Question

Identify the reducing agent in the following reaction:
\[ \mathrm{CH_4(g) + O_2(g) \rightarrow CO_2(g) + 2H_2O(l)} \]

• A. \(\mathrm{CO_2(g)}\)
• B. \(\mathrm{H_2O(l)}\)
• C. \(\mathrm{O_2(g)}\)
• D. \(\mathrm{CH_4(g)}\)

Hint:

The substance that gets oxidized always acts as the reducing agent.

Answer 1

The Correct Option is D

Step 1: Recall definition of reducing agent.
A reducing agent is the substance that undergoes oxidation by losing electrons.
Step 2: Analyze oxidation states.
In \(\mathrm{CH_4}\), carbon has oxidation state \(-4\).
In \(\mathrm{CO_2}\), carbon has oxidation state \(+4\).
Step 3: Identify the oxidized species.
Carbon in methane is oxidized from \(-4\) to \(+4\), hence methane undergoes oxidation.
Step 4: Conclusion.
Therefore, \(\mathrm{CH_4}\) acts as the reducing agent in the reaction.