Enter electrons as e-. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur when Zn metal is put into a 1M aqueous Al3+ solution. If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank.
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Use the table of standard reduction potentials (Table $17-1$ ) to pick a reagent that is capable of each of the following oxidations (under standard conditions in acidic solution). a. oxidize $\mathrm{Br}^{-}$ to $\mathrm{Br}_{2}$ but not oxidize $\mathrm{Cl}^{-}$ to $\mathrm{Cl}_{2}$ b. oxidize Mn to $\mathrm{Mn}^{2+}$ but not oxidize $\mathrm{Ni}$ to $\mathrm{Ni}^{2+}$
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