TABLE: Magnesium: Mg(s) Mg2+(aq) + 2 e- Aluminum: Al(s) Al3+(aq) + 3 e- Manganes

Question

TABLE:

Magnesium: Mg(s) Mg2+(aq) + 2 e-

Aluminum: Al(s) Al3+(aq) + 3 e-

Manganese: Mn(s) Mn2+(aq) + 2 e-

Zinc: Zn(s) Zn2+(aq) + 2 e-

Chromium: Cr(s) Cr3+(aq) + 3 e-

Iron: Fe(s) Fe2+(aq) + 2 e-

Nickel: Ni(s) Ni2+(aq) + 2 e-

Lead: Pb(s) Pb2+(aq) + 2 e-

Copper: Cu(s) Cu2+(aq) + 2 e-

Mercury: Hg(s) Hg2+(aq) + 2 e-

Platinum: Pt(s) Pt2+(aq) + 2 e-

Gold: Au(s) Au3+(aq) + 3 e-

Pick all of the reactions that will occur.

Cu(s) + Mg2+(aq) -->

Mg(s) + Cu2+(aq) -->

Hg(s) + Au3+(aq) -->

Fe(s) + Pt2+(aq) -->

Hg(s) + Pb2+(aq) -->

Mn(s) + Mg2+(aq) -->

please tell me, which reactions will occur and WHY??? :(((

Explanation / Answer

What you need to do is go through and complete all of these reactions. Then assign oxidation numbers. If the substance that is oxidized is higher on the list, then the reaction will occur. On the flip side, if the oxidized substance is lower on the list, the reaction will not occur.

The 6 reactions have a metal (LHS) and an ion RHS
The metal will react if it is more reactive than the metal of the ion

2,3,4

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