Question

HELP NEED ANSWERED TODAY BY 11:50PM!!!

Part A

Write balanced equation for the anode of the following galvanic cell
Fe(s)|Fe2+(aq)||O2(g)|H+(aq),H2O(l)|Pt(s)

Express your answer as a chemical equation. Identify all of the phases in your answer.

Part B

Write balanced equation for the cathode of the following galvanic cell
Fe(s)|Fe2+(aq)||O2(g)|H+(aq),H2O(l)|Pt(s)

Express your answer as a chemical equation. Identify all of the phases in your answer.

Part C

Write balanced equation for overall cell reactions of the following galvanic cell
Fe(s)|Fe2+(aq)||O2(g)|H+(aq),H2O(l)|Pt(s)

Express your answer as a chemical equation. Identify all of the phases in your answer.

Part D

Calculate E∘ for each of the following reactions, and tell which are spontaneous under standard-state conditions.

1.

2Fe2+(aq)+Pb2+(aq)→2Fe3+(aq)+Pb(s)

Express your answer using two decimal places.

2.

Mg(s)+Ni2+(aq)→Mg2+(aq)+Ni(s)

Express your answer using two decimal places.

Part E

Consider a galvanic cell that uses the reaction
2Ag+(aq)+Sn(s)→2Ag(s)+Sn2+(aq)

Calculate the potential at 25∘C for a cell that has the following ion concentrations: [Ag+] = 1.5×10⁻² M , 3.2×10⁻² M .

Express your answer using two significant figures.

Answer 1

The given cell notation is as follows Part A In a cell notation, the half-cell that present left to the salt bridge (l) represents the reaction that occurs at anode. At anode, oxi dati on takes place. Thus, the balanced reaction occurs at anode is as follows Fe(s)Fe2 (ag) +2 e Part B In a cell notation, the half-cell that present right to the salt bri dge (1) represents the reaction that occurs at cathode. At cathode, reducti on takes place Thus, the balanced reaction occurs at cathode is as follows 02(8) +4H (aq) +4e2 H20(0) Part C The overall cell reaction is determinde as follows 2 Fe(s)> 2 Fe* (aq) +4 e O2 (g) 4 H*(a) +4 e2 H20 2 Fe(s) +02(8) +4H(aa) 2Fe () 2H,(U)