Bi (s) + Cl"(aq) + Hg (OH), Bicl, + Hg" 1. Write the two half- reactions (Oxidation and reduction reaction) 2. Balance the atoms undergoing oxidation and reduction/ all other atoms other than "O" and "H". 3. Balance atoms and charges in each half-reaction. a. Use H20 to balance o atoms. b. Use H* to balance H atoma c. Neutralize H* by adding the same number of OH to each side of the equation d. Use e to balance positive charges 4. Multiply each half-reaction by some integer so the the number of e- lost in the Oxidation half-reaction equals the number of e- gained in the Reduction half- reaction 5. Add the half - reactions together, canceling species that appear on both sides. The e- must completely cancel and not be present in the end.

A student followed the procedure in this experiment, using 48.70 ml of 1.028 molar HCl and 50.60 mL of 1.028 molar NaOH. Analysis of the collected data resulted in a heat transfer of 2843 J during reaction. Use this information to determine the heat of neutralization for this reaction in kJ/mol.

What type of reaction has occurred? How do you know? CH3 CH2

Controlling the ammonia and ammonium ion concentrations is one of the biggest problems in maintaining a healthy fish aquarium. Ammonia, which is highly toxic to fish because it interferes with their uptake of oxygen, is formed from wastes excreted by the fish, uneaten food, and decaying plants. Beneficial bacteria oxidize the ammonia and ammonium to nitrate, which is not highly toxic to fish in low to moderate levels. Complete and balance the following reaction equation describing the oxidation of ammonium to nitrate ions in acidic solution. NH4*(aq) + O2(aq) NO3 (aq)