In chemistry, a mole is a quantity used relate reactants to products in stoichiometric equations. A mole of any substance is equal to 6.02 x 10^23 particles -- usually atoms or molecules -- of that substance. For a given element, the mass (in grams) of o
Most people are familiar with the use of words for numerical values such as "dozen" for twelve and "pair" for two. Chemistry employs a similar concept with the mole (abbreviated mol), which refers not to a small burrowing mammal but to the number 6.022 x
Chemistry is full of many different confusing conversions. These conversions are important because they ultimately allow us to discover how a particular atom or molecule will interact with other atoms and molecules. Central to chemical conversions is the conversion of grams to moles, and vice versa....
First, it is necessary to understand how atoms and molecules combine in chemical reactions, which is not quite like the "ingredients" in, say a cooking recipe or a construction project. Ordinarily, you would keep track of different objects by measuring their masses (in kilograms, pounds or oun...
Identify the moles of a solute per liter of a solution Know when molality is usually used Learn the essential characteristics of molarity Appreciate the defining characteristics of a concentration Understand the essential characteristics of molality ...
I understand. Looks like there are some ways to figure it out, but still a novice guess in most instances until you become more familiar with substances and properties. So before we close this topic, or we can continue, What about the -ates, -ites? Or does it just depend?
I also want to state an easier, simpler-to-understand definition of a mole (of chemistry). Moles are a unit of measurement of chemical compounds. Just like how physical quantities, such as distance, mass, time etc. have measurement units (meters, grams, seconds respectively), similarly, chem...
Learn how to find the percent composition of an empirical compound Appreciate what the empirical compound shows Understand the contrasts with a chemical formula You are viewing quiz7 in chapter 9 of the course: Chemistry 101: General Chemistry Course Practice ...
Now this example will help you understand the mole fraction more clearly. Suppose you dissolve 77 gram of carbon tetrachloride in 78 gram of acetone. So, now what will be the mole fraction of this compound? First of all, convert the masses to the number of moles of each com...
In fact, there are so many that it can be very difficult to really understand the number of them. You're dealing with enormous numbers of a very tiny particle. But, chemistry requires the knowledge of how many particles for many reasons, among which include predicting reactions and making ...