Rate of reactions vs. HEat energy evolves per second inititally

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The reaction between nitrogen dioxide and carbon monoxide produces nitric oxide and carbon dioxide, with a rate law of k[NO2]^2, where the rate constant is 0.515 L/(mol*s). To calculate the heat energy evolving per second from a 3.50 L mixture containing 0.0250 M NO2, first determine the number of moles of NO2 present, which is 0.0875 moles. Using the enthalpy change of 33.1 kJ/mol, the heat energy can be calculated based on the moles reacting per second. If 1 mole of NO2 is produced per second, the energy released would be 33.1 kJ, and for 0.5 moles, it would be 16.55 kJ. The relationship between concentration, volume, and rate constant is crucial for determining the rate of reaction and subsequent heat energy release.
yannguyen
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Nitrogen dioxide reacts with carbon monoxide by the overall equation:

NO2(g) + CO(g) ----> NO(g)+ CO2(g)

At a particular temperature, the reaction is second order In NO2 and zero order in CO. The rate constant is 0.515 L/(mol*s). How much heat energy evolves per second initially from 3.50 L of reaction mixture containing .0250 M NO2?

Assume the enthalpy change is constant with temperature.How much heat energy evolves per second initially from 3.50 L of reaction mixture containing .0250 M NO2?

I figured out the rate law for this = k[NO2]^2
The enthalpy change for NO2 is 33.1 kJ/mol
However I don't really understand how the concentration, the volume, and the rate constant would relate to find out the heat energy?

Should i find the number of moles of NO2 or what should I do? I totally have no idea about this!

Any help would be highly appreciate
 
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How much energy would evolve during a second if there were 1 mole of NO2 produced per second? And if there were 0.5 mole produced? And if there were n moles produced?
 

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