for solving chemistry problems accurately.
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Homework Statement



2 C8 H18 + 50 O2 --> 16 C O2 + 18 H2 O

How many moles of oxygen are required to burn 5.00 moles of octane?

I got 125?

Homework Equations





The Attempt at a Solution

 
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Check if the oxygen is balanced.

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Is it?

How many atoms on the left? How many atoms on the right?

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methods
 
Oh sorry my mistake, borek
thats why I'm getting bad results for chemistry, eh? :S
 
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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