consider the following oxidation-reduction reaction : 2 Fe 3+(aq) + 2 Hg (l) + 2
ID: 1000858 • Letter: C
Question
consider the following oxidation-reduction reaction :
2 Fe 3+(aq) + 2 Hg (l) + 2Cl- (aq)
-----> 2Fe 2+ (aq) + Hg2Cl2 (s)
Which one of the following pairs correctly indicates the oxidizing agent and reducing agent in this reaction? Please give me step by step with clearly legible instructions thank you
LOn3ider the tollowing oxidation-reduction rexction: ich one of the following pairs comceily indicates thc uxidizing ageni and the reducing agent u xidizing agent Reducing agent IIg) Hg(D) Fe(ag) Fe(ag) Cr(ag) a) Hain Fe (aq) c(ag) 2Fe:-(aq) + 2Hg +2Cl (aq) 2Fe-Taq) Consider the following reaction: Fe (ay) is the reducing agent. Fe (aq) is the reducing agent. Fe"(ag) loses electrons. Hg(0) loses electrons.Explanation / Answer
The correct pair is [ oxidizing agent : Fe3+(aq), reducing agent: Hg(l) ]
In this reaction Fe3+ got reuced to Fe2+. means it itself recuced and it oxidises the Hg0 to Hg+ in (Hg2Cl2).
Hg0(l) got oxidised itself to Hg+ to reduce Fe3+ to Fe2+.
Therfore Fe3+(aq) is an oxidizing agent and Hg(l) is a reducing agent:
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