Chemistry 2008–2012 Written examination – November Examination Specifications
... • give simpliÞed answers with an appropriate number of signiÞcant Þgures to all numerical questions; unsimpliÞed answers will not be given full marks. • show all working in your answers to numerical questions. No credit will be given for an incorrect answer unless it is accompanied by details of the ...
... • give simpliÞed answers with an appropriate number of signiÞcant Þgures to all numerical questions; unsimpliÞed answers will not be given full marks. • show all working in your answers to numerical questions. No credit will be given for an incorrect answer unless it is accompanied by details of the ...
AP Chemistry Syllabus - Tuloso
... laboratory reports, summaries of literature or scientific investigations, and oral, written, and graphic presentations. ...
... laboratory reports, summaries of literature or scientific investigations, and oral, written, and graphic presentations. ...
Chapter 5 Review
... Establish an arbitrary scale with the standard enthalpy of formation ( DHf ) as a reference point for all enthalpy expressions. Standard enthalpy of formation ( DHf ) - the heat change that results when one mole of a compound is formed from its elements at a pressure of 1 atm. The standard enthalp ...
... Establish an arbitrary scale with the standard enthalpy of formation ( DHf ) as a reference point for all enthalpy expressions. Standard enthalpy of formation ( DHf ) - the heat change that results when one mole of a compound is formed from its elements at a pressure of 1 atm. The standard enthalp ...
CHAPTER 9
... (2) An exothermic reaction occurs when the energy required to break bonds in reactants is less than the energy released by bond formation in the products. (3) The concentrations of pure liquids and pure solids are never included in an equilibrium constant expression because such concentrations never ...
... (2) An exothermic reaction occurs when the energy required to break bonds in reactants is less than the energy released by bond formation in the products. (3) The concentrations of pure liquids and pure solids are never included in an equilibrium constant expression because such concentrations never ...
Chap 3 - HCC Learning Web
... Since C4H10 contains 4 carbon atoms, so we need four carbon atoms at the right side, which leads us to put 4 (called coefficient) in front of the CO2. Now the equation is updated to be 1 C4H10 + __ O2 4 CO2 + __ H2O As there are 10 hydrogen atoms in C4H10, thus we need to balance the hydrogen atom ...
... Since C4H10 contains 4 carbon atoms, so we need four carbon atoms at the right side, which leads us to put 4 (called coefficient) in front of the CO2. Now the equation is updated to be 1 C4H10 + __ O2 4 CO2 + __ H2O As there are 10 hydrogen atoms in C4H10, thus we need to balance the hydrogen atom ...
Personal Tutoring Help on Questions and Problems
... (c) SO3, (d) C6H6, (e) NaI, (f) K2SO4, (g) Ca3(PO4)2. 3.24 Calculate the molar mass of the following substances: (a) Li2CO3, (b) CS2, (c) CHCl3 (chloroform), * (d) C H 6 8O6 (ascorbic acid, or vitamin C), (e) KNO3, (f) Mg3N2. 3.25 Calculate the molar mass of a compound if 0.372 mole of it has a mass ...
... (c) SO3, (d) C6H6, (e) NaI, (f) K2SO4, (g) Ca3(PO4)2. 3.24 Calculate the molar mass of the following substances: (a) Li2CO3, (b) CS2, (c) CHCl3 (chloroform), * (d) C H 6 8O6 (ascorbic acid, or vitamin C), (e) KNO3, (f) Mg3N2. 3.25 Calculate the molar mass of a compound if 0.372 mole of it has a mass ...
Chemical Formulas and Composition Stoichiometry
... Chemical Formulas and Composition Stoichiometry Chapter 2 ...
... Chemical Formulas and Composition Stoichiometry Chapter 2 ...
PCSD General Chemistry Pacing Guide
... molecules of a substance given the mass or the number of moles and vice versa Use dimensional analysis method to calculate the volume of a gas at standard conditions Determine the percent composition of a given compound Given experimental data, calculate the empirical formula and molecular formula o ...
... molecules of a substance given the mass or the number of moles and vice versa Use dimensional analysis method to calculate the volume of a gas at standard conditions Determine the percent composition of a given compound Given experimental data, calculate the empirical formula and molecular formula o ...
ALE 23. Balancing Redox Reactions
... the substance that is oxidized loses electrons and therefore serves as a reducing agent since it provides electrons to another atom thereby causing that atom to be reduced. The species being reduced serves as the oxidizing agent because it removes electrons from another substance, thereby causing th ...
... the substance that is oxidized loses electrons and therefore serves as a reducing agent since it provides electrons to another atom thereby causing that atom to be reduced. The species being reduced serves as the oxidizing agent because it removes electrons from another substance, thereby causing th ...
Chap. 4 - Chemical Reactions
... 2. Solid calcium reacts with oxygen gas. 3. Solutions of aluminum chloride & sodium carbonate are mixed. 4. Liquid magnesium bromide is decomposed at high temperature. 5. Solid nickel is reacted with aqueous magnesium sulfate. 6. Chlorine gas is reacted with aqueous potassium bromide. 7. Solid magne ...
... 2. Solid calcium reacts with oxygen gas. 3. Solutions of aluminum chloride & sodium carbonate are mixed. 4. Liquid magnesium bromide is decomposed at high temperature. 5. Solid nickel is reacted with aqueous magnesium sulfate. 6. Chlorine gas is reacted with aqueous potassium bromide. 7. Solid magne ...
Aqueous chemistry is a very important component to laboratory
... time, these chemically opposite substances were described in properties such as their taste; their effects on metals, carbonates, and dyes (called indicators); their feel to the touch, and their ability to react with each other. According to the Arrhenius theory, pure water dissociates to some exten ...
... time, these chemically opposite substances were described in properties such as their taste; their effects on metals, carbonates, and dyes (called indicators); their feel to the touch, and their ability to react with each other. According to the Arrhenius theory, pure water dissociates to some exten ...
Masterton and Hurley Chapter 4
... Strong and Weak Acids and Bases • Strong acids ionize completely to H+ • HCl (aq) → H+ (aq) + Cl- (aq) • In a solution of 1.0 M HCl, there is 1M H+ and 1M Cl• No HCl is left un-ionized • Other strong acids ionize in similar fashion ...
... Strong and Weak Acids and Bases • Strong acids ionize completely to H+ • HCl (aq) → H+ (aq) + Cl- (aq) • In a solution of 1.0 M HCl, there is 1M H+ and 1M Cl• No HCl is left un-ionized • Other strong acids ionize in similar fashion ...
Chapter 14
... mol/L, it takes __________ s for the concentration to decrease to 0.11 mol/L. A) 0.017 B) 0.68 C) 9.1 D) 40. E) 5.2 Chapter 15 Chemical Equilibrium 1) At equilibrium, __________. A) all chemical reactions have ceased B) the rates of the forward and reverse reactions are equal C) the rate constants o ...
... mol/L, it takes __________ s for the concentration to decrease to 0.11 mol/L. A) 0.017 B) 0.68 C) 9.1 D) 40. E) 5.2 Chapter 15 Chemical Equilibrium 1) At equilibrium, __________. A) all chemical reactions have ceased B) the rates of the forward and reverse reactions are equal C) the rate constants o ...
9 free IB Chem labs (sent to OCC) - VicPark-IBRoundtable-2009
... magnesium hydroxide. This is then further oxidized by burning to convert all of the Mg to magnesium oxide. Based on the weights of the reactants and the product, the percent composition of the product can be found. Using this information, the empirical formula of the oxide, MgxOy can be ...
... magnesium hydroxide. This is then further oxidized by burning to convert all of the Mg to magnesium oxide. Based on the weights of the reactants and the product, the percent composition of the product can be found. Using this information, the empirical formula of the oxide, MgxOy can be ...
reactions taking place within cells
... • Incomplete combustion due to inadequate supply of O 2 leading to CO or C(indicated by deposit of soot on the bottom of calorimeter) 1st law of thermodynamics Energy can’t be created or destroyed, only converted from one form to another Hess’s law H for a reaction is independent of the route it ta ...
... • Incomplete combustion due to inadequate supply of O 2 leading to CO or C(indicated by deposit of soot on the bottom of calorimeter) 1st law of thermodynamics Energy can’t be created or destroyed, only converted from one form to another Hess’s law H for a reaction is independent of the route it ta ...
Chapter 1 Introduction to Chemistry
... Filtration- technique that uses a porous barrier to separate a solid from a liquid Distillation- technique that is based on differences in the boiling points of substances Crystallization- technique that results in the formation of pure solid particles of a substance from a solution containing the d ...
... Filtration- technique that uses a porous barrier to separate a solid from a liquid Distillation- technique that is based on differences in the boiling points of substances Crystallization- technique that results in the formation of pure solid particles of a substance from a solution containing the d ...
2. The Magic of Chemical Reactions
... IntroductionIn last year we have studied about the reactant, products and chemical reaction. We have also studied about physical and chemicalchanges/poperties of substances. In day today life we observe many chemical changes such as conversion of milk into curd, Ripening of fruits, farmentation of i ...
... IntroductionIn last year we have studied about the reactant, products and chemical reaction. We have also studied about physical and chemicalchanges/poperties of substances. In day today life we observe many chemical changes such as conversion of milk into curd, Ripening of fruits, farmentation of i ...
Unit 8 Note Packet
... 6) Copper metal and aqueous silver nitrate react to form silver metal and aqueous copper (II) nitrate. 7) Gaseous propane (C3H8) will react with oxygen gas when heated to produce carbon dioxide gas and gaseous dihydrogen monoxide. ...
... 6) Copper metal and aqueous silver nitrate react to form silver metal and aqueous copper (II) nitrate. 7) Gaseous propane (C3H8) will react with oxygen gas when heated to produce carbon dioxide gas and gaseous dihydrogen monoxide. ...
Solving General Gas Law Problems
... 3. Use conversions to make units the same as the units of the gas constant R (frequently R=0.0821 L-atm/K-mol is used for the gas constant) Useful Conversions: - Pressure: 1.00 atm = 760 mmHg - Volume: 1 L = 103 mL = 106 µL, etc. - Temperature: K = °C + 273 - Moles: 1 mole = grams of compound (molar ...
... 3. Use conversions to make units the same as the units of the gas constant R (frequently R=0.0821 L-atm/K-mol is used for the gas constant) Useful Conversions: - Pressure: 1.00 atm = 760 mmHg - Volume: 1 L = 103 mL = 106 µL, etc. - Temperature: K = °C + 273 - Moles: 1 mole = grams of compound (molar ...
Document
... 5. Halogens: The oxidation number of fluorine is -1. Each of the other halogens (Cl, Br, I) has an oxidation number of -1 in binary compounds, except when the other element is another halogen above it in the periodic table or the other element is oxygen. 6. Compounds and ions: The sum of the oxidat ...
... 5. Halogens: The oxidation number of fluorine is -1. Each of the other halogens (Cl, Br, I) has an oxidation number of -1 in binary compounds, except when the other element is another halogen above it in the periodic table or the other element is oxygen. 6. Compounds and ions: The sum of the oxidat ...
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.