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Chemistry I February 1st – 5th Name___________________________ Muhiga Weekly Moles Monday, Find molar mass of PCl3 Tuesday, What is the mass of 1.00 mol of sodium hydrogen carbonate? Wednesday, Find molar mass. CO2 SF7 Thursday, Calculate the mass, in grams, of 2.50 mol of iron (II) hydroxide. Chemistry I February 1st – 5th Name___________________________ Muhiga Weekly Moles Daily Homework: Monday, Feb 01: Mole Activity Questions Tuesday, Feb 02: Read 10.1 pg. 306-315 Ques. 9-15 Wednesday, Feb 03: Mole-mass Worksheet Thursday, Feb 04: Read 10.2 pg 317-323, Ques. 24-32 Friday, Feb 05: No School Events this Week: 02/01: Ch 10: The Mole Activity 02/02: Ch 10.2: Mole -Mass 02/03: Ch 10.2: The Mole -Volume 02/04: Ch 10.3: Percent Composition 02/05: No School State Standards: C. 4.3: Given mass of a sample, use the mole concept to determine the number of moles and number of atoms or molecules in samples of elements and compounds. C. 4.7: Perform calculations to determine the composition of a compound or mixture when given the formula Key-Terms/ Vocabulary: mole, Avogadro’s # representative particles, molar mass, Avogadro’s hypothesis, standard temperature and pressure (STP), molar volume, percent composition, empirical formula, molecular formula. Objectives: Check off the objectives once you feel you understand the material well. I will be able to: ___: Convert any given amount of substance to the needed quantity. ___: Explain/show how chemists measure and count substances. ___: Determine the molar mass of an element or compound. ___: Use dimensional analysis to convert the mass of a substance to moles, or moles to mass. ___: Use dimensional analysis to convert the volume of a gas at STP to the number of moles, or moles to volume at STP Big Idea This Week The mole (mol) is a unit used to count particles indirectly. A mole, also called Avogadro’s number may be expressed as 6.02 x 10 23, gram molecular mass and molar mass of the representative particles of that substance (atoms, ions, molecules or formula units). One mole of a gas occupies a volume of 22.4 L at STP (standard temperature and pressure). Standard pressure is equivalent to 101.3 kPa, 1atm, or 760 mm Hg, while standard temperature is equivalent to 273 K, 00C or -32 0F. The molar mass of an element is the numerical equivalent of the atomic mass (amu) in grams. Subscripts in a chemical formula indicate how many mols of each element are in one mol of the compound. The molar mass of a compound is the sum of all the masses of the moles of elements present in the compound Inter-conversions between moles and other quantities, e.g., grams, particles and liters may be accomplished using dimensional analysis. In determining the formula of a compound, the relative amounts of the elements present in the compound should be obtained through measurement. This information is then expressed as the percent composition.