Chemistry · Electrochemistry
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Choose the true statement regarding the reaction given below
2Na(g) + Cl2(g)--> 2NaCl(s)
- A
Chloride is oxidized and sodium is reduced
- B
Chlorine acts as an oxidizing agent and sodium as a reducing agent
- C
Chlorine acts as a reducing agent
- D
None of the above
In the reaction 2Na(s) + Cl2(g) ⟶ 2NaCl(s), sodium (Na) is oxidized to Na+, losing electrons, and thus acts as the reducing agent. Chlorine (Cl₂) is reduced by gaining electrons to form Cl⁻, acting as the oxidizing agent. Therefore, the correct answer is Option B. Options A and C incorrectly describe the roles of chloride and chlorine, and Option D is incorrect because Option B is the accurate description of the reaction.
Incorrect. Chloride (Cl⁻) is not oxidized, and sodium (Na) is not reduced. Chlorine (Cl₂) is reduced and sodium is oxidized in this reaction.
Correct. In this reaction, sodium (Na) loses electrons and is oxidized, acting as the reducing agent. Chlorine (Cl₂) gains electrons and is reduced, acting as the oxidizing agent.
Incorrect. Chlorine is reduced in the reaction, meaning it gains electrons and acts as an oxidizing agent, not a reducing agent.
Incorrect. Option B correctly describes the roles of chlorine and sodium in the reaction.
Tagged under Chemistry · Electrochemistry · 2016