Consider a galvanic cell that consists of Mg/Mg^2+ half-cell and a SHE. Write a

Question

Consider a galvanic cell that consists of Mg/Mg^2+ half-cell and a SHE. Write a balanced net ionic equation for the galvanic cell. Calculate the standard emf of the cell Give the cell diagram for the reaction occurring in this galvanic cell. Calculate E^0_cell and then predict whether the following reactions would occur spontaneously in aqueous solution at 25 degree C. Assume that the initial concentrations of dissolved species are all 1.0 M. Ca(s) + Cd^2+(aq) rightarrow Ca^2+(aq) + Cd(s) 2 Br^-(aq) + Sn^2+(aq) rightarrow Br_2(1) + Sn(s) 2 Ag(s) + Ni^2+(aq) rightarrow 2 Ag^1+(aq) + Ni(s) Cu^+(aq) + Fe^3+(aq) rightarrow Cu^2+(aq) + Fe^2+(aq) Which species in each pair is a better oxidizing agent under standard-state conditions? Br_2 or Au^3+ H^+ or Ag^+ Cd^2+ or Cr^3+ O_2 in an acidic media or O_2 in an basic media Which Species in each pair is a better reducing agent under standard-state conditions?

Explanation / Answer

8.

in order to reactions to be spontnous, you need to have a possitive E°cell

so:

Ca2+(aq) + 2e– Ca(s) –2.87

Cd2+(aq) + 2e– Cd(s) –0.403

Cd favours , then it is spotnanous

b.

Br2(l) + 2e– 2Br–(aq) +1.07

Sn2+(aq) + 2e– Sn(s) –0.14

is more likely that Bromine gets the electron, therefore, this is NOT favoured

c.

Ag+(aq) + e– Ag(s) +0.80

Ni2+(aq) + 2e– Ni(s) –0.26

this favours the formation of solid Ag, therefore it is NOT favoured

d.

Cu2+(aq) + e– Cu+(aq) +0.153

Fe3+(aq) + e– Fe2+(aq) +0.771

this favours more Fe3+ than Cu+; so... this is NOT spotnaous

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