Consider the reaction represented $$ \mathrm{byCr}_{2} \mathrm{O}_{7}^{2-}+\mathrm{Cl}^{-} \xrightarrow{ ext { i. Explain why the reaction is a redox reaction. }} \quad \mathrm{Cr}^{3+}+\mathrm{Cl}_{2} $$ iii. Balance the redox equation State five physical properties of metals

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Consider the reaction represented $$ \mathrm{byCr}_{2} \mathrm{O}_{7}^{2-}+\mathrm{Cl}^{-} \xrightarrow{	ext { i. Explain why the reaction is a redox reaction. }} \quad \mathrm{Cr}^{3+}+\mathrm{Cl}_{2} $$ iii. Balance the redox equation State five physical properties of metals

Bernard Powers · Accepted Answer

### i. Explanation of why the reaction is a redox reaction The reaction is a redox reaction because there is a transfer of electrons between the species involved, leading to changes in their oxidation states. Chloride ion is oxidized to chlorine gas, and dichromate ion is reduced to chromium ions. ### ii. Balancing the redox equation The balanced redox equation is: $$ \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-} + 6 \mathrm{Cl}^- + 14 \mathrm{H}^+ \rightarrow 2 \mathrm{Cr}^{3+} + 3 \mathrm{Cl}_2 + 7 \mathrm{H}_2\mathrm{O} $$ ### iii. Five physical properties of metals 1. Conductivity 2. Malleability 3. Ductility 4. Luster 5. Density

Consider the reaction represented \( \mathrm{byCr}_{2} \mathrm{O}_{7}^{2-}+\mathrm{Cl}^{-} \xrightarrow{\text { i. Explain why the reaction is a redox reaction. }} \quad \mathrm{Cr}^{3+}+\mathrm{Cl}_{2} \) iii. Balance the redox equation State five physical properties of metals

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Consider the reaction represented \( \mathrm{byCr}_{2} \mathrm{O}_{7}^{2-}+\mathrm{Cl}^{-} \xrightarrow{\text { i. Explain why the reaction is a redox reaction. }} \quad \mathrm{Cr}^{3+}+\mathrm{Cl}_{2} \) iii. Balance the redox equation State five physical properties of metals

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