CHEM1411,chapter 1-2-3 exercises 1. In 1828, the diameter of the
... 19. Calculate the percent composition by mass of carbon in Na2CO3. 20. Commonly used gases in the laboratory are generally obtained from pressurized metal gas cylinders, but for small amounts of occasionally used gases, it is sometimes easier just to prepare them chemically as needed. For example, n ...
... 19. Calculate the percent composition by mass of carbon in Na2CO3. 20. Commonly used gases in the laboratory are generally obtained from pressurized metal gas cylinders, but for small amounts of occasionally used gases, it is sometimes easier just to prepare them chemically as needed. For example, n ...
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... B. Which interval on the diagram represents equilibrium between the solid and gas phases? I-II C. Would the solid float or sink in the liquid? Explain. It would sink. The slope of line II-III indicates that the solid is denser than the liquid D. What phase change would occur if at 200̊C the pressure ...
... B. Which interval on the diagram represents equilibrium between the solid and gas phases? I-II C. Would the solid float or sink in the liquid? Explain. It would sink. The slope of line II-III indicates that the solid is denser than the liquid D. What phase change would occur if at 200̊C the pressure ...
Word - Chemistry and More
... b) Calculate the mass of barium nitrate needed to form 3.00 g of barium hydroxide. c) Calculate the percent yield if only 2.70 g of barium hydroxide are formed in (b). d) Determine the mass percentage of each element in barium hydroxide. e) Determine the number of moles of oxygen in 49.7 grams of ba ...
... b) Calculate the mass of barium nitrate needed to form 3.00 g of barium hydroxide. c) Calculate the percent yield if only 2.70 g of barium hydroxide are formed in (b). d) Determine the mass percentage of each element in barium hydroxide. e) Determine the number of moles of oxygen in 49.7 grams of ba ...
Quiz Samples
... See above: mols Zn=0.0015. One mol Zn reacts with 2 mols HCl. mols HCl needed=0.0030. 3MHCl means 3 mols/1L or 0.003 per mL Complete and balance the equation, and calculate mols of gas produced from 0.65 g Zn (atomic weights: Zn=65, H=1, Cl=35.5): Zn + HCl Æ Same as above, but easier Charles’ Law co ...
... See above: mols Zn=0.0015. One mol Zn reacts with 2 mols HCl. mols HCl needed=0.0030. 3MHCl means 3 mols/1L or 0.003 per mL Complete and balance the equation, and calculate mols of gas produced from 0.65 g Zn (atomic weights: Zn=65, H=1, Cl=35.5): Zn + HCl Æ Same as above, but easier Charles’ Law co ...
CHEM1405 2012-J-2 June 2012 • What is the ground state electron
... • The radioactive isotopes 131I and 137Cs have been detected in drinking water near the Japanese Fukushima nuclear reactor. They have half lives of 8 days and 30 years, respectively. What is the definition of half-life? Half-life is the amount of time required for the amount (or activity) of a sampl ...
... • The radioactive isotopes 131I and 137Cs have been detected in drinking water near the Japanese Fukushima nuclear reactor. They have half lives of 8 days and 30 years, respectively. What is the definition of half-life? Half-life is the amount of time required for the amount (or activity) of a sampl ...
Chemical calculations review
... Given the unbalanced equation: ___Ca(OH)2 + ___(NH4)2SO4 → ___CaSO4 + ___NH3 + ___H2O What is the sum of the coefficients when the equation is completely balanced using the smallest whole-number coefficients? ...
... Given the unbalanced equation: ___Ca(OH)2 + ___(NH4)2SO4 → ___CaSO4 + ___NH3 + ___H2O What is the sum of the coefficients when the equation is completely balanced using the smallest whole-number coefficients? ...
Chapter 8 Chemical Equations and Reactions
... Write word and formula equations for the chemical reaction that occurs when solid sodium oxide is added to water at room temperature and forms sodium hydroxide (dissolved in the water). Include symbols for physical states in the formula equation. Then balance the formula equation to give a balanced ...
... Write word and formula equations for the chemical reaction that occurs when solid sodium oxide is added to water at room temperature and forms sodium hydroxide (dissolved in the water). Include symbols for physical states in the formula equation. Then balance the formula equation to give a balanced ...
200 Ways to Pass the Chemistry
... Pb(C2H3O2)2 51. The masses (and energy and charge) of the reactants in a chemical equation is always equal to the masses (and energy and charge) of the products. “Law of Conservation of Mass(and Energy).” 52. The gram formula mass (molar mass) of a substance is the sum of the atomic masses of all th ...
... Pb(C2H3O2)2 51. The masses (and energy and charge) of the reactants in a chemical equation is always equal to the masses (and energy and charge) of the products. “Law of Conservation of Mass(and Energy).” 52. The gram formula mass (molar mass) of a substance is the sum of the atomic masses of all th ...
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... A reaction between an acid and a base yields a salt and water. Such a reaction is a neutralization reaction. Ex: 2KOH + H2SO4 K2SO4 + 2H2O ...
... A reaction between an acid and a base yields a salt and water. Such a reaction is a neutralization reaction. Ex: 2KOH + H2SO4 K2SO4 + 2H2O ...
spring semester review
... d) The reaction is not spontaneous at any temperatures e) We cannot tell from the information given 59. What is the reducing agent in following reaction: Cr2O72- + 6S2O32- + 14H+ --> 2Cr3+ + 3S4O62- + 7H20 a) Cr2O72b) S2O32c) H+ d) Cr3+ e) S4O6260. Which substance is the oxidizing agent in the follo ...
... d) The reaction is not spontaneous at any temperatures e) We cannot tell from the information given 59. What is the reducing agent in following reaction: Cr2O72- + 6S2O32- + 14H+ --> 2Cr3+ + 3S4O62- + 7H20 a) Cr2O72b) S2O32c) H+ d) Cr3+ e) S4O6260. Which substance is the oxidizing agent in the follo ...
Energy of Reactions
... combustion reaction with octane (C8H18) releases a total of -5.55x104 kJ of energy. If the heat of combustion for octane is -250kJ/mole, how many grams of octane did you start with? ...
... combustion reaction with octane (C8H18) releases a total of -5.55x104 kJ of energy. If the heat of combustion for octane is -250kJ/mole, how many grams of octane did you start with? ...
Export To Word
... Standard: Matter A. A working definition of matter is that it takes up space, has mass, and has measurable properties. Matter is comprised of atomic, subatomic, and elementary particles. B. Electrons are key to defining chemical and some physical properties, reactivity, and molecular structures. Rep ...
... Standard: Matter A. A working definition of matter is that it takes up space, has mass, and has measurable properties. Matter is comprised of atomic, subatomic, and elementary particles. B. Electrons are key to defining chemical and some physical properties, reactivity, and molecular structures. Rep ...
Molecular Formulas - Hatboro
... To the AP Chemistry Student: Welcome to my AP Chemistry class! The Advance Placement Chemistry experience is designed to provide a full year of college-level chemistry, so it places heavy demands on the student, especially in terms of the time commitment required. In fact, the College Board suggests ...
... To the AP Chemistry Student: Welcome to my AP Chemistry class! The Advance Placement Chemistry experience is designed to provide a full year of college-level chemistry, so it places heavy demands on the student, especially in terms of the time commitment required. In fact, the College Board suggests ...
Thermodynamics (Part 2)
... What about reactions that are endothermic & nonspontaneous at one temp, but are spont. when temp is raised? ex: ice melting at temps above 0C -there must be another factor besides the loss of energy to predict the direction of spontaneity ...
... What about reactions that are endothermic & nonspontaneous at one temp, but are spont. when temp is raised? ex: ice melting at temps above 0C -there must be another factor besides the loss of energy to predict the direction of spontaneity ...
AP Chemistry Summer Assignment
... 41. How many grams of sodium hydroxide are required to form 51.63 g of lead hydroxide? Pb(NO3)2(aq) + NaOH(aq) ----> Pb(OH)2(s) + NaNO3(aq) (unbalanced) ...
... 41. How many grams of sodium hydroxide are required to form 51.63 g of lead hydroxide? Pb(NO3)2(aq) + NaOH(aq) ----> Pb(OH)2(s) + NaNO3(aq) (unbalanced) ...
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... 0.500 moles of Cu, ________. Cu(s) + 4 HNO3(aq) → Cu(NO3)2(aq) + 2 NO2(g) + 2 H2O() a) you need at least 0.125 moles of HNO3 to produce 0.500 moles of Cu(NO3)2. b) you need at least 0.250 moles of HNO3 to produce 0.500 moles of Cu(NO3)2. c) you need at least 2.00 moles of HNO3 to produce 0.500 mole ...
... 0.500 moles of Cu, ________. Cu(s) + 4 HNO3(aq) → Cu(NO3)2(aq) + 2 NO2(g) + 2 H2O() a) you need at least 0.125 moles of HNO3 to produce 0.500 moles of Cu(NO3)2. b) you need at least 0.250 moles of HNO3 to produce 0.500 moles of Cu(NO3)2. c) you need at least 2.00 moles of HNO3 to produce 0.500 mole ...
AP Thermo I Notes
... First Law of Thermodynamics section 5.2 Energy(E) is neither created nor destroyed. The internal energy of a system is the sum of ...
... First Law of Thermodynamics section 5.2 Energy(E) is neither created nor destroyed. The internal energy of a system is the sum of ...
CHEM 115 EXAM #1 - chem.wilkes.edu
... The term used to describe a substance composed of two or more elements chemically combined in a fixed ratio is: a. solution ...
... The term used to describe a substance composed of two or more elements chemically combined in a fixed ratio is: a. solution ...
Gas-Forming reactions Reactions that form a
... When the fuel is a hydrocarbon, there are two different types of combustion, complete and incomplete. ...
... When the fuel is a hydrocarbon, there are two different types of combustion, complete and incomplete. ...
Calorimetry Key - Iowa State University
... Consider the reverse reaction, namely, the formation of H2 (g) and O2 (g) from H2O (l). a. Is this reaction exothermic or endothermic? (Circle one) 4. Given the following information, circle the term that best completes the statement. Ag2O(s) 2 Ag(s) + ½ O2(g) ΔH° = 31.05 kJ a. Heat is released/ab ...
... Consider the reverse reaction, namely, the formation of H2 (g) and O2 (g) from H2O (l). a. Is this reaction exothermic or endothermic? (Circle one) 4. Given the following information, circle the term that best completes the statement. Ag2O(s) 2 Ag(s) + ½ O2(g) ΔH° = 31.05 kJ a. Heat is released/ab ...
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.