(Solved): Balancing Redox Equations Using the Oxidation Number Method Step 1. Assign oxidation numbers to all ...

Balancing Redox Equations Using the Oxidation Number Method Step 1. Assign oxidation numbers to all atoms in the equation. Step 2. Identify the atoms that are oxidized and the atoms that are reduced. Step 3. Determine the change in oxidation number for the atoms that are oxidized and for the atoms that atoms that are reduced. Step 4. Make the changes in oxidation number equal in magnitude by adjusting coefficients in the equation. Step 5. If necessary, use the conventional method to balance the remainder of the equation. Solve the following problems using the 5-step method. Indicate the atoms that are reduced and the ones that are oxidized, and the coefficient you are multiplying each one by, if needed (like I did in class). Rewrite the balanced equation after step 5 . 1. ${\mathrm{Cu}}_2\mathrm{O}+\mathrm{NO}\mathrm{CuO}+{\mathrm{N}}_2$ 2. ${\mathrm{Al}}_2{\mathrm{O}}_3+\mathrm{C}+{\mathrm{N}}_2\mathrm{AIN}+\mathrm{CO}$ 3. $\mathrm{Ag}+{\mathrm{HNO}}_3{\mathrm{AgNO}}_3+\mathrm{NO}+{\mathrm{H}}_2\mathrm{O}$ $3{\mathrm{Ag}}_{(s)}+4{\mathrm{HNO}}_3(\mathrm{aq})\to 3\mathrm{Ag}\mathrm{NO}(\mathrm{aq})+\mathrm{NO}(g)+2{\mathrm{H}}_2\mathrm{O}(1)$