Activity Series of Metals in Aqueous Solution
Metal | Oxidation Reaction |
Lithium | Li( s ) → Li+ ( aq ) + e- |
Potassium | K( s ) → K + ( aq ) + e- |
Barium | Ba( s ) → Ba2 + ( aq ) + 2e- |
Calcium | Ca( s ) → Ca2 + ( aq ) + 2e- |
Sodium | Na( s ) → Na + ( aq ) + e- |
Magnesium | Mg( s ) → Mg2 + ( aq ) + 2e- |
Aluminum | Al( s ) → Al3 + ( aq ) + 3e- |
Manganese | Mn( s ) → Mn2 + ( aq ) + 2e- |
Zinc | Zn( s ) → Zn2 + ( aq ) + 2e- |
Chromium | Cr( s ) → Cr3 + ( aq ) + 3e- |
Iron | Fe( s ) → Fe2 + ( aq ) + 2e- |
Cobalt | Co( s ) → Co2 + ( aq ) + 2e- |
Nickel | Ni( s ) → Ni2 + ( aq ) + 2e- |
Tin | Sn( s ) → Sn2 + ( aq ) + 2e- |
Lead | Pb( s ) → Pb2 + ( aq ) + 2e- |
Hydrogen | H2 ( g ) → 2H + ( aq ) + 2e- |
Copper | Cu( s ) → Cu2 + ( aq ) + 2e- |
Silver | Ag( s ) → Ag + ( aq ) + e- |
Mercury | Hg( l ) → Hg2 + ( aq ) + 2e- |
Platinum | Pt( s ) → Pt2 + ( aq ) + 2e- |
Gold | Au( s ) → Au3 + ( aq ) + 3e- |
Using the activity series (Table 4.5 in the textbook), write balanced chemical equations for the following reactions.
hydrogen gas is bubbled through an aqueous solution of nickel (II) chloride
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