Question

4
what are the products of this reaction? * (0.5 points)
__agno₃(aq) + __al(s) →
○ al(no₃)₃ + ag
○ alo + agn
○ no₃ + alag
○ ag + alno₃
○ no reaction

Explanation:

Step1: Identify Reaction Type

This is a single - displacement reaction. In a single - displacement reaction, a more reactive metal displaces a less reactive metal from its compound. The reactivity series tells us that aluminum (Al) is more reactive than silver (Ag). So, Al will displace Ag from $AgNO_3$.

Step2: Determine Products

The general form of a single - displacement reaction for a metal displacing another metal from its nitrate compound is: $Metal_1 + Metal_2(NO_3)_n
ightarrow Metal_1(NO_3)_n+Metal_2$. Here, $Metal_1 = Al$ and $Metal_2 = Ag$. The nitrate ion ($NO_3^-$) has a charge of - 1. Aluminum has a charge of + 3 in its compounds, so the formula for aluminum nitrate is $Al(NO_3)_3$. And the displaced metal is Ag (silver). So the reaction is $3AgNO_3(aq)+Al(s)
ightarrow Al(NO_3)_3(aq)+3Ag(s)$.

Answer:

A. $Al(NO_3)_3 + Ag$