Question

complete the following equations (note that the equations are not balanced). use the activity series if necessary.
li > k > ba > sr > ca > na > mg > al > mn > zn > cr > fe > cd >
co > ni > sn > pb > h > sb > bi > cu > ag > pd > hg > pt > au
al + agcl → ?
alcl₃ + ag
alag₃ + cl₂
no reaction
alcl + cl

Explanation:

Step1: Check Activity Series

In the activity series, Al is more reactive than Ag (Al is before Ag: \( \text{Al} > \text{Ag} \) from the given series \( \text{Li} > \text{K} > \dots > \text{Al} > \dots > \text{Ag} > \dots \)). So a single - replacement reaction will occur.

Step2: Determine Products

In a single - replacement reaction between a metal (Al) and a metal salt (AgCl), the more reactive metal (Al) will replace the less reactive metal (Ag) in the compound. The reaction is \( \text{Al}+\text{AgCl}\to\text{AlCl}_3+\text{Ag} \) (we consider the common oxidation states: Al has a + 3 oxidation state and Cl has a - 1 oxidation state, so the aluminum chloride formed is \( \text{AlCl}_3 \), and Ag is displaced as a pure metal). The other options are incorrect: \( \text{AlAg}_3+\text{Cl}_2 \) is not a valid product of this single - replacement reaction, there is a reaction (so "no reaction" is wrong), and \( \text{AlCl}+\text{Cl} \) is not a valid product.

Answer:

A. \( \text{AlCl}_3 + \text{Ag} \)