Description 1. What is the oxidation state of each element in Mn(NO3)2? N = 2. Assign oxidation states to the species in the unbalanced redox reaction. Ag+(aq)+Cu(s)?Ag(s)+Cu2+(aq) Ag+(aq)= Balance the redox reaction. redox reaction: Ag+(aq)+Cu(s)?Ag(s)+Cu2+(aq) 3. The quantity of antimony in an ore can be determined by an oxidation?reduction titration with an oxidizing agent. The ore is dissolved in hot, concentrated acid and passed over a reducing agent so that all of the antimony is in the form of Sb3+(aq) . The Sb3+(aq) is completely oxidized by an aqueous solution of BrO?3(aq) . Complete and balance the equation for this reaction in acidic solution. equation: BrO?3+Sb3+?Br?+Sb5+ 4. Balance the half-reaction in basic solution. Use e? as the symbol for an electron. half-reaction: SO2?3?S2O2?4 5. For a particular redox reaction, NO?2 is oxidized to NO?3 and Fe3+ is reduced to Fe2+. Complete and balance the equation for this reaction in basic solution. The phases are optional. balanced reaction: NO?2+Fe3+?NO?3+Fe2+ 6. Use the activity series interactive to complete the table. Mg Zn Cu Ag Mg2+ Zn2+ Cu2+ Ag+ REACTION OR NO REACTION 7.
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