2H
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A 3.00 L bottle weighs 1.70 kg.
When filled with wine, it weighs 4.72 kg.
The wine contains 11.5% ethanol by mass.
Calculate the grams of ethanol in 250.0 mL of this wine.
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A reaction of 0.406 g magnesium with oxygen produces 0.674 g magnesium oxide.
Calculate the mass of oxygen consumed in the reaction:
Reaction: Mg + 1/22 Mg → 0.4063 + x
0.6743 - 0.4063 = 0.2683 g for oxygen consumed.
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In an experiment, 2.18 g of sodium reacts with 16.12 g of chlorine.
All sodium is consumed resulting in 5.54 g of sodium chloride (table salt).
In a second experiment, 2.10 g of chlorine reacts with 10.00 g of sodium.
All chlorine is consumed yielding 3.46 g of sodium chloride.
Demonstrate that these results adhere to the law of definite proportions.
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Data obtained for compounds formed between nitrogen and hydrogen:
Nitrogen:
Mass 1 (g): 0.500
Mass 2 (g): 0.108
Mass 3 (g): 1.000
Mass 4 (g): 0.0720
Mass 5 (g): 0.750
Mass 6 (g): 0.108
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Calculating ratios for compound formation:
Example calculations for different ratios involving nitrogen and hydrogen.
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The standard for atomic masses is based on Carbon-12.
Carbon's atomic mass appears as 12.011 due to natural isotopes.
Carbon-12 is the standard, but Carbon-13 is also present in nature.
Average atomic masses take into account the natural abundance of isotopes.
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Silver has two natural isotopes with the following abundances:
51.84% of 107 Ag
48.16% of 109 Ag
Given 107 Ag's mass of 106.905092, calculate the mass of 109 Ag:
Use the equation Ag = 107.87.
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Properties of the periodic table:
Elements are organized by increasing atomic number.
Similar elements are grouped vertically.
Group examples: Sodium and Potassium in Group 1.
Chlorine is located in Group 17 (Halogens).
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Group 1: Alkali metals
Period 3:
Group 17: Halogens
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Elements are classified into metals and nonmetals.
Metals are generally solid at room temperature (except mercury).
Nonmetals exhibit opposite properties to metals (e.g., poor electrical conductivity).
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Noble gases and metalloids are small element groups in the periodic table.
Periods are horizontal arrangements of the periodic table.
First period contains just Hydrogen and Helium.
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Group number identification can vary:
Newly adopted IUPAC numbering system (1-18).
Older American notation with letters and numbers.
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Each element is represented in boxes:
Element symbol, atomic number (above), and average atomic mass (below).
Some tables include other properties (e.g., density).
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The periodic table organizes elements by atomic number:
Each group shares similar physical and chemical properties.
Classification includes metals, nonmetals, metalloids, and noble gases.
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Concept of moles and Avogadro's number:
Avogadro's number: 6.02214 x 10^23.
Represents the number of units in one mole of a substance.
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The mole concept is frequently used in calculations.
For example: 1 mol of sulfur (S) = 6.022 x 10^23 atoms = 32.065 g.
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Avogadro's number relates to atomic quantities in moles:
1 mole indicates the number of units in a particular elemental mass.
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Example weights of different atoms for 6.02214 x 10^23 atoms:
Fluorine (F): 18.9984 g
Chlorine (Cl): 35.453 g
Magnesium (Mg): 24.3050 g
Lead (Pb): 207.2 g
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Calculate the number of Cu atoms in a silver alloy weighing 33.24 g:
Sterling silver contains 92.5% silver by weight.
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A graduated cylinder filled halfway with 8.0 g of diatomaceous earth, mostly composed of silica.
Calculate the volume of water needed to fill the cylinder to the 100.0 mL mark:
Density of diatomaceous earth is 2.2 g/cm³.