CHEM 1127Q Lecture 8: Chapter 3-Sections 3.1, 3.2

• School: UConn
• Department: Chemistry
• Course: CHEM 1127Q
• Professor: Niluka Wasalathanthri

Document Summary

Topics covered: 3. 1 formula mass and mole concept, 3. 2 determining the molecular and empirical formulas. Calculated by adding the atomic weights of the atoms in the molecular formula of the compound. Example: find the formula mass of oh2. First, you need to look at the periodic table to find the atomic weights of hydrogen and oxygen. Do not forget that you have two hydrogens, so you need to multiply by 2. Defined as the number equal to the number of carbon atoms in exactly 12g of pure carbon-12 isotope. We normally round this to 6. 022 1023. Molar mass mass (g) no. of moles (mols) Defined as mass in grams of one mole of the substance. 3, slide 9-11: beryllium (be) is a light metal used to fabricate transparent x-ray windows for medical imaging instruments. 1023 is used for the conversion to atoms: how many moles of sucrose,