Consider the following redox reaction: Fe(s) + 2 HCI(aq) FeCl2(aq) + H2(g) Which of the following statements are true? (Check all correct answers.) Chlorine (CI) is being reduced Fe(s) is being oxidized The oxidation state of iron in FeCl, is +2 The oxidation state of each Cl atom in FeCl2 is -2 Hydrogen is being reduced The oxidation state of hydrogen in H2(g) is +1

I think you forgot one. Thank you.

What actually happens in a single displacement reaction of the type: + 2 AGNO3 (aq) cu (s) → 2 Ag(s) + Cu(NO3)2 (aq) a. one metal atom loses its electrons b. one metal ion gains electrons C. metal atoms force their electrons onto metallic ions d. metallic ions accept electrons from polyatomic ions Which of the following is the rule when using metals in the metal activity serie a. a more active metallic ion can displace a less active metallic ion O b. a more active metallic ion can displace a less active metal atom C. a more active metal atom can displace a less active metal atom da more active metal atom can disnlace a less active metallic ion M lyp

4) Zinc metal reacts with hydrochloric acid (HCl) according to the reaction: Zn (s) + 2HCl (aq) ------> ZnCl2 (aq) + H2 (g) a) Is this a redox reaction? b) If so, tell what is reduced and what is oxidized?