This is a more specific version of the previous question. What specific atom was

Question

This is a more specific version of the previous question. What specific atom was oxidized in the following equation? Which specific atom was reduced? Finally identify the oxidizing agent and the reducing agent. 6HCl(aq) + 2Fe(s) rightarrow 2FeCl_3(aq) + 3H_2(g) What is being oxidized? H^+ ions are being oxidized The H atoms inside H_2(g) are being oxidized Cl^- ions are being oxidized The Cl atoms inside Cl^2 (g) are being oxidized Fe(s) atoms are being oxidized Fe^3+ ions are being oxidized What is being reduced? H^+ ions are being oxidized The H atoms inside H_2(g) are being oxidized Cl^- ions are being oxidized The Cl atoms inside Cl^2 (g) are being oxidized Fe(s) atoms are being oxidized Fe^3+ ions are being oxidized What is the oxidizing agent? HCl (aq) Fe (s) FeCl_3 (aq) H_2 (g) What is the reducing agent HHCl (aq) Fe (s) FeCl_3 (aq) H_2 (g)

Explanation / Answer

OXidation: Fe since it goes from 0 to +2, it loses electrons

Reduction: H since it goes form +1 to 0, it gians electrons, therefore reduces

oxidizing agent --> HCl(aq)

reducing agnet -> Fe(s)

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