the information below describes a redox reaction.\n$cr^{3 + }(aq)+2cl^{-}(aq)longrightarrow…

the information below describes a redox reaction.\n$cr^{3 + }(aq)+2cl^{-}(aq)longrightarrow cr(s)+cl_{2}(g)$\n$2cl^{-}(aq)longrightarrow cl_{2}(g)+2e^{-}$\n$cr^{3 + }(aq)+3e^{-}longrightarrow cr(s)$\nwhat is the final, balanced equation for this reaction?\n$2cr^{3 + }(aq)+6cl^{-}(aq)longrightarrow 2cr(s)+3cl_{2}(g)$\n$2cr^{3 + }(aq)+2cl^{-}(aq)+6e^{-}longrightarrow cl_{2}(g)+2cr(s)$\n$cr^{3 + }(aq)+6cl^{-}(aq)+3e^{-}longrightarrow 2cr(s)+3cl_{2}(g)$\n$cr^{3 + }(aq)+2cl^{-}(aq)longrightarrow cr(s)+cl_{2}(g)$

the information below describes a redox reaction.\n$cr^{3 + }(aq)+2cl^{-}(aq)longrightarrow cr(s)+cl_{2}(g)$\n$2cl^{-}(aq)longrightarrow cl_{2}(g)+2e^{-}$\n$cr^{3 + }(aq)+3e^{-}longrightarrow cr(s)$\nwhat is the final, balanced equation for this reaction?\n$2cr^{3 + }(aq)+6cl^{-}(aq)longrightarrow 2cr(s)+3cl_{2}(g)$\n$2cr^{3 + }(aq)+2cl^{-}(aq)+6e^{-}longrightarrow cl_{2}(g)+2cr(s)$\n$cr^{3 + }(aq)+6cl^{-}(aq)+3e^{-}longrightarrow 2cr(s)+3cl_{2}(g)$\n$cr^{3 + }(aq)+2cl^{-}(aq)longrightarrow cr(s)+cl_{2}(g)$

Answer

Answer:

2Cr$^{3 +}$(aq) + 6Cl$^{-}$(aq) $\longrightarrow$ 2Cr(s) + 3Cl$_{2}$(g)

Explanation:

Step1: Determine electron - transfer balance

Oxidation half - reaction: 2Cl$^{-}$(aq) $\longrightarrow$ Cl$_{2}$(g) + 2e$^{-}$ (loses 2 electrons). Reduction half - reaction: Cr$^{3 +}$(aq) + 3e$^{-}$ $\longrightarrow$ Cr(s) (gains 3 electrons).

Step2: Make electron gain and loss equal

Multiply oxidation half - reaction by 3 and reduction half - reaction by 2. Oxidation: 6Cl$^{-}$(aq) $\longrightarrow$ 3Cl$_{2}$(g) + 6e$^{-}$. Reduction: 2Cr$^{3 +}$(aq) + 6e$^{-}$ $\longrightarrow$ 2Cr(s).

Step3: Combine half - reactions

2Cr$^{3 +}$(aq) + 6Cl$^{-}$(aq) $\longrightarrow$ 2Cr(s) + 3Cl$_{2}$(g)