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

Which statement about this reaction is correct?

The reaction of one mole of oxygen (O2) absorbs 445 kJ of energy.

The reaction of one mole of oxygen (O2) releases 445 kJ of energy.

The reaction of one mole of methane (CH4) absorbs 890 kJ of energy.

The reaction of two moles of methane (CH4) releases 890 kJ of energy.

The reaction of one mole of oxygen (O2) releases 445 kJ of energy.

Explanation:

Firstly, the reaction is exothermic since the sign of enthalpy change ΔH is negative.

The balanced equation: CH₄ (g) + 2O₂ (g) → CO₂ (g) + 2H₂O (l) : ΔH = - 890 kJ,

Shows that 1 mole of CH₄ react with 2 moles of oxygen and releases 890 kJ.

So, every choice says that absorb is wrong (choice 1& 3).

Choice no. 4 is wrong since it says that 2 moles of methane releases 890 kJ, because only one mole release this amount of energy.

So, the right choice is The reaction of one mole of oxygen (O2) releases 445 kJ of energy.