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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.

Respuesta :

superman1987

Answer:

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.

pstnonsonjoku

The reaction is exothermic as one mole of methane (CH4) releases 890 kJ of energy.

In a chemical reaction, heat could be absorbed or emitted.

  • When heat is absorbed in a chemical reaction, it is an endothermic reaction
  • When heat is emitted in a chemical reaction, it is an exothermic reaction.

Hence, for the reaction shown, CH4(g) + 2O2(g) → CO2(g) + 2H2O(l): ΔH = −890 kJ, we can see clearly that the reaction of one mole  of methane (CH4) releases 890 kJ of energy.

Learn more about exothermic reaction: https://brainly.com/question/4345448

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