PPT-Mole Review 1.) Calculate the number of moles in 60.4L of O

2 2 How many moles are there in 632g of Cl 2 604L O 2 224L O 2 1 mol O 2 27 mol O 2 632g Cl 2 70g Cl 2 1mol Cl 2 0903mol Cl 2 Ch 9 Math In Chemistry. HIGHER LESSON. Learning Objectives. To . explain. what chemical equations tell us about chemical reactions. To . explain. how we use equations to calculate masses of reactants and products. HIGHER LESSON. HIGHER LESSON. Learning Objectives. To . explain. what chemical equations tell us about chemical reactions. To . explain. how we use equations to calculate masses of reactants and products. HIGHER LESSON. They tell us how much of each substance is involved in a chemical reaction. 2H. 2. + O. 2. .  2H. 2. O. 2 moles of hydrogen react with 1 mole of oxygen to make 2 moles of water. This is useful because now we can use it to work out what mass of hydrogen and oxygen we need and how much water is made. 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 . Use . the coefficients to predict the amount of reactant consumed or product formed. The ratio of the coefficients is a ratio of the moles taking part in a reaction.. Reactants (on the left of the arrow) are consumed. Chapter Objectives. Describe the chemical processes used in biomass production and conversion to biofuels.. Explain balancing a chemical reaction as an application of the . law of conservation of mass. 12.00 g C-12 = 1 mol The number of particles in 1 mole isatoms 1 mol6.022 The Mole in Chemistry . Not this!!. Not this!!!. The Mole. The mole is a counting unit. 1 pair = 2. 1 dozen = 12. 1 mole = 6.022 x 10. 23. atoms. This number is known as Avogadro’s number after Italian chemist . 2. O. 3. ) . C/W. 23/09/2020. 3.2.1. Ar of Al = 27. Mass of Al in Al. 2. O. 3. = 27 x 2 = 54. Mr of Al. 2. O. 3. = (27x2) +(16x3) = 102. Percentage of aluminium = 54/102 x 100 = 52.94%. Progress Outcomes. Chapter 9. History. About 200 years ago scientists needed a unit of measure that connected the mass of a molecule or atom with how many of them there were. . Amadeo Avogadro proposed his hypothesis in 1811. At that time, there was no data on the number of particles in a mole, or an agreement on any atomic weights or the standard. . 23. How do you measure how much?. You can measure mass, . or volume,. or you can count pieces.. We measure mass in grams.. We measure volume in liters.. We count pieces in . MOLES.. . Counting. . Counting words are used to simplify a description of a number of items. . Matter is made of different kinds of particles. . We count the number of particles of that substance. . Since there are a very large number of particles in any substance, we need to define a unit of measure:.  . What’s a mole?. The . mole. is a unit of . measure. .. Just like meters tells us . length. and seconds tells us how much . time. , . the . mole. measures an . amount. . (how much).. Units of measure similar to mole include: . r. ). Total of all the relative atomic masses of all the atoms in the compound. % mass of an element in compound . =. A. r. x number of atoms of that element. M. r. of the compound. x100. e.g. % by mass of chloring in MgCl.