Problem: Consider the combustion of a single molecule of CH4(g) forming H2O(l) as a product.How much energy, in J, is produced during this reaction?

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Reaction will appear as:

CH(g) + 2 O(g)  → CO2 (g) + 2 H2O (g)Calculate ΔHrxn by accounting the bonds in the product and reactants:

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Consider the combustion of a single molecule of CH4(g) forming H2O(l) as a product.

How much energy, in J, is produced during this reaction?

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