4 If no reaction was observed, place three drops of the oxidizing agent in another well.
13 Before leaving, go to a computer in the laboratory and enter your results in the In-Lab assignment.
Keep the reactions away from ignition sources, and rinse acid off metal before discarding.
C Which species is the strongest reducing agent?Voltmeters are sensitive to the direction of electron flow (electrical current and indicate the direction by means of the sign on the potential difference.The solutions from Part B of the experiment should be rinsed into the waste code promo sport découverte container for redox solutions.If all results are scored as correct, log out.The Pb wire will be dull gray and very bendable.Question 4: Write the half-reactions for the reducing agents in order, from weakest to strongest.The liquids can be flushed down the sink with water.It will consist of a round plastic base with one center indentation lined with a porous frit which contains the salt bridge solution and indentations around the circumference for the various half-cell solutions.Consider the redox reaction (1) and Figure 1 below: ( 1 zn(s) Cu2(aq) Zn2(aq) Cu(s).6 Add about 10 mL of tap water to each beaker.3M HCl gives off acidic and irritating vapors.If something happened, write "R" (reaction) in Data Table A1 and make a brief note of what occurred in the space below.
Separating half-reactions also allows one to measure the energy difference between the electrons in the donor orbitals of a reducing agent and the acceptor orbitals of an oxidizing agent.
Goals 1, to explore the relative oxidizing and reducing strengths of different metals.
The electrons in the higher energy orbital in zinc can spontaneously move to the lower energy orbital in copper(II).