PPT-Formula Mass

vs Gram Formula Mass AMUs vs Grams Aim How can we find the formula mass and gram formula mass of a compound Essential Questions How can we find the formula mass and gram formula mass of a compound. . vs. . Empirical Formula. Different compounds can have the . same. empirical formula. but . different. molecular formulas. .. Empirical . Formula is a . reduced. . form of Molecular formula . Molecular Formula and Empirical Formula. . Chemical . Reactions and. . Reaction . Stoichiometry. James F. Kirby. Quinnipiac University. Hamden, CT. Lecture Presentation. Stoichiometry. The study of the mass relationships in chemistry. Based on the Law of Conservation of Mass (Antoine Lavoisier, 1789). . - . hydrates. Dr. Chin Chu. Chemistry. River Dell High School. Definition:. Hydrates in Inorganic Chemistry – are inorganic salts “containing water molecules combined in a definite ratio as an integral part of the salt crystal that are either bound to a metal center or that have crystallized with the metal complex.. Isotopes of Carbon. . . C-12 has 6 protons and 6 neutrons with an abundance of 98.90%. C-13 has 6 protons and 7 neutrons with an abundance of only 1.10%. The Mole. . . The number of units (atoms) in this amount of carbon-12 is our “bunch”. This bunch is called a . Empirical & Molecular Formula Notes. Drill. Calculate the percent composition of Na. 2. SO. 4. .. HW:. Finish pg. 3 (Empirical Formulas). MM=142.05 . g. /mol. 32.37% Na, 22.58% S, 45.05% O. Objectives. Lecture Presentation. Chapter 3. Molecules, Compounds, and Chemical Equations. How Many Different Substances Exist? . Elements combine with each other to form . compounds. . . The great diversity of substances that we find in nature is a direct result of the ability of elements to form compounds. . Why Study Chemistry?. . Think about current issues in the news.. . . . . . . 2. Why Study Chemistry?. . Think about current issues in the news.. Energy sources. . . THE MOLE. Mole. -The . number of C atoms in exactly 12.0 g of carbon., also a number 6.022 x 10. 23. Avogadro’s number . 6.022 x 10. 23. , the number of . particles. in a mole of . anything. More on the mole later……. Moles and Mass. The . molar mass . gives us the relationship between the . number of moles . and the . mass of an element or compound. .. We can . use the molar mass . to . calculate . the . mass. or . Mr. Guerrero. Stoichiometry. Homework, due on the day of chapter exam. . Zumdahl. Text, 9. th. ed. . page 126: . #10, 13, 18, 38, 40, 46, 50, 66, 74, 84, 86, 88, 100, 106, 122, 124, 126.. Write out all conceptual(non-math) questions & answer in complete sentences.. Atomic mass. Atoms of different elements have different masses. . Mass of a single atom is incredibly small so a special unit called atomic mass unit (. amu. ) is used. . Atomic Mass. Atoms are composed of three particles:. Due at end of Period. The compound . benzamide. has the following percent composition. What is the empirical formula? . C . = 69.40 % H= 5.825 % O = 13.21 % N= 11.57 % . 2. A . component of protein called serine has an approximate . I. Percent Composition. Think about this:. How would you find the percent of boys in our class?. # of boys (part)____. x 100% . Total # of students (whole). I. Percent Composition. . Determining Molecular Formulas. Calculate the molecular formula of a compound whose molar mass is 60.0 g/mol and has an empirical formula of CH4N.. What you need:. Empirical Formula. Molar Mass. Calculate the molar mass of the empirical formula.