Question

Consider the following unbalanced equation. Pb(s) + Mg2+(aq) right --> Mg(s) + Pb2+(aq)

(a) What are the following standard voltages? Include the sign, changing it as appropriate. Use the standard reduction potentials in the Reference Tables. Enter the number of decimal places allowed by the data in the table.

-standard oxidation potential for the oxidation half-cell: ___ V

-standard reduction potential for the reduction half-cell: ___ V

-potential for the entire cell:___ V

(b) Select all that apply for the reaction running in the spontaneous direction under standard conditions.

_Pb2+ is the substance being reduced.

_Mg2+ is the substance being reduced.

_Pb is the substance being oxidized.

_Mg is the substance being oxidized.

_The forward reaction is spontaneous.

_The reverse reaction is spontaneous.

_Electrons will flow from the Pb half-cell to the Mg half-cell.

_Electrons will flow from the Mg half-cell to the Pb half-cell.

_[Pb2+] increases as the cell operates.

_[Pb2+] decreases as the cell operates.

_[Mg2+] increases as the cell operates.

_[Mg2+] decreases as the cell operates.

_[Pb2+] and [Mg2+] remain constant.

Answer 1

For given reaction.

Pb is getting oxidised.

Mg2+ is being reduced.