will learn to determine the formula mass of a substance and thenumber of moles of a substance. You will practice writing and balancing chemical equations,and you will learn to use these equations in determining the amounts of substances that reactand are produced in chemical reactions.actice ExercisesThe formula mass (Sec. 6.1) of a compound is the sum of the atomic masses, expressed inatomic mass units (amu), of the atoms in the chemical formula of the substance. Calculate theformula mass, rounded to the hundredths place, for each of the compounds below. Atomicmasses are given on the inside front cover of your textbook.FormulaCalculations with atomic massesFormula massK= 39 + Br=80Chこ35C03%3D100119.00amu75amu146.00amKBrCa=40CaCl,Na,CO,(NH,),PO,The mole (Sec. 6.2 and 6.3) is a useful unit for counting numbers of atoms and molecules.The number of particles in a mole is 6.02 x 103, which is known as Avogadro's number(Sec. 6.2). Use the definition of Avogadro's number as a conversion factor in the calculationsbelow:MolesQuantity with conversion factořNumber of atoms1.00 mole He atoms2.60 moles Na atoms0.316 mole Ar atomsThe mass of mole, the molar mass (Sec. 6.3), of any substance is its formula mass (amu)expressed in grams. Answer the questions below to check your understanding of molar mass.1. What is the mass in amu of one carbon atom?2. What is the molar mass of carbon?3. How many atoms of carbon are in 1 molar mass of carbon?4. What is the mass of three moles of carbon atoms?5. How many carbon atomns are in 36.03 g of carbon?45Cengage Learning. All Rights Reserved. May not be scanned, copied or duplicated, or pastcd to a publicly accessible website, in whole or in part. Chemical Calculations: Formula Masses,Moles, and Chemical EquationsChapter 6Chapter OverviewCalculation of the ratios and masses of the substances involved in chemical reactions is veryimportant inmole, a convenient counting unit for atoms and molecules.In this chapter you will learm to determine the formula mass of a substance and thenumber of moles of a substance. You will practice writing and balancing chemical equations,and you will leam to use these equations in determining the amounts of substances that reactand are produced in chemical reactions.a many chemical processes. Central to these calculations is the concept of thePractice Exercises6.1The formula mass (Sec. 6.1) of a compound is the sum of the atomic masses, expressed inatomic mass units (amu), of the atoms in the chemical formula of the substance. Calculate theformula mass, rounded to the hundredths place, for each of the compounds below. Atomicmasses are given on the inside front cover of your textbook.FormulaCalculations withomic massesFormula mass119.00amu75amuNA2= 410 CO3 = 0H6.00amu= 39 + Br=80KBrCa=40Chこ35CaCl,Na,CO,(NH,),PO,6.2The mole (Sec. 6.2 and 6.3) is a useful unit for counting numbers of atoms and molecules.The number of particles in a mole is 6.02 x 10, which is known as Avogadro's number(Sec. 6.2). Use the definition of Avogadro's number as a conversion factor in the calculationsbelow:MolesQuantity with conversion factorNumber of atoms1.00 mole He atoms2.60 moles Na atoms0.316 mole Ar atomsThe mass of 1 mole, the molar mass (Sec. 6.3), of any substance is its formula mass (amu)expressed in grams. Answer the questions below to check your understanding of molar mass.6.31. What is the mass in amu of one carbon atom?2. What is the molar mass of carbon?3. How many atoms of carbon are in 1 molar mass of carbon?4. What is the mass of three moles of carbon atoms?5. How many carbon atoms are in 36.03 g of carbon?45O 2016 Cengage Learning All Rights Reserved. May not be scanned, copied or duplicated, or posted to a publicly accesa ble webaite, in whole or in part.

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Formula Calculations with atomic masses Formula mass 119.00amu 75amul 146.00am K= 39 + Br=80 KBr Ca-40 CLこ35 CaCl2 Naz=40 CO3 = Na,CO, (NH),PO. The mole (Sec 6 2 and 6 2) in n voeful ueit fe