PDF Publication Title:
Text from PDF Page: 002
• 2 plastic cups, 12-16 oz, preferably clear • 2 shiny, clean pennies • Ruler, with mm markings • Epsom salt (about 6 tsp); this is sold at most drug stores, usually as a laxative • Table salt (about 6 tsp) • Water • Optional: 1⁄2 cup and 1 tsp measuring spoon; exact measurements don’t matter so can approximate Key Concepts: • Electrolysis is the process by which electricity is used to drive a chemical reaction. • A chemical reaction where some molecule gains electrons is known as a reduction reaction. • A chemical reaction where some molecule loses electrons is an oxidation reaction. • An electrolyte solution is one in which ions (charged particles) are dissolved in water. • Electric current will flow only if there is a continuous circuit of conducting material to carry it. • Which chemical reaction occurs in an electrolytic cell depends on what molecules are present and how easily they gain or accept electrons. A table of standard reduction potentials is useful for summarizing which molecules are most easily oxidized or reduced. • Writing down balanced chemical reactions is useful for figuring out relative quantities of products formed. Introductory Mini-Lecture: Electrolysis refers to the use of electricity to drive a chemical reaction that would not normally occur on its own. In this lab, you will build an electrolytic cell – an apparatus for carrying out electrolysis and use it to produce various gases and other chemical compounds. A diagram of a basic electrolytic cell is shown here. The battery drives an electric current through the cell. If the battery is not hooked up to anything, no electricity flows. In order for a current to flow, there must be a complete circuit of conducting material from one terminal of the battery to the other. In the setup shown, electrons flow out of the negative terminal of the battery, through a wire into the negative electrode (called the cathode). The electrode can be any good conductor (eg: a metal) that is stuck into the electrolytic cell solution. Electrons also flow out of the positive electrode (the anode) into the positive terminal of the battery. But how is electric current carried from one electrode to the other? The electrolytic cell is filled with an electrolyte solution – a solution of ions (charged particles) in water. Because these charged particles can move, they are capable of carrying current across from one electrode to another. Thus, there is a complete circuit for current to flow! When we run current through an electrolytic cell, two chemical reactions occur. At the negative electrode, there is a reduction reaction – some molecule gains electrons. At the positive electrode, there is an oxidation reaction – some molecule loses electrons. These two chemical reactions can produce all sorts of useful products – like hydrogen gas for fuel cells, or purified metals from minerals. What specific chemical species is oxidized or reduced depends on how easily the various molecules present gain or accept electrons. This information is summarized in a table of standard reduction potentials. In this Created by LABScI at Stanford 2PDF Image | Electrolysis splitting water
PDF Search Title:
Electrolysis splitting waterOriginal File Name Searched:
Electrolysis-TA.pdfDIY PDF Search: Google It | Yahoo | Bing
Salgenx Redox Flow Battery Technology: Power up your energy storage game with Salgenx Salt Water Battery. With its advanced technology, the flow battery provides reliable, scalable, and sustainable energy storage for utility-scale projects. Upgrade to a Salgenx flow battery today and take control of your energy future.
| CONTACT TEL: 608-238-6001 Email: greg@salgenx.com | RSS | AMP |