Question

now you know how to recognize redox reactions. add a label to additionally identify the reactions below as one of the five reaction types you learned previously. ptcl₄(s) → pt(s) + 2cl₂(g) 2na(s) + cl₂(g) → 2nacl(s) cu(s) + 2agno₃(aq) → cu(no₃)₂(aq) + 2ag(s) nacl(aq) + agno₃(aq) → nano₃(aq) + agcl(s)

Explanation:

• For \(PtCl_{4}(s)\to Pt(s) + 2Cl_{2}(g)\): A single compound \(PtCl_{4}\) breaks down into two simpler substances \(Pt\) and \(Cl_{2}\). This is characteristic of a decomposition reaction.
• For \(2Na(s)+Cl_{2}(g)\to 2NaCl(s)\): Two substances \(Na\) and \(Cl_{2}\) combine to form a single compound \(NaCl\). This is a combination reaction.
• For \(Cu(s)+2AgNO_{3}(aq)\to Cu(NO_{3})_{2}(aq)+2Ag(s)\): One element \(Cu\) replaces another element \(Ag\) in a compound \(AgNO_{3}\). This is a single - replacement reaction.
• For \(NaCl(aq)+AgNO_{3}(aq)\to NaNO_{3}(aq)+AgCl(s)\): The positive ions (\(Na^{+}\) and \(Ag^{+}\)) exchange their negative ion partners (\(Cl^{-}\) and \(NO_{3}^{-}\)). This is a double - replacement reaction.

Answer:

1. Decomposition
2. Combination
3. Single Replacement
4. Double Replacement