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Chemistry

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2nd Semester Chem Final Doc

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2nd Semester Practice Chemistry Final 2009-2010 Multiple Choice: Identify the letter of the choice that best completes the statement or answers the question. 1. What happens to the volume of a gas during compression? a. The volume increases. b. The volume decreases. c. The volume remains constant. d. It is impossible to tell because all gases are different. 2. Name the compound Fe(NO3)2. a. iron(II) nitrate c. iron(I) nitrite b. iron(II) nitrite d. iron nitrate 3. What is the molar mass of (NH4)2SO4? a. 114.09 g/mol c. 128.06 g/mol b. 118.34 g/mol d. 132.13 g/mol 4. What is the pressure exerted by 1.2 mol of a gas with a temperature of 20.?C and a volume of 9.5 L? a. 0.030 atm c. 3.0 atm b. 1.0 atm d. 30. atm

zumdahl 2 power point chapter 2

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AP Chemistry A. Allan Chapter 2 Notes - Atoms, Molecules and Ions 2.1 The Early History Refer to the Chemistry History Timeline for this chapter 2.2 Fundamental Chemical Laws A. Law of Conservation of Mass 1. "Mass is neither created nor destroyed" 2. Translation: In ordinary chemical reactions, the total mass of the reactants is equal to the total mass of the products B. Law of Definite Proportion 1. "A given compound always contains the same proportions of elements by mass" 2. Translation: Compounds have an unchanging chemical formula C. Law of Multiple Proportions 1. "When two elements form a series of compounds, the ratios of the masses of the second element that combine with one gram of the first element can always be reduced to small whole numbers

asd

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Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 25 oC and a pressure of 754 mm Hg. If the wet H2 gas formed occupies a volume of 8.73 L, the number of grams of H2 formed is 0.691 g. The vapor pressure of water is 23.8 mm Hg at 25 oC. Feedback: The total pressure over the water in the collection vessel is equal to the sum of the partial pressure of H2 and the vapor pressure of water at 25.0. Therefore the partial pressure of H2 is calculated as PH2 = Ptotal - PH2O = 754 mm Hg - 23.8 mm Hg = 730 mm Hg

a

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A?33.0?mL sample of a?0.406?M aqueous?hypochlorous acid?solution is titrated with a?0.387?M aqueous?barium hydroxide?solution. What is the pH after?6.54?mL of base have been added? pH =??7.24 Feedback: Please note that while the results of the intermediate calculations below are displayed rounded to 3 significant digits, the actual calculations are done internally without rounding. When the strong base,?Ba(OH)2, is added, the weak acid reacts to neutralize the OH-.The balanced equation is:? 2?HClO?+?Ba(OH)2??Ba(ClO)2?+?2?H2O The initial number of moles of the weak acid?HClO?is given by?0.406?M??3.30E-2?L =?1.34E-2?mol Similarly, the number of moles of?Ba(OH)2?added is given by?0.387?M??6.54E-3?L =?2.53E-3?mol

Chapter 11 Vocab

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Chemistry Chapter 11 Vocabulary Avogadro?s number: the number 6.02 x10^23, which is the number of representative particles in a mole Empirical formula: a formula that shows the smallest whole number mole ratio of the elements of a compound Hydrate: a compound that has a specific number of water molecules bound to it?s atoms Molar mass: the mass in grams of one mole of any pure substance Mole: base unit used to measure the amount of a substance Molecular formula: a formula that specifies the actual number of atoms of each element in one molecule or formula unit of the substance Percent composition: the percent by mass of each element in a compound

Half Lives

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half-life. radioisotope

Half Life The time required for one half of a radioisotope?s nuclei to decay into its products Amount Time # of ? Lives Equations: To solve for amounts: To solve for Time: Variables: T: time elapsed : half Life
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Chemical reactions

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Electrochemical reactions involve the transfer of electrons. Mass and charge are conserved when balancing these reactions, but you need to know which atoms are oxidized and which atoms are reduced during the reaction.?Oxidation numbers?are used to keep track of how many electrons are lost or gained by each atom. These oxidation numbers are assigned using the following rules: The convention is that the cation is written first in a formula, followed by the anion. For example, in NaH, the H is H-; in HCl, the H is H+. The oxidation number of a free element is always 0. The atoms in He and N2, for example, have oxidation numbers of 0. The oxidation number of a monatomic ion equals the charge of the ion. For example, the oxidation number of Na+?is +1; the oxidation number of N3-?is -3.

Alum Lab

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Umair and Zubair Khan 9-16-11 Block 1 Title: Alum Synthesis Lab Report Introduction/Purpose: Among the several purposes of this lab were: Synthesize Alum from Aluminum so that the Alum crystals can be tested to verify how pure the compositions and properties of the experimental alum are compared to theoretical values. To get familiar with accurate methods of weighing, gravity and vacuum filtration, and crystallization. To become familiar with the use of laboratory equipment such as beakers, Test tubes, Erlenmeyer flasks, Hot Plates, Burets, Buchner Apparatuses, Capillary Tubes, Thermometer,etc. To practice Stochiometry to determine the percent yield of alum synthesized from aluminum Procedure Part 1:

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