Answer:
Al (s) + AgClO3 (aq) will result in a chemical reaction.
Al(s) + 3AgClO₃(aq) -----> Al(ClO₃)₃(aq) + 3Ag(s)
Cd(s) + CuNO3(aq) will also result in a chemical reaction.
Cd(s) + 2CuNO₃ -----> Cd(NO₃)₂ + 2Cu
Explanation:
For chemical reactions, metals lower on the activity series cannot normally displace ions of metals higher than them in the activity series.
Metals at the lower end of the activity series are not easily oxidized.
The activity series is attached to this solution. (Note: Cadmium is not on the attached chart, but Cadmium is between Iron (Fe) & Cobalt (Co) on the activity series)
- Pb is way lower Mg in the activity series, hence, it cannot become oxidized by displacing Mg2+ ion in solution.
- Al is way higher than Ag in the activity series. Hence it will easily be oxidized and displace displace Ag from it's solution easily.
- Cadmium will displace Copper in solution too because Cd is higher than Cu on the activity series.
- Platinum cannot displace Cobalt from solution as Pt is lower than Co on the activity series.
The reactions that would occur are those reactions in which metals that are lower in the series are displaced from aqueous solution by metals that are higher in the series.
The activity series is an arrangement of metals in order of decreasing reactivity. Metals that are higher up in the series are far more reactive than the metals that are lower in the series. A metal that is higher in the series will displace metals below it from their aqueous solutions.
Bearing this information in mind, the following reactions are possible;
Aluminium is far higher than silver in the series so it can displace silver from its aqueous solution. Also cadmium is higher than copper in the activity series so the reaction is possible.
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