How Much Heat is Released When Carbon Reacts with Oxygen?

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To determine the heat released when 4.72 g of carbon reacts with excess oxygen, first calculate the number of moles of carbon using its molar mass. The reaction releases 393.5 kJ of heat per mole of carbon consumed. After finding the moles of carbon, multiply by the heat released per mole to find the total heat output. The limiting reagent is not a concern here since excess O2 is present. This approach will yield the total heat released in kilojoules.
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I am struggling with a recent chemistry lesson. Immediate help is needed and would be greatly appreciated. I know that we have to first find the limiting reagent, and then go on to determine the heat released in kiloJoules.

Homework Statement



How much heat will be released when 4.72 g of carbon reacts with excess O2 according to the following equation?

Homework Equations



C + O2 --> CO2 (Delta) H = -393.5 kJ

The Attempt at a Solution

 
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How many moles of C are there in 4.72g?
The equation says you get 393.5kJ for each mole.
 
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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