Write balanced half-reactions for the following redox reaction: 4 Cl2(g)+ AsH 3(g)+4H,0(1) → 8 Ci (aq)+H3A$O4(aq)+ 8 H¯ (aq) reduction: 4Ci, (g) + 2e → 8C1 (aq) oxidation:

Electrolysis is the process of using electrical current to cause a nonspontaneous reaction to occur. For example, water molecules do not readily decompose into hydrogen and oxygen. However, water can be decomposed using electrolysis according to the reaction 2 H₂O(1)→ 2H₂(g) + O₂(g) Because electrolysis involves the transfer of electrons, it is classified as a type of oxidation-reduction (redox) reaction. For the given reaction, identify which atoms are oxidized and which are reduced. Which atoms are oxidized? Both oxygen atoms in O₂(g). The oxygen atom in H₂O(1). Both hydrogen atoms in H₂(g). Both hydrogen atoms in H₂O(1). MacBook Pro Which atoms are reduced? Both hydrogen atoms in H₂(g). The oxygen atom in H₂O(1). Both hydrogen atoms in H₂O(1). Both oxygen atoms in O₂(g).

Which of the following is an oxidation-reduction reaction? OHCl(aq) + LiOH(aq) → LiCl(aq) + H₂O(1) Nal(aq) + AgNO3(aq) → Agl(s) + NaNO3(aq) Pb(C₂H3O2)2(aq) + 2 NaCl(aq) → PbCl2(s) + 2 NaC₂H3O₂(aq) Mg(s) + 2 HCl(aq) → MgCl₂(aq) + H₂(g) All of these are oxidation-reduction reactions.

How do we solve this redox reaction?

Write balanced half-reactions for the following redox reaction: 8 CO₂(aq) + AsH3(g)+8 OH¯(aq) → 4C₂0¾¯(aq) + H₂AsO 4(aq) + 4H₂O(1) reduction: 0 oxidation: ロ→ロ e X S

Write balanced half-reactions for the following redox reaction: 2+ 4 Zn²+ (aq) + AsH₂(g) +8 OH(aq) 4 Zn(s) + H₂ AsO4(aq) + 4H₂O(1) reduction: oxidation:

Balance the following oxidation-reduction reaction that occurs in an acidic solution using the half-reaction method. I(aq) + Clo-(ag) → I3¯(aq) + CI-(aq) HOW DO WE GET THERE? For the reduction half-reaction, which half-reaction correctly balances the elements on both sides? ClO (aq) + H2O(1) → CI-(aq) + 2 H*(aq) clo-(aq) → Cl-(aq) 2 H+(aq) + ClO-(aq) → Cl-(aq) + H20(I) Clo-(aq) → CI-(aq) + H20(1) Clo-(aq) → Cl(aq) + H20(1) + 2 H*(aq) Check Next (4 of 6)

Balance the following redox equation, for a reaction which takes place in basic solution. HS (aq) + ClO3(aq) → S(s) + Cl(aq) (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) - HS (aq) + ClO3(aq) + S(s) Cl(aq) +

Write balanced half-reactions for the following redox reaction: 3+ Fe³+ (aq) +NO₂(g) +H₂O(l) reduction: oxidation: 2+ Fe²(aq)+NO3(aq) + 2 H+ (aq)

Use the relative strengths of nonmetals and metals as oxidizing and reducing agents, as indicated in the following unbalanced equations, to construct a table of half‐reactions. Ag (s) + Br2 (l) → AgBr (s) Ag (s) + I2 (s) → no evidence of reaction Cu2+ (aq) + I‐ (aq) → no redox reaction Br2 (l) + Cl‐ (aq) → no evidence of reaction