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Ideal Gas Law The gas law which describes the relationship between P, V, n, R, and T in an equation where moles are present. P represents pressure, V represents volume, T represents temperature, n represents the number of moles given in the equation, and R is a number which eliminates all units of measurement in the equation and is measured in either atm, torr, or Pa, depending on what information is given. The equation is written as: P x V = nRT Example: A gas system has pressure,volume and moles of 1190torr, 2.29L and 0.193moles, respectively. What is the temperature in K? Step 1: Determine values to input into equation P = 1190torr | V = 2.29L | T = ? | n = 0.193moL | R = 62.364 Step 2: Convert all units (if necessary) to L and K Step 3: Plug in values & simplify/Solve the equation 1190torr x 2.29L = 0.193moL(62.364torr)( T ) Note: R eliminates all units 1190 x 2.29 = 0.193(62.364)( T ) 2,725.1 = 12.036252T 226.407689 = T Answer: T = 226K Step 4: Apply units and significant figures 123
The Learning Goal for this assignment is: The students will learn how the interactions between water molecules account for the unique properties of water and how aqueous solutions form. Take note over the following chapter. Use the Headings provided to organize your notes. Define and number all highlighted vocabulary (total 22 ) as well as summarize and take notes over the sections. You may add pictures where needed. The pictures should be an appropriate size. Use Arial 12 for all text. This document should be 2 pages and should be saved as a pdf before you submit it into Angel. Chapter 15 Water and Aqueous Systems Pages 488 - 507 15.1 Water and Its Properties Water in the Liquid State - (Q) What factor causes the high surface tension, low vapor pressure, and high boiling point of water? Water is a polar molecule consisting of 3 atoms, 1 oxygen atom and 2 hydrogens. The oxygen forms a covalent bond with each of the hydrogens. The oxygen has a greater electronegativity than hydrogen, so it attracts the electron pair of the O – H bond to a greater extent. Thus, the O – H bond is highly polar. The oxygen (more electronegative) gains a partial negative charge, and the hydrogen (less electronegative) gains a partial positive charge. Generally, polar molecules are attracted to each other by dipole interactions. The negative end of one attracts the positive end of another. This attraction between poles of water molecules results in hydrogen bonding. Hydrogen bonds aren’t as strong as covalent bonds, but they are stronger than other intermolecular forces. (A) Many unique and important properties of water – including its high surface tension, low vapor pressure, and high boiling point – result from hydrogen bonding. You may have noticed that water forms almost perfectly spherical, or slightly ovular, droplets (i.e. rain drops or dew on grass). Or that when a cup is overflowing with water, the water just bulges slightly above the rim. This is due to surface tension. || Surface Tension [1]: The inward force, or pull, that tends to minimize the surface area of a liquid. || Water has a uniquely high surface tension, and this is attributed to its ability to form hydrogen bonds. The molecules on the surface of a droplet, unlike the ones inside which form hydrogen bonds to every nearby water molecule, can only bond to the other molecules inside of the drop. Thus, the water molecules at the surface tend to be drawn inward. || Surfactant [2]: Any substance that interferes with the hydrogen bonding between water molecules and thereby surface tension. || To decrease the surface tension of water, you can add surfactants (i.e. soaps and detergents). Adding detergent to water on a greasy surface decreases surface tension in the water, and causes the droplets to flatten out. Hydrogen bonds also explain waters unusually low vapor pressure. This low vapor pressure caused by hydrogen bonding allows water to maintain its liquid state in conditions that would usually evaporate a liquid. Thus allowing for water to sustain life. Hydrogen bonds also cause water to have an abnormally high boiling point for such a low molar mass (18.0g/mol). If it wasn’t for water’s high boiling point, and it was as volatile as ammonia in its boiling point, it would exist as a gas at Earth’s normal temperature. Again, these properties make it ideal for sustaining life. Water in the Solid State 15.2 Homogeneous Aqueous Systems 124
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Chemistry Notebook By: Joel J
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Unit 1 Measurement Lab Separation o
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Unit 5 (28 days) Chapter 10 Chemica
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30. Always lubricate glassware (tub
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Chapter 1 Unit 1 Introduction to Ch
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To use the Stair-Step method, find
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Using SI Units Match the terms in C
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Standards of Measurement Fill in th
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SCIENTIFIC NOTATION RULES How to Wr
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Convert each number from Scientific
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Significant Figures Rules There are
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How Many Significant Digits for Eac
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The following rule applies for mult
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1qt=32 oz 1gal = 4qts 1.00 qt = 946
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Chapter 5 Electrons in Atoms The st
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Atoms Are Building Blocks Atoms are
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Electrovalence Don't get worried ab
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Summary Atoms are essentially the b
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Electron Configuration Color the su
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Electron Configuration In order to
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Calcium (Ca) Nickel (Ni) Carbon (C)
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Research the Scientist and summariz
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Using Wikipedia, define the 8 categ
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Ionization Energy Define Ionization
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Ion Size Define Ion Size: Ion size
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Chapter 7 Ionic and Metallic Bondin
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10. Name __________________________
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The Nucleus A typical model of the
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Gamma Radiation After a decay react
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This analysis shows that sodium has
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Metals, with only a few electrons i
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POLAR BONDING results when two diff
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Step 6 Put the atoms in the structu
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Trigonal Planal Molecular Geometry
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Tetrahedral Molecular Geometry Orbi
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Bent Molecular Geometry Orbital Equ
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Page 77 and 78: Square Planar Molecular Geometry Or
Page 79 and 80: sp 3 d 2 AX6 None 90 Octahedral sp
Page 81 and 82: Chapter 9 Unit 4 Chemical Names and
Page 83 and 84: Learning Goals: Describe the proper
Page 85 and 86: Unit 5 Chapter 10 Chemical Quantiti
Page 87 and 88: www.youtube.com/watch?v=AsqEkF7hcII
Page 89 and 90: Categories of Reactions All chemica
Page 91 and 92: List what type the following reacti
Page 93 and 94: How to Balance Chemical Equations A
Page 95 and 96: Step 5 Balance the hydrogen atoms n
Page 97 and 98: 6) ___ Mn(NO2)2 + ___ BeCl2 ___ Be
Page 99 and 100: The Learning Goal for this assignme
Page 101 and 102: Stoichiometry and Balanced Equation
Page 103 and 104: Step 1: 200g C3H8 is equal to 4.54
Page 105 and 106: Stoichiometry and balanced equation
Page 107 and 108: %yield = 6.1 tons × 100 = 64% 9.6t
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Page 111 and 112: Unit 6 Chapter 13 States of Matter
Page 115 and 116: uniform internal structure, and amo
Page 117 and 118: Volume Pressure Temperature is Aver
Page 119 and 120: Volume and temperature (in Kelvins)
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Page 125: Combined Gas Law: This gas law comb
Page 129 and 130: Unit 7 Chapter 16 Solutions The stu
Page 133 and 134: Part 5: Molarity Molarity (M) is th
Page 137 and 138: The Time-Temperature Graph We are g
Page 139 and 140: Step Two: solid ice melts Now, we c
Page 141 and 142: Step Four: liquid water boils Now,
Page 143 and 144: The following table summarizes the
Page 145 and 146: The Learning Goal for this section
Page 147 and 148: B. decreasing the concentration of
Page 149 and 150: everse reaction rate as well. 11. I
Page 151 and 152: Unit 8 Chapter 19 Acid and Bases Th
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Page 155 and 156: This would be a generic base: XOH -
Page 157 and 158: HCl + H2O ⇌ H3O + + Cl¯ HCl - th
Page 159 and 160: Several categories of substances ca
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Page 165: 2. What is the oxidation number of
Page 170 and 171: Table E Selected Polyatomic Ions Fo
Page 172 and 173: Table H Vapor Pressure of Four Liqu
Page 174 and 175: Table K Common Acids Table N Select
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Table R Organic Functional Groups C
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Table S Properties of Selected Elem
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Table T Important Formulas and Equa
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CHEMISTRY EXAM FORMULA AND RESOURCE
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Activity Series of Metals Name Symb
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