Zn + CuCl2 → ZnCl2 + Cu
3CuCl + 2Al → 3Cu + 2AlCl3
Mg + 2AgNO3 → 2Ag + Mg (NO3)2
d. For the three reactions that are demonstrated, describe each in as much detail as possible. Include any added catalysts and/or nonreactive substances and provide each of their functions to the reactions. Where possible indicate whether the reaction is endothermic or exothermic.
In order to describe each of the reactions in detail, let's break down each one:
a. Zn + CuCl2 → ZnCl2 + Cu
In this reaction, zinc (Zn) reacts with copper(II) chloride (CuCl2) to form zinc chloride (ZnCl2) and copper (Cu). This is a single replacement reaction where the zinc displaces copper from the copper chloride compound.
There are no added catalysts or nonreactive substances mentioned in this reaction. It can be considered an exothermic reaction because it releases energy in the form of heat.
b. 3CuCl + 2Al → 3Cu + 2AlCl3
In this reaction, copper(I) chloride (CuCl) reacts with aluminum (Al) to produce copper (Cu) and aluminum chloride (AlCl3). This is also a single replacement reaction where aluminum displaces copper from the copper chloride compound.
There are no added catalysts or nonreactive substances mentioned in this reaction. It can also be considered an exothermic reaction.
c. Mg + 2AgNO3 → 2Ag + Mg(NO3)2
In this reaction, magnesium (Mg) reacts with silver nitrate (AgNO3) to form silver (Ag) and magnesium nitrate (Mg(NO3)2). This is again a single replacement reaction where magnesium displaces silver from the silver nitrate compound.
There are no added catalysts or nonreactive substances mentioned in this reaction. It can be considered an exothermic reaction.
Overall, all three reactions involve the displacement of a less reactive metal by a more reactive metal. No catalysts or nonreactive substances are mentioned, simplifying the reaction details. The reactions are exothermic, meaning they release energy in the form of heat.