Question

Using the activity series(Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, simply write NR. (a) Iron metal is added to a solution of copper(II) nitrate; (b) zinc metal is added to a solution of magnesium sulfate; (c) hydrobromic acid is added to tin metal; (d) hydrogen gas is bubbled through an aqueous solution of nickel(II) chloride; (e) aluminum metal is added to a solution of cobalt(II) sulfate.

Short answer

a) \(Fe + Cu(NO3)_2 \rightarrow Fe(NO3)_2 + Cu\) b) NR (no reaction) c) \(2HBr + Sn \rightarrow SnBr_2 + H_2\) d) NR (no reaction) e) \(2Al + 3CoSO_4 \rightarrow Al_2(SO_4)_3 + 3Co\)

Step-by-step solution

a) Reaction of Iron metal with Copper (II) Nitrate

According to the activity series, iron (Fe) is more reactive than copper (Cu). Therefore, when iron is added to a solution of copper (II) nitrate (Cu(NO3)2), it will displace copper and form iron (II) nitrate. Balanced equation: \(Fe + Cu(NO3)_2 \rightarrow Fe(NO3)_2 + Cu\)

b) Reaction of Zinc metal with Magnesium Sulfate

In this case, zinc (Zn) is added to a solution of magnesium sulfate (MgSO4). Looking at the activity series, we can see that zinc is less reactive than magnesium (Mg). This means that no reaction will occur between zinc and magnesium sulfate. Answer: NR (no reaction)

c) Reaction of Hydrobromic Acid with Tin metal

Here, hydrobromic acid (HBr) is added to tin (Sn) metal. According to the activity series, tin is more reactive than hydrogen (H), which means that tin will replace hydrogen in hydrobromic acid, forming Tin(II) bromide (SnBr2) and releasing hydrogen gas. Balanced equation: \(2HBr + Sn \rightarrow SnBr_2 + H_2\)

d) Reaction of Hydrogen gas with Nickel (II) Chloride solution

In this reaction, hydrogen gas (H2) is bubbled through an aqueous solution of nickel(II) chloride (NiCl2). As per the activity series, hydrogen is less reactive than nickel (Ni), meaning that no reaction will take place between hydrogen gas and nickel(II) chloride solution. Answer: NR (no reaction)

e) Reaction of Aluminum metal with Cobalt (II) Sulfate solution

We are given that aluminum (Al) metal is added to a solution of cobalt(II) sulfate (CoSO4). Referring to the activity series, aluminum is more reactive than cobalt (Co). Consequently, aluminum will replace cobalt in the compound, resulting in the formation of aluminum sulfate (Al2(SO4)3) and cobalt metal. Balanced equation: \(2Al + 3CoSO_4 \rightarrow Al_2(SO_4)_3 + 3Co\)