1.) Use a table of Standard Reduction Potentials to predict if a reaction will occur when...

1.) Use a table of Standard Reduction Potentials to predict if a reaction will occur when Mg metal is put into a 1M aqueous H⁺solution.

If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank.

2.) Use a table of Standard Reduction Potentials to predict if a reaction will occur between Zn metal and I₂(s), when the two are brought in contact via standard half-cells in a voltaic cell.

If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank.

Expert Solution

1)




			standard reduction potential of Mg is more than H so following reaction occurs: Mg > Mg +2 + 2 e^ - 2 H+ + 2 e^ - > H2 (aq) overall Mg + 2 H+ > Mg +2 (aq) So Mg dissolves in Acids(H+ ions ) that is it gives two electrons ..where as H+ ions accept electrons 2) standard electrode potential of Zn is more that I so following reaction occurs Zn > Zn+2 + 2 e^- 2 I - < 2 e - + I 2 (aq) ------------------------------- Overall : Zn + I2 > Zn+2 + 2I^ - (aq) (aq)

queen_honey_blossom answered 2 years ago

Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ∘C) for the following reaction:

Standard reduction potentials Reduction half-reaction E∘ (V) Ag+(aq)+e−→Ag(s) 0.80 Cu2+(aq)+2e−→Cu(s) 0.34 Sn4+(aq)+4e−→Sn(s) 0.15 2H+(aq)+2e−→H2(g) 0 Ni2+(aq)+2e−→Ni(s) −0.26 Fe2+(aq)+2e−→Fe(s) −0.45 Zn2+(aq)+2e−→Zn(s) −0.76 Al3+(aq)+3e−→Al(s) −1.66 Mg2+(aq)+2e−→Mg(s) −2.37 Part A Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ∘C) for the following reaction: Fe(s)+Ni2+(aq)→Fe2+(aq)+Ni(s) Express your answer numerically. Part B Calculate the standard cell potential (E∘) for the reaction X(s)+Y+(aq)→X+(aq)+Y(s) if K = 3.04×10−3. Express your answer to three significant figures and include the appropriate...

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