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The combustion of methane is represented by the following chemical equation:

[tex]\[ \text{CH}_4(g) + 2\text{O}_2(g) \rightarrow \text{CO}_2(g) + 2\text{H}_2\text{O}(g) + \text{energy} \][/tex]

Is this reaction endothermic or exothermic?

[tex]\[ \square \][/tex]

Sagot :

GinnyAnswer
To determine whether the combustion of methane is endothermic or exothermic, let's closely examine the given chemical equation:

[tex]\[ CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(g) + \text{energy} \][/tex]

1. Understanding the Chemical Reaction:

- Reactants: Methane (CH[tex]\(_4\)[/tex]) and Oxygen (O[tex]\(_2\)[/tex]).
- Products: Carbon Dioxide (CO[tex]\(_2\)[/tex]), Water (H[tex]\(_2\)[/tex]O), and Energy.

2. Energy Consideration:

In any chemical reaction, the energy involving the breaking and forming of chemical bonds is crucial to determine if a reaction is endothermic or exothermic.

- Endothermic Reaction: This type of reaction absorbs energy from the surroundings, resulting in a net intake of energy. Such reactions feel cold to the touch as they require energy.

- Exothermic Reaction: This type of reaction releases energy to the surroundings, resulting in a net release of energy. Such reactions usually feel warm or hot to the touch as they release energy.

3. Given Information:

The chemical equation explicitly states that energy is produced as a product of the reaction. The inclusion of energy on the right side of the equation indicates that the reaction releases energy.

4. Conclusion:

Since the reaction produces energy and releases it into the surroundings, this indicates the reaction is exothermic.

Thus, the combustion of methane is an exothermic reaction.

[tex]\[ \boxed{\text{exothermic}} \][/tex]
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