Calculate the approximate enthalpy change, δhrxn, for the combustion of one mole of methane a shown in the balanced chemical equation: ch4+2o2→2h2o+co2 use the values you calculated in parts a, b, c, and d, keeping in mind the stoichiometric coefficients

To solve for the enthalpy of reaction, we apply the Hess's Law.

ΔHrxn = ∑(ν×Hf of products) - ∑(ν×Hf of reactants)
where
v is the stoichiometric coefficient determined from the balanced reaction
Hf is the standard heat of formation; these are empirical values:
*For CH₄: Hf = −74.87 kJ/mol
*For O₂: Hf = 0
*For CO₂: -393.5 kJ/mol 
*For H₂O: -241.82 kJ/mol

ΔHrxn = [(2*-241.82 kJ/mol)+(1*-393.5 kJ/mol)] - [(1*−74.87 kJ/mol)+(2*0 kJ/mol)] = -802.27 kJ/mol

The answer is b on plato.

A. ​it generates energy from carbohydrates.b. it requires activation by oxygen.​c. ​it is used by cells to dispose of excess electrons