MOLAR MASS AND MOLECULAR WEIGHT Themolar mass of a molecule is the sum of the atomic weights of all atoms in the molecule. Molar Mass.

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1 Counting Atoms Mg burns in air (O 2 ) to produce white magnesium oxide, MgO. How can we figure out how much oxide is produced from a given mass of Mg? PROBLEM: If If g of Mg is is burned, how much MgO is is formed? Mg has a molar mass of g/mol g g 8.23 x 10-3 mol That means that mol of MgO is formed and is composed of mol of Mg and mol of O mol of O has a mass of ( mol) (16.0 g/mol) g. So the mass of MgO is g Notice that I use unit analysis. Reminder: The molar mass (also called atomic weight) for each element is found on the periodic table. Molar Mass 12 Mg atomic number symbol atomic weight So the magnesium found on earth weighs grams for each mole. MOLAR MASS AND MOLECULAR WEIGHT Themolar mass of a molecule is the sum of the atomic weights of all atoms in the molecule. This is sometimes called molecular weight. To calculate molar mass of a molecule, simply add all molar masses of all the components.

2 What is the molar mass of ethanol, CH 3 CH 2 OH? of ethanol contains 2 mol C (12.01 g /mol C) g C 6 mol H (1.01 g /mol H) 6.06 g H O (16.00 g /mol O) g O How many molecules of alcohol are there in a standard can of beer if it contains 21.3 g of CH 3 CH 2 OH? We know there are mol of CH 3 CH 2 OH mol x 1023 molecules 2.78 x molecules TOTAL molar mass g/mol How many moles of alcohol are there in a standard can of beer if it contains 21.3 g of CH 3 CH 2 OH? (a) Molar mass of CH 3 CH 2 OH g/mol (b) Calculate the moles of alcohol 213. g g / mol mol (c) Notice the units they show by cancellation how to write the equation. How many atoms of C are there in the ethanol in a standard can of beer? We know there are 2.78 x molecules of ethanol. Each molecule contains 2 C atoms. Therefore, the number of C atoms is 2.78 x molecules 2 C atoms ecule 5.56 x C atoms

3 Empirical and Molecular Formulas A pure compound always consists of the same elements combined in the same proportions by weight. Therefore, we can express molecular composition as PERCENT BY WEIGHT Ethanol, C 2 H 6 O, is 52.13% C, 13.15% H and 34.72% O by weight Consider NO 2 What is the weight percent of N and of O in NO 2? M g/ mol g/ mol 46. 0g/ mol Percent Composition Wt. % N Wt. % O 14.0 g N / mol 46.0 g NO / mol 2 2(16.0 g O / mol) 46.0 g NO / mol 2 100% 30.4 % 100% 69.6 % Empirical and Molecular Formulas Why? The molar mass of ethanol is g/mol. Of that mass, the amount due to carbon is g/mol, that due to hydrogen is 6.06 g/mol and that due to oxygen is g/mol. For C, 24.03/ % For H, 6.06/ % For O, 16.00/ % Determining Formulas In chemical analysis we determine the % by weight of each element in a given amount of pure compound and derive the EMPIRICAL or SIMPLEST formula. PROBLEM: A compound of B and H is 81.10% B by weight. What is its empirical formula?

4 First some logic: Because the compound contains only B and H, it must contain 18.90% H. In g of the compound there are g of B and g of H. Now use this to calculate the number of moles of each constituent in this amount of compound. Now, recognize that atoms combine in the ratio of small whole numbers. For example, for boron trihydride 1 atom B + 3 atoms H ecule BH 3 or B atoms + 3 mol H atoms BH 3 molecules Now find the ratio of moles of elements in our compound. Calculate the number of moles of each element in g of sample g B g H g g mol B mol H Take the ratio of moles of B and H. Always divide by the smaller number mol H mol B mol H mol B But we need a whole number ratio. 2.5 mol H/1.0 mol B 5 mol H / 2 mol B EMPIRICAL FORMULA B 2 H mol H 1.0 mol B

5 What is its molecular formula? Tylenol Is the molecular formula B 2 H 5, B 4 H 10, B 6 H 15, B 8 H 20, etc.? To determine this we need to know the molar mass. In this case, the molar mass (or molecular weight) is 53.3 g/mol. Formula C 8 H 9 NO 2 Molar mass g/mol What is the percent weight of N in this compound? What is its What is its molecular formula? Compare this value, 53.3 g/mol with the mass of B 2 H g/unit (the smallest possible unit with a 2:5 ratio). Now find the ratio of these masses g/mol 2 units of B H g/unit of B2H5 1mol Molecular formula B 4 H 10

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