Atoms, Ions and Molecules Calculations
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1 Atoms, Ions and Molecules Calculations 1. How do you calculate the atomic mass of an element? Atomic Mass = (% abundance of isotope 1)(mass of isotope 1) + (% abundance of isotope2)(mass of isotope 2) +.. Include every isotope for the given element in this calculation. a. What is the atomic mass of copper if 63 Cu has a mass of amu and percent abundance of 69.09% and isotope 65 Cu has a mass of amu and percent abundance of 30.91%. (62.93 amu)(0.6909) + (64.93 amu)(.3091) = amu b. What are the percent abundances for 151 Eu and 153 Eu if the atomic mass of the element is amu and the isotope masses are amu and amu respectively? Remember that, as there are only 2 isotopes, their combined percent abundances must equal 100%. Thus = ( )(x) + ( )(y) Where x equals the percent abundance (in decimal form) of 151 Eu and y equals the percent abundance of 153 Eu. x% + y% = 100% or x + y = 1 so = ( )(x) + ( )(1-x) x= % y= %
2 2. What is a mole? A mole is a convenient way of describing a very large quantity of something. 1 mole = x particles (6.022 x is known as Avogadros number) 3. How does the molecular formula relate to the number of moles? The molecular formula indicates the number of individual atoms of a particular element in a given molecule. This value is directly equal to the number of moles of a given element within a mole of a molecule. For example, in C 6 H 6, there are 6 carbon atoms in every one molecule of C 6 H 6. This can also be understood as 6 moles of carbon for every mole of C 6 H What is the molar mass of a compound? It is the of a given substance. Molar mass = (Number of moles of element 1 in compound)(atomic mass of element 1) + (number of moles of element 2 in compound)(atomic mass of element 2)+. Atomic mass of each element is obtained from the periodic table. a. Calculate the molar mass of C 6 H In 3.35 x total atoms of CH 3 OH there are how many a. Molecules
3 b. Moles c. Grams For this problem you needed to solve for the molar mass of the CH 3 OH first using techniques already discussed. 6. What is % composition (by mass)? The percent that an element, within a given compound, contributes to the overall molar mass. 7. Fungal laccase is 0.390% Cu by mass. If a fungal laccase molecule contains 4 copper atoms, what is the molar mass of fungal laccase? Solving for molar mass of fungal laccase 6.52 x 10 4 g/mol
4 8. Combustion is a technique frequently used to determine the formula of an unknown substance (typically a hydrocarbon). When using this experimental method the empirical formula is obtained this is the formula with the most reduced ratio between atoms). Using this and the actual molar mass of the compound a molecular formula can be determined. For example: CH would be the empirical formula for the molecular formula C 4 H 4 CO 2 would be both the empirical and molecular formula for carbon dioxide as the molecular formula is already in its most reduced form. 9. Combustion requires the presence of oxygen. 10. H x C y + O 2 (g) H 2 O (g) + CO 2 (g) 11. Terephthalic acid contains C, H and O. Combustion of mg terephthalic acid produces mg CO 2 and 6.45 mg H 2 O. If mol of terephthalic acid has a mass of 41.5g, determine the molecular formula of terephthalic acid. Gather the pertinent data points: mg terephthalic acid was combusted mg of CO 2 was produced (this will give us information about the amount of carbon present in the original sample.) 6.45 mg of H 2 O was produced (this will give us information about the amount of hydrogen present in the original sample.) Step 1 Determine the amount of carbon, hydrogen and oxygen present in original terephthalic acid sample.
5 As there were no sources, other than the terephthalic acid, for the C and H. The amounts of the C and H contained in the CO 2 and H 2 O are the same as the amounts contained in the original sample. How about the O? Since the compound is only made up of C,H and O. The sum of the individual masses of each must equal the total mass sample so g terephthalic acid g C x 10-4 g H = g O Step 2 Determine the % by mass of each element in the terephthalic acid Step 3 Determine the number of moles of C, H, O contained in a 100g sample of terephthalic acid.
6 Step 4 Solve for the smallest whole number ratio between the values of moles determined in the previous step. Step 5 Solve for the factor using the formula below. Multiply the mole ratio of the empirical formula by the factor to determine the molecular formula. The problem indicated that.250 moles of terephthalic acid had a mass of 41.5g. This information indicates the molar mass. Remember that MM=g/mol so.
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![7. How many moles of hydrogen sulfide are contained in a 35.0-g sample of this gas? [A] 2.16 mol [B] 7.43 mol [C] 6.97 mol [D] 10.4 mol [E] 1.](/thumbs/74/71034449.jpg "7. How many moles of hydrogen sulfide are contained in a 35.0-g sample of this gas? [A] 2.16 mol [B] 7.43 mol [C] 6.97 mol [D] 10.4 mol [E] 1.")
1. Bromine exists naturally as a mixture of bromine-79 and bromine-81 isotopes. An atom of bromine-79 contains [A] 35 protons, 44 neutrons, 35 electrons. [B] 79 protons, 79 electrons, and 35 neutrons.