Answer:
The amount of heat released by the combustion of 2 moles of methane = 1605.1 kJ
Option 3 is correct.
ΔH°(combustion of 2 moles of methane)
= -1,605.1 kJ
Explanation:
The balanced equation for the combustion of methane is presented as
CH₄ + 2O₂ → CO₂ + 2H₂O
The heat of formation for the reactants and products are
CH₄ (g): ΔHf = –74.6 kJ/mol;
CO₂ (g): ΔHf = –393.5 kJ/mol;
and H₂O(g): ΔHf = –241.82 kJ/mol.
ΔHf for O₂ = 0 kJ/mol
ΔH°rxn for the combustion of methane is given as
ΔH°rxn = ΣnH°(products) - ΣnH°(reactants)
ΣnH°(products) = (1×-393.5) + (2×-241.82)
= -877.14 kJ/mol
ΣnH°(reactants) = (1×-74.6) + (2×0)
= -74.6 kJ/mol
ΔH°rxn = -877.14 - (-74.6) = -802.54 kJ/mol
For 2 moles of methane, the heat of combustion = 2 moles × -802.54 kJ/mol
= -1,605.08 kJ = -1,605.1 kJ
Hope this Helps!!!
X rays are the correct answer :)
Answer:
why u blocked i fought we were mates
Explanation:
