Ch.11 Chemistry Mole – Flashcards
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How do you find a substance's molar mass?
answer
By adding the mass of each element in a compound.
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How many moles are in 10.0 g of Al?
answer
10g Al x ( 1 Mol Al/26.98 g Al) = .371 Mol Al
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How many atoms are in 10 G of Al
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10g Al x(1 Mol Al/26.98 g Al) x (6.011 x 10 23 Atoms Al)/1 Mol Al 1 Mol/ 6.022 x10 23 Atoms Atomic Mass of element in Grams/ 1 Mol Element
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Calculate th percent by mass of Al in Aluminum hydroxide (Al(OH)3)
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Al= 26.98 O=16.0 x3= 48 H= 1.01 x3 = 3.03 Molar mass = 78.01 Al = 26.98 is what % of 78.01? Al= 34.6%
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Calculating Empirical formulas
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Example: A sulfur compound contains 50% Sulfur and 50% O Find the Empirical Formula 100 g of compound contains 50g S and 50 g of O No of Moles of Atoms 50/32.07 = 1.56 mol S 50/16.0 = 3.114 mol of O Empirical formula = SO2 There is twice as many moles of O as there is S
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Molecular Formula
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A compound is found to be made up of 71.9% Carbon, 12.13% Hydrogen and 15.97% Oxygen The Compound has a Molecular weight (Molar Mass) of 300.54 g Determine the actual chemical formula for the compound. 100 grams of compound contains 71.9g C, 12.13g H, 15.97g O No of Moles of Atoms 71.9g C / 12.01 = 5.9 9 Moles of C 12.13g H /1.01 = 12 Moles of H 15.97 g O / 16.0 = 1 Mol of O Empirical Formula = c6h12o Molar Mass of Empirical Formula =100.18 Molecular Formula = C18H36O3
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Hydrates
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An analysis of a hydrate is found to contain 639% Copper II Sulfate (CuSO4) and 36.1% Water Calculate the simplest formula for this hydrate. 100g compound contains 63.9% CuSO4, 36.1% H2O # of Moles of Atoms 63.9/159.62 = .4 Moles of CuSO4 2.003/0.400 = 2.003 moles of H2O Empirical Formul o the Hydrate = CuSO4 ¥ 5H2O
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