A hypothetical metal Fresnium (Fn) is placed in a solution of 1M fresnium(ll) ni

Question

A hypothetical metal Fresnium (Fn) is placed in a solution of 1M fresnium(ll) nitrate, and a standard copper reference electrode is also placed in the solution. In order to get a positive voltage reading, the copper electrode must be connected to the - pole of the voltmeter, and the fresnium metal to the + pole. The voltage meter reads + 0.63 volts. Write out the reaction equation, then calculate the standard reduction potential of Fresnium. Another hypothetical metal Joaquium (Jq) and its 1M salt solution (Jq^2+) generate 1.12 volts when placed in a standard cell with copper/copper ion, where the copper electrode was the anode. Write out the reaction equation, and then calculate the standard reduction potential of Joaquium. Write out the two reactions above (Fn/Cu and Jq/Cu) in cell notation form (e.g.: Cu degree (s) | Cu^2+ (aq)|| Ag^+ (aq)|Ag degree (s)) Write the three standard reductions of fresnium, copper, and joaquium in the format of a standard reduction potential table. What is the strongest oxidizing agent and the strongest reducing agent of the three?

Explanation / Answer

c, Cell notation,

Fn/Cu

Cu (s) | Cu2+ (aq) || Fn2+ (aq) || Fn (s)

Jq/Cu

Cu (s) | Cu2+ (aq) || Jq2+ (aq) || Jq (s)

4. Standard reduction of,

fresnium,

Fn2+ (aq) + 2e- <==> Fn(s)

Joaquium

Jq2+(aq) + 2e- <==> Jq(s)

Copper

Cu2+(aq) + 2e- <==> Cu(s)

Strongest oxidizing agent : joaquium

Strongest reducing agent : copper

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