using the activity series provided. which reactants will form products?\nna > mg > al > mn > zn > cr > fe >…

Explanation:

Step1: Understand activity - series concept

In a single - displacement reaction, a more reactive metal can displace a less reactive metal from its compound.

Step2: Analyze option 1 ($Ag + NaNO_3$)

Silver ($Ag$) is less reactive than sodium ($Na$) according to the activity series ($Na>Ag$). So, $Ag$ cannot displace $Na$ from $NaNO_3$. No reaction.

Step3: Analyze option 2 ($Fe + Al_2O_3$)

Iron ($Fe$) is less reactive than aluminum ($Al$) ($Al > Fe$). So, $Fe$ cannot displace $Al$ from $Al_2O_3$. No reaction.

Step4: Analyze option 3 ($Ni+NaCl$)

Nickel ($Ni$) is less reactive than sodium ($Na$) ($Na > Ni$). So, $Ni$ cannot displace $Na$ from $NaCl$. No reaction.

Step5: Analyze option 4 ($Fe + Cu(NO_3)_2$)

Iron ($Fe$) is more reactive than copper ($Cu$) ($Fe>Cu$). So, $Fe$ can displace $Cu$ from $Cu(NO_3)_2$. The reaction is $Fe + Cu(NO_3)_2\rightarrow Fe(NO_3)_2+Cu$.

Answer:

$Fe + Cu(NO_3)_2\rightarrow$ will form products.