Chem 1 Worksheets WSHEET 1: Working with Numbers Practice
... 1. Calcium fluoride, CaF2, is a source of fluorine and is used to fluoridate drinking water. Calculate its molar mass. 2. Calculate the molar mass of Ca(BO2)2·6H2O. 3. Calculate the number of moles in 17.8 g of the antacid magnesium hydroxide, Mg(OH)2. 4. Calculate the number of oxygen atoms in 29.3 ...
... 1. Calcium fluoride, CaF2, is a source of fluorine and is used to fluoridate drinking water. Calculate its molar mass. 2. Calculate the molar mass of Ca(BO2)2·6H2O. 3. Calculate the number of moles in 17.8 g of the antacid magnesium hydroxide, Mg(OH)2. 4. Calculate the number of oxygen atoms in 29.3 ...
Dr. Audrey Lugo`s AP Chemistry Course Syllabus
... As this is an extremely fast-paced course, keeping up with work is imperative. Late work will only be accepted with “Mole Bucks.” Six Mole Bucks will be handed out per semester and 1 Mole Buck equals one day late on chapter problems or chapter notes, up to two days late. 2 Mole Bucks equal one day l ...
... As this is an extremely fast-paced course, keeping up with work is imperative. Late work will only be accepted with “Mole Bucks.” Six Mole Bucks will be handed out per semester and 1 Mole Buck equals one day late on chapter problems or chapter notes, up to two days late. 2 Mole Bucks equal one day l ...
EXAMINATION OF THE USE OF AMMONIUM ACETATE AS
... This study is focused on the dissolution kinetics of zinc oxide in ammonium acetate solutions to recover the zinc from alkaline and zinc-carbon spent battery powders. This study represents a first step for further studies in which actual waste powder is to be used. Therefore, the experiments were pe ...
... This study is focused on the dissolution kinetics of zinc oxide in ammonium acetate solutions to recover the zinc from alkaline and zinc-carbon spent battery powders. This study represents a first step for further studies in which actual waste powder is to be used. Therefore, the experiments were pe ...
Practice problems for chapter 1, 2 and 3 1) A small amount of salt
... 11) How many molecules of CH4 are in 48.2 g of this compound? 12) A 30.5 gram sample of glucose (C6H12O6) contains __________ mol of glucose. 13) A sample of CH2F2 with a mass of 19 g contains __________ atoms of F. 14) A sample of CH4O with a mass of 32.0 g contains __________ molecules of CH4O. 15 ...
... 11) How many molecules of CH4 are in 48.2 g of this compound? 12) A 30.5 gram sample of glucose (C6H12O6) contains __________ mol of glucose. 13) A sample of CH2F2 with a mass of 19 g contains __________ atoms of F. 14) A sample of CH4O with a mass of 32.0 g contains __________ molecules of CH4O. 15 ...
AP Chemistry
... (D) 1.0 M CH3COOH (E) 1.0 M NaCl (B) 1.0 M H2SO4 (C) 1.0 M H3PO4 1213. Although structural isomers C3H7OH and C2H5OCH3 exhibit different properties, which of the following would be expected to be the same for both compounds? (A) Heats of fusion (D) Molecular masses (B) Melting points (E) Heats of va ...
... (D) 1.0 M CH3COOH (E) 1.0 M NaCl (B) 1.0 M H2SO4 (C) 1.0 M H3PO4 1213. Although structural isomers C3H7OH and C2H5OCH3 exhibit different properties, which of the following would be expected to be the same for both compounds? (A) Heats of fusion (D) Molecular masses (B) Melting points (E) Heats of va ...
Energy and Chemical Reactions
... and (6) the temperature after the reaction is complete (T2). 32. Given the following for a calorimeter experiment, calculate the molar heat of reaction (∆H°): (1) enough information to get a balanced chemical equation for a reaction including states, (2) ) the amount of reactant in terms of mass or ...
... and (6) the temperature after the reaction is complete (T2). 32. Given the following for a calorimeter experiment, calculate the molar heat of reaction (∆H°): (1) enough information to get a balanced chemical equation for a reaction including states, (2) ) the amount of reactant in terms of mass or ...
Name - cloudfront.net
... If heat is released by a chemical system, an equal amount of heat will be ____. By what quantity must the heat capacity (J/oC) of an object be divided to obtain the specific heat (J/goC) of that material? 64. When energy is changed from one form to another, ____. 65. What happens to the energy produ ...
... If heat is released by a chemical system, an equal amount of heat will be ____. By what quantity must the heat capacity (J/oC) of an object be divided to obtain the specific heat (J/goC) of that material? 64. When energy is changed from one form to another, ____. 65. What happens to the energy produ ...
Chemical Energetics
... • 3. a. The value of H depends on temp , pressure and concentrations of reactants. • b. H are measured under standard conditions : • Temperature = 298K ( 250 C ) • Pressure = 1 atm / 1.01 x 105 Pa • Concentrations = 1 mol dm-3 ...
... • 3. a. The value of H depends on temp , pressure and concentrations of reactants. • b. H are measured under standard conditions : • Temperature = 298K ( 250 C ) • Pressure = 1 atm / 1.01 x 105 Pa • Concentrations = 1 mol dm-3 ...
Chemical Reactions
... Elements – unique substances that cannot be broken down by ordinary chemical means Atoms – more-or-less identical building blocks for each element Atomic symbol – one- or two-letter chemical shorthand for each element ...
... Elements – unique substances that cannot be broken down by ordinary chemical means Atoms – more-or-less identical building blocks for each element Atomic symbol – one- or two-letter chemical shorthand for each element ...
Chemistry: Unit Organizer Name 6-__ Matter has physical properties
... Chemical Reaction: a process in which chemical bonds are broken and atoms rearranged. During the process a new substance is formed. Compound: 2 or more elements combined to make something new, Ex. Na (sodium) + Cl (chlorine) = NaCl (salt) Density:The measurement of how much mass of a substance is co ...
... Chemical Reaction: a process in which chemical bonds are broken and atoms rearranged. During the process a new substance is formed. Compound: 2 or more elements combined to make something new, Ex. Na (sodium) + Cl (chlorine) = NaCl (salt) Density:The measurement of how much mass of a substance is co ...
Practice problems for chapter 1, 3 and 5 1) A small amount of salt
... 11) How many molecules of CH4 are in 48.2 g of this compound? 12) A 30.5 gram sample of glucose (C6H12O6) contains __________ mol of glucose. 13) A sample of CH2F2 with a mass of 19 g contains __________ atoms of F. 14) A sample of CH4O with a mass of 32.0 g contains __________ molecules of CH4O. 15 ...
... 11) How many molecules of CH4 are in 48.2 g of this compound? 12) A 30.5 gram sample of glucose (C6H12O6) contains __________ mol of glucose. 13) A sample of CH2F2 with a mass of 19 g contains __________ atoms of F. 14) A sample of CH4O with a mass of 32.0 g contains __________ molecules of CH4O. 15 ...
11.2 Types of Chemical Reactions
... These equations describe two examples of single-replacement reactions. A single-replacement reaction is a chemical change in which one element replaces a second element in a compound. You can identify a singlereplacement reaction by noting that both the reactants and the products consist of an eleme ...
... These equations describe two examples of single-replacement reactions. A single-replacement reaction is a chemical change in which one element replaces a second element in a compound. You can identify a singlereplacement reaction by noting that both the reactants and the products consist of an eleme ...
Chapter 3 PowerPoint
... look on the table. • To determine the molar mass of a compound, add up the molar masses of the elements that make it up. ...
... look on the table. • To determine the molar mass of a compound, add up the molar masses of the elements that make it up. ...
Complex Ions and Free Energy
... solubility of AgI in pure water and (b) calculate the equilibrium constant for the reaction: ...
... solubility of AgI in pure water and (b) calculate the equilibrium constant for the reaction: ...
Chapter 5 Alt Notes 0910
... Finally, calculate the DHrxn based on the limiting reactant calculation. ...
... Finally, calculate the DHrxn based on the limiting reactant calculation. ...
PHYSICAL SETTING CHEMISTRY
... This is a test of your knowledge of chemistry. Use that knowledge to answer all questions in this examination. Some questions may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry. You are to answer all questions in all parts of this examination according to the dir ...
... This is a test of your knowledge of chemistry. Use that knowledge to answer all questions in this examination. Some questions may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry. You are to answer all questions in all parts of this examination according to the dir ...
AP Chem
... 57. A solution contains equal masses of glucose (mm =180) and toluene (mm=90). What is the mole fraction of glucose in the solution? A. .25 B. .33 C. .5 D. .67 E. .75 58. What is the mass of oxygen in 148 grams of calcium hydroxide? A. 16g B. 24g C. 32g D. 48g E. 64g 59. C3H8 + O2 = CO2 + H2O ...
... 57. A solution contains equal masses of glucose (mm =180) and toluene (mm=90). What is the mole fraction of glucose in the solution? A. .25 B. .33 C. .5 D. .67 E. .75 58. What is the mass of oxygen in 148 grams of calcium hydroxide? A. 16g B. 24g C. 32g D. 48g E. 64g 59. C3H8 + O2 = CO2 + H2O ...
Lesson 1 of 6
... • In any chemical reaction, mass is conserved. – In other words, the mass of the reactant(s) is the same as the mass of the product(s). – The elements on one side of the equation are the same as those on the other. – Matter cannot be created nor destroyed. ...
... • In any chemical reaction, mass is conserved. – In other words, the mass of the reactant(s) is the same as the mass of the product(s). – The elements on one side of the equation are the same as those on the other. – Matter cannot be created nor destroyed. ...
Document
... One cannot weigh a single atom, but it is possible to determine the mass of one atom relative to another experimentally. ...
... One cannot weigh a single atom, but it is possible to determine the mass of one atom relative to another experimentally. ...
The Gibbs Function of a Chemical Reaction*
... Some chemists raise another objection to definition (1) in that the reaction events denoted by the chemical reaction equation are only rarely those actually taking ...
... Some chemists raise another objection to definition (1) in that the reaction events denoted by the chemical reaction equation are only rarely those actually taking ...
Final Exam Practice 2016 (MC)
... d) There are too many electrons in this diagram. The lone pair on carbon should instead be a double bond with one of oxygen’s lone pairs. 23. The molecules CO2 and SO2 have very similar formulas yet make a different shape. What is different about their Lewis structures that give them a different sha ...
... d) There are too many electrons in this diagram. The lone pair on carbon should instead be a double bond with one of oxygen’s lone pairs. 23. The molecules CO2 and SO2 have very similar formulas yet make a different shape. What is different about their Lewis structures that give them a different sha ...
Stoichiometry
Stoichiometry /ˌstɔɪkiˈɒmɨtri/ is the calculation of relative quantities of reactants and products in chemical reactions.Stoichiometry is founded on the law of conservation of mass where the total mass of the reactants equals the total mass of the products leading to the insight that the relations among quantities of reactants and products typically form a ratio of positive integers. This means that if the amounts of the separate reactants are known, then the amount of the product can be calculated. Conversely, if one reactant has a known quantity and the quantity of product can be empirically determined, then the amount of the other reactants can also be calculated.As seen in the image to the right, where the balanced equation is:CH4 + 2 O2 → CO2 + 2 H2O.Here, one molecule of methane reacts with two molecules of oxygen gas to yield one molecule of carbon dioxide and two molecules of water. Stoichiometry measures these quantitative relationships, and is used to determine the amount of products/reactants that are produced/needed in a given reaction. Describing the quantitative relationships among substances as they participate in chemical reactions is known as reaction stoichiometry. In the example above, reaction stoichiometry measures the relationship between the methane and oxygen as they react to form carbon dioxide and water.Because of the well known relationship of moles to atomic weights, the ratios that are arrived at by stoichiometry can be used to determine quantities by weight in a reaction described by a balanced equation. This is called composition stoichiometry.Gas stoichiometry deals with reactions involving gases, where the gases are at a known temperature, pressure, and volume and can be assumed to be ideal gases. For gases, the volume ratio is ideally the same by the ideal gas law, but the mass ratio of a single reaction has to be calculated from the molecular masses of the reactants and products. In practice, due to the existence of isotopes, molar masses are used instead when calculating the mass ratio.