Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (d) hydrogen gas is bubbled through an aqueous solution of nickel(II) chloride

Verified step by step guidance

1. Identify the reactants: hydrogen gas (H₂) and nickel(II) chloride (NiCl₂).
2. Consult the activity series to determine if hydrogen can displace nickel from nickel(II) chloride.
3. Note that hydrogen is less reactive than nickel in the activity series, meaning it cannot displace nickel.
4. Conclude that no reaction occurs because hydrogen cannot replace nickel in the compound.
5. Write 'NR' to indicate that no reaction takes place.

Key Concepts

Activity Series

The activity series is a list of metals ranked by their ability to displace other metals from solutions of their ions. More reactive metals can displace less reactive metals from their compounds in solution. Understanding this series is crucial for predicting whether a reaction will occur when a metal is introduced to a solution containing metal ions.

Redox Reactions

Redox (reduction-oxidation) reactions involve the transfer of electrons between substances, leading to changes in oxidation states. In the context of the activity series, a more reactive metal will reduce the ions of a less reactive metal, while itself being oxidized. Recognizing these electron transfer processes is essential for balancing chemical equations and determining the occurrence of reactions.

Solubility Rules

Solubility rules help predict whether a compound will dissolve in water or form a precipitate. In the case of nickel(II) chloride, it is soluble in water, allowing for the presence of nickel ions in solution. Understanding solubility is important for determining the feasibility of reactions and the products formed when different substances are mixed.