CHEM 30: Electrochemistry Complete Actual Exam Questions With Correct Detailed Answers.

Oxidize - correct answer When a substance LOSES its electrons. Reduced - correct answer When a substance GAINS its electrons. Redox Reaction - correct answer The net reaction of oxidation and reduction. Oxidation and Reduction - correct answer Occur together in ONE reaction. Oxidizing Agent - correct answer A substance that gets reduced causes another substance to be oxidized. Reducing Agent - correct answer A substance that gets oxidized cause another substance to be reduced. Disproportionation - correct answer A reaction in which the same substance functions as both the oxidizing agent and a reducing agent; it is both reduced and oxidized. Oxidation Number - correct answer A positive or negative number that allows you to determine what is happening to the electron in the reaction. Oxidation Number Increaese - correct answer The substance is being OXIDIZED. Oxidation Number Decrease - correct answer The substance is being REDUCED. Oxidization States Constants - correct answer All atoms: 0 Hydrogen: +1, except in hydrides then -1 Oxygen: -2, except in peroxides then -1 Monatomic inons: charge on ion Spontaneity Rule - correct answer If the OA is above the RA pn the redox half reaction table. 5 Step Methode - correct answer Step 1: list all entities present and classify as OA and RA and SOA and SRA. Step 2: Write down the half reactions for the SOA. Step 3: Write down the half reactions for the SRA. Step 4: Balance the electrons in both half reactions and put the two half reactions together. Step 5: Perdict spontinaity. Voltaic Cell - correct answer An electrochemical cell that spontaneously reacts to PRODUCE electricity. Electrolytic Cell - correct answer An electrochemical cell that USES electricity to cause a non-spontanious chemical change. Electrode - correct answer The solid in the half-cell where the wires attach. Anode - correct answer The electrode where oxidization occurs, where the strongest RA reacts. Cathode - correct answer The eletrode where reduction occurs, where the strongest OA reacts. Anion - correct answer A negative ion, moves toward the anode. Cation - correct answer A postive ion, moves toward the cathode. Salt Bridge - correct answer A barrier the keeps the solutions in a voltaic cell apart, but allows the flow of ions between the solutions to prevent an electrical charge build up. Required by Voltaic Cells Electrolyte - correct answer A substance the conducts electricity when dissolved in water. Power Supply - correct answer An electronic device that replaces a battery. External Circuit - correct answer The wires that are used to connect the anode to the cathode. Electron Flow - correct answer Anode to Cathode. Ion FLow - correct answer Anions to Anode; Cations to Cathade. Cell Spontanaity - correct answer Voltaic: yes Electrolytic: no Net Electrode Potencial of Cells (E°net ) - correct answer Voltaic: positve Electrolytic: negative Line Notion of Cells - correct answer anode / anode electrolyte // cathode electrolyte / cathode Chloride Anomaly - correct answer When chloride acts as the reducing agent when with water in a reaction. Standard Hydrogen Half-Cell - correct answer What is used to measure the standard reduction potentials. It contains 1.00 mol/L of the hydrogen ion. Standard Cell Difference Equation - correct answer E°net= E°r(cathode) - E°r(anode) Calculating Cell Potential Difference - correct answer Step 1: List all entities present Step 2: Determine OAs and RAs Step 3: Determine SOAs and SRAs Step 4: Write down anode and cathode half reactions (redox half reactions) Step 5: Calculate the cell potential difference Spontaneity in Electrochemical Cells - correct answer If OA is above the RA, it is spontaneous. If the cell potential is positive, the reactions is spontaneous. Faraday's Constant - correct answer 9.65 x 10^4 C/mol → it represents the number of coulombs per mole of electrons. Moles of an Electron Equation - correct answer (I x t)/F I = amps t = time in seconds F = Faraday's consta