Question

based on the activity series, which of the reactions will occur?
most reactive least reactive
li na k mg al zn fe ni sn pb h cu ag pt
f₂ cl₂ br₂ i₂
hint: is the free element more reactive than the one in the compound?
k + fe(no₃)₂ →
pb + snso₄ →
pb + zn(clo₃)₂ →
ag + pbso₄ →

Explanation:

Step1: Analyze the first reaction

Check the reactivity of \(K\) and \(Fe\). From the activity series, \(K\) (potassium) is more reactive than \(Fe\) (iron). So \(K\) can displace \(Fe\) from \(Fe(NO_3)_2\).

Step2: Analyze the second reaction

Check the reactivity of \(Pb\) (lead) and \(Sn\) (tin). From the activity series, \(Pb\) is less reactive than \(Sn\). So \(Pb\) cannot displace \(Sn\) from \(SnSO_4\).

Step3: Analyze the third reaction

Check the reactivity of \(Pb\) and \(Zn\) (zinc). From the activity series, \(Pb\) is less reactive than \(Zn\). So \(Pb\) cannot displace \(Zn\) from \(Zn(ClO_3)_2\).

Step4: Analyze the fourth reaction

Check the reactivity of \(Ag\) (silver) and \(Pb\) (lead). From the activity series, \(Ag\) is less reactive than \(Pb\). So \(Ag\) cannot displace \(Pb\) from \(PbSO_4\).

Answer:

\(K + Fe(NO_3)_2\to\)