III Writing the half-reactions of a complex redox reaction in acidic.... Write balanced half-reactions for the following redox reaction: 6 Cl₂(9)+C₂H₂OH()+ 3H₂O() 12 Cl(aq)+2 CO₂(g) +12 H (aq) reduction: oxidation: 1 0-0 0. X S C

Answer the four questions below related to the spontaneous redox reaction that occurs whenCr(OH)3(s) reacts with NO3–(aq) to produce CrO42–(aq)and NO2–(aq) under basic conditions. Write the balanced net ionic equation, including states of matter, for the overall reaction.

A galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to this galvanic cell under standard conditions reads 0.45 V, and AG, xn = -79 kJ/mol. If the concentration of Fe2+ is increased to 2.0 M, then Ecell will and AGrxn will be than AGxn- Fe(s) + 2H*(aq) Fe2* + H2(g) decrease, less negative O decrease, more negative O increase, more negative O increase, less negative

Calculate the equilibrium constant, K, for the reaction shown at 25 °C. Fe+(aq)+B(s) + 6 H, O(1) → Fe(s) + H,BO,(s) + 3 H,O*(aq) The balanced reduction half-reactions for the equation and their respective standard reduction potential values (E") are Fe3+ (aq) + 3 e- → Fe(s) H,BO, (s) + 3 H,0*(aq) + 3 e- – B(s) + 6 H, O(1) E' = -0.04 V E' = -0.8698 V K =

Balance the following redox reaction in basic solution: Cu(s) + HNO3(aq) ---> Cu2+(aq) + NO(g)     Oxidation half reaction: Reduction half reaction: Overall balanced equation:

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: AG° 2+ Ni²+(aq) + Sn(s) → Ni(s) + Sn²+ (aq) Ni2+ (aq) + 2e → Ni(s) Fre = -0.250 V Sn2+ red (aq) + 2e¯ → Sn(s) red EO = -0.140 V kJ K for this reaction would be than one.

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 210, (aq) + 12H" (aq)+ 5Co (s) → L, (s)+ 6H,0 (1)+ 5Co" (aq) Suppose the cell is prepared with 6.10 M IO, and 1.61 M H' in one half-cell and 7.06 M Co 2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. х10

a) Balance the following redox reaction occurring under basic conditions using the Oxidation  Number method: IO31-(aq) + C2O42-(aq) → I1-(aq) + CO2(g)  b) Identify the oxidizing agent and the reducing agent. Give reasons for your choices.