This second article in a three-part series on gas laws describes how to use a Mason jar to collect data and demonstrate the pressure-temperature relationship, Gay-Lussac’s law. Its huge advantage is that the gas temperature is measured, NOT the temperature of the water bath.
Vitamin C, chemically known as L-ascorbic acid, is an important nutrient that provides support to body structures, contributes to wound healing and aids the immune system in preventing infection. In this activity, participants learn how to determine whether vitamin C is present in commercial drinks and, if so, how to measure the relative amount.
As the piece of metal skitters across the surface of the water in a beaker and — particularly in the case of potassium — it appears to catch fire, it is not obvious that the explanation for both phenomena lies in the production of hydrogen gas. There is a simple and safe way to demonstrate the reaction.
Consulting the print edition of the Canadian Compendium of Pharmaceuticals and Specialties1 (CPS) for the product monograph of the drug Bisoprolol, my attention strayed to the immediately preceding entry Bismutal...
This three-part series will describe how to use syringes, pressure gauges and mason jars to study gas laws — Boyle’s law, Gay-Lussac’s law and Avogadro’s law. Most likely you did not learn the properties of gases using mason jars, syringes and pressure gauges.
Stacey Lavery has these rules for students at the University of Waterloo. Do you have a “top ten lab rules” list?
From our combined experiences as coordinators and instructors of large first-year chemistry classes, we have noticed that students need not only to master subject-specific concepts and problem-solving skills to be successful, but also to think deeply about effective study habits, time management and test-writing skills. Indeed, during individual meetings with students after each initial term test, we spend more time talking about these ideas rather than chemistry concepts.
Enzyme catalysis is an important topic which is often neglected in introductory chemistry courses. In this paper, we present a simple experiment involving the yeast-catalyzed fermentation of sugars.
On its own, hydrogen peroxide slowly decomposes into oxygen and water. For this reason, fresh bottles of drugstore hydrogen peroxide, labeled 3%, are actually 6%. This is so the hydrogen peroxide remains above 3% at the expiration date, if stored properly.
This photo gives Chem 13 News the opportunity to share a teacher’s frightening experience with this demonstration. It informs and reminds readers about necessary safety considerations.