Question

youve classified reactions as one of the five types and determined which of those reactions were redox. use the summary of your work below to determine which kinds of reactions can be redox. $\boldsymbol{ptcl_{4}(s) \to pt(s) + 2cl_{2}(g)}$ decomposition $\boldsymbol{4na(s) + o_{2}(g) \to 2na_{2}o(s)}$ combination $\boldsymbol{cu(s) + 2agno_{3}(aq) \to cu(no_{3})_{2}(aq) + 2ag(s)}$ single replacement $\boldsymbol{nacl(aq) + agno_{3}(aq) \to nano_{3}(aq) + agcl(s}$ double replacement $\boldsymbol{ch_{4}(g) + 2o_{2}(g) \to co_{2}(g) + 2h_{2}o(g)}$ combustion select all of the kinds of reactions that can be redox: decomposition combination single replacement double replacement combustion

Explanation:

• Decomposition: In \(PtCl_{4}(s)\to Pt(s) + 2Cl_{2}(g)\), \(Pt\) goes from \(+4\) oxidation state in \(PtCl_{4}\) to \(0\) in \(Pt\) (reduction), and \(Cl\) goes from \(- 1\) in \(PtCl_{4}\) to \(0\) in \(Cl_{2}\) (oxidation). So decomposition can be redox.
• Combination: In \(4Na(s)+O_{2}(g)\to2Na_{2}O(s)\), \(Na\) goes from \(0\) to \(+1\) (oxidation) and \(O\) goes from \(0\) to \(-2\) (reduction). So combination can be redox.
• Single Replacement: In \(Cu(s)+2AgNO_{3}(aq)\to Cu(NO_{3})_{2}(aq)+2Ag(s)\), \(Cu\) goes from \(0\) to \(+2\) (oxidation) and \(Ag\) goes from \(+1\) to \(0\) (reduction). So single - replacement can be redox.
• Combustion: In \(CH_{4}(g)+2O_{2}(g)\to CO_{2}(g)+2H_{2}O(g)\), \(C\) goes from \(-4\) in \(CH_{4}\) to \(+4\) in \(CO_{2}\) (oxidation) and \(O\) goes from \(0\) in \(O_{2}\) to \(-2\) in \(CO_{2}\) and \(H_{2}O\) (reduction). So combustion can be redox.
• Double Replacement: In \(NaCl(aq)+AgNO_{3}(aq)\to NaNO_{3}(aq)+AgCl(s)\), there is no change in oxidation states of any elements. It is a non - redox reaction.

Answer:

Decomposition, Combination, Single Replacement, Combustion