Question

CH4(g) + 2O2 (g) →CO2(g) + 2H2O (l), ΔH = -890kj/mol
Calculate much heat is released when 3.5 moles of methane gas undergo a combustion reaction

Answer 1

A combustion reaction is a reaction that reacts with oxygen to produce the product. 3.5 moles of methane release - 3115 kJ/mol of heat.  

What is a combustion reaction?

A combustion reaction is a chemical reaction that involves the burning of the reactant in the presence of the oxygen molecule to release heat.

The balanced reaction of methane combustion is given as:

CH₄(g) + 2O₂ (g) → CO₂(g) + 2H₂O (l), ΔH = -890 kJ/mol

From the reaction, it can be said that 1 mole of methane combusts to produce -890kJ/mol enthalpy.

So, 3.5 moles will produce, 3.5 × -890kJ/mol = - 3115 kJ/mol.

Therefore, 3.5 moles of methane produce - 3115 kJ/mol heat.

Learn more about combustion reaction here:

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