Slide 1
... – To accomplish this task we must first determine the relative amount of reactants and products to burn the propane. This requires setting up the chemical reaction. – The next step is to determine the relative mass of each based on the ratios determined from the chemical reaction. – Then express eve ...
... – To accomplish this task we must first determine the relative amount of reactants and products to burn the propane. This requires setting up the chemical reaction. – The next step is to determine the relative mass of each based on the ratios determined from the chemical reaction. – Then express eve ...
Chemical equilibrium, redox and pE
... ∆U = qv qv= heat at constant volume • System at constant pressure (all reactions open to atmosphere) ∆U = qp - P∆V Ideal gas law P∆V = ∆nRT R is the gas constant = 8.314 Joules mol-1 K-1 therefore ∆U = qp - ∆nRT rearranging qp = ∆U + ∆nRT ...
... ∆U = qv qv= heat at constant volume • System at constant pressure (all reactions open to atmosphere) ∆U = qp - P∆V Ideal gas law P∆V = ∆nRT R is the gas constant = 8.314 Joules mol-1 K-1 therefore ∆U = qp - ∆nRT rearranging qp = ∆U + ∆nRT ...
Earth Science - Green Local Schools
... Average atomic mass energy levels Metal Valence electron Nonmetal Period Semiconductor Group Alkali metal Ion Alkaline-earth metal Atomic number Transition metal Mass number Noble gases Electron Cloud Model / Bohr Model Be able to find the number of neutrons, protons, and electrons in an atom Be ...
... Average atomic mass energy levels Metal Valence electron Nonmetal Period Semiconductor Group Alkali metal Ion Alkaline-earth metal Atomic number Transition metal Mass number Noble gases Electron Cloud Model / Bohr Model Be able to find the number of neutrons, protons, and electrons in an atom Be ...
Fall 2008 Blank Exam 1 - Department of Chemistry | Oregon State
... This exam consists of 25 multiple-choice questions. Each question has four points associated with it. Select the best multiple-choice answer by filling in the corresponding circle on the rear page of the answer sheet. If you have any questions before the exam, please ask. If you have any questions d ...
... This exam consists of 25 multiple-choice questions. Each question has four points associated with it. Select the best multiple-choice answer by filling in the corresponding circle on the rear page of the answer sheet. If you have any questions before the exam, please ask. If you have any questions d ...
Ch 02.01-03: Atoms Molecules Ions
... source or how they were prepared, have the same proportions of their constituent elements. ...
... source or how they were prepared, have the same proportions of their constituent elements. ...
Safety - Wando High School
... 2. Covalent compound is called? 3. Ionic compound is called? 4. What do coefficients represent? 5. Write out the equation for the sentence below. a. Two atoms of aluminum react with three units of aqueous copper(II) chloride to produce three atoms of copper and two units of aqueous aluminum chloride ...
... 2. Covalent compound is called? 3. Ionic compound is called? 4. What do coefficients represent? 5. Write out the equation for the sentence below. a. Two atoms of aluminum react with three units of aqueous copper(II) chloride to produce three atoms of copper and two units of aqueous aluminum chloride ...
AP Chemistry
... (NH4)2CO3(s) Δ → H2O(g) + CO2(g) + 2NH3(g) CaCO3(s) Δ → CaO(s) + CO2(g) NaHCO3(s) Δ → Na2CO3(s) + H2O(g) + CO2(g) C) Single Displacement (Redox) An element reacts with a compound totake the place of one of the elements of that compound. A new element is formed along with a new compound. a) Metal and ...
... (NH4)2CO3(s) Δ → H2O(g) + CO2(g) + 2NH3(g) CaCO3(s) Δ → CaO(s) + CO2(g) NaHCO3(s) Δ → Na2CO3(s) + H2O(g) + CO2(g) C) Single Displacement (Redox) An element reacts with a compound totake the place of one of the elements of that compound. A new element is formed along with a new compound. a) Metal and ...
Document
... chemical reaction. There are three types: 1. Actual yield- what you get in the lab when the chemicals are mixed 2. Theoretical yield- what the balanced equation tells should be made ...
... chemical reaction. There are three types: 1. Actual yield- what you get in the lab when the chemicals are mixed 2. Theoretical yield- what the balanced equation tells should be made ...
Stoichiometry: Calculations with Chemical Formulas and Equations
... of 1 mol of a substance (i.e., g/mol). – The molar mass of an element is the mass number for the element that we find on the periodic table. – The formula weight (in amu’s) will be the same number as the molar mass (in g/mol). Stoichiometry © 2012 Pearson Education, Inc. ...
... of 1 mol of a substance (i.e., g/mol). – The molar mass of an element is the mass number for the element that we find on the periodic table. – The formula weight (in amu’s) will be the same number as the molar mass (in g/mol). Stoichiometry © 2012 Pearson Education, Inc. ...
Document
... If the compound is soluble that means that it will remain as ions in the solution, if it is insoluble then the compound precipitated out of the reaction (it became the precipitate or solid). 2. If at least one INSOLUBLE product is formed (which means a precipitate will form) the reaction will occur! ...
... If the compound is soluble that means that it will remain as ions in the solution, if it is insoluble then the compound precipitated out of the reaction (it became the precipitate or solid). 2. If at least one INSOLUBLE product is formed (which means a precipitate will form) the reaction will occur! ...
How many significant figures are there in each of these
... calculated density, we must improve the poorest measurement. We must use a more precise device to measure the VOLUME (which only has two significant figures in this example)! ...
... calculated density, we must improve the poorest measurement. We must use a more precise device to measure the VOLUME (which only has two significant figures in this example)! ...
STOICHIOMETRY (I) Molecular Mass: The sum of the masses of the
... An amount of substance that contains as many elementary entities as there are atoms in exactly 12 g of C-12. Avogadro’s number is the actual number of entities in 1 mole of substance: 6.022137 x 1023 per mole. (IV) Molar Mass: The mass of 1 mole of a particular substance. Is numerically equivalent t ...
... An amount of substance that contains as many elementary entities as there are atoms in exactly 12 g of C-12. Avogadro’s number is the actual number of entities in 1 mole of substance: 6.022137 x 1023 per mole. (IV) Molar Mass: The mass of 1 mole of a particular substance. Is numerically equivalent t ...
Final Exam Review Day 1
... The Noble gases are stable because they have ___ ______________ ____________. Elements are placed in order of increasing ______________ _______________ and placed in groups according to their ___________________ __________________. Rows = ______________ =___________ __________ _______ Columns =_____ ...
... The Noble gases are stable because they have ___ ______________ ____________. Elements are placed in order of increasing ______________ _______________ and placed in groups according to their ___________________ __________________. Rows = ______________ =___________ __________ _______ Columns =_____ ...
Chemistry A - Montgomery County Public Schools
... use solubility rules to predict if a precipitate will form in a double displacement reaction. use coefficients to balance simple chemical equations. apply the Law of Conservation of Mass to account for the same number of atoms of each type appearing in both the reactants and products. identi ...
... use solubility rules to predict if a precipitate will form in a double displacement reaction. use coefficients to balance simple chemical equations. apply the Law of Conservation of Mass to account for the same number of atoms of each type appearing in both the reactants and products. identi ...
Second Semester Final Review Guide
... 9. What happens to the solubility of a solid solute in a liquid solvent if the temperature of the solvent is increased? 10. What happens to the solubility of a gas solute in a liquid solvent if the temperature of the solvent is increased? 11. What happens to the boiling point of a solution as the co ...
... 9. What happens to the solubility of a solid solute in a liquid solvent if the temperature of the solvent is increased? 10. What happens to the solubility of a gas solute in a liquid solvent if the temperature of the solvent is increased? 11. What happens to the boiling point of a solution as the co ...
Per 5 - Old Saybrook Public Schools
... 31. A certain compound is 7.7% hydrogen and 92.3% carbon by mass. If the compound’s molecular mass is 78, find its molecular formula. ...
... 31. A certain compound is 7.7% hydrogen and 92.3% carbon by mass. If the compound’s molecular mass is 78, find its molecular formula. ...
STUDY GUIDE for DIGESTION and NUTRITION
... Explain what indicators are used for and how they help determine if a substance is acidic or basic. Explain the significance of the pH scale. Find the names and formulas of common acids in your data booklet (e.g. HCl, H2SO4,) Chemical Reactions Describe the difference between a physical and ...
... Explain what indicators are used for and how they help determine if a substance is acidic or basic. Explain the significance of the pH scale. Find the names and formulas of common acids in your data booklet (e.g. HCl, H2SO4,) Chemical Reactions Describe the difference between a physical and ...
ch8 - Otterville R-VI School District
... BaCl2(aq) + Na2SO4(aq) NaCl(aq) + BaSO4(s) iron sulfide and hydrochloric acid FeS(aq) + HCl(aq) FeCl2(aq) + H2S(g) hydrochloric acid and sodium hydroxide HCl(aq) + NaOH NaCl(aq) + H2O(l) potassium iodide and lead (II) nitrate KI(aq) + Pb(NO3)2 KNO3(aq) + PbI2(s) ...
... BaCl2(aq) + Na2SO4(aq) NaCl(aq) + BaSO4(s) iron sulfide and hydrochloric acid FeS(aq) + HCl(aq) FeCl2(aq) + H2S(g) hydrochloric acid and sodium hydroxide HCl(aq) + NaOH NaCl(aq) + H2O(l) potassium iodide and lead (II) nitrate KI(aq) + Pb(NO3)2 KNO3(aq) + PbI2(s) ...
File
... Suppose that in one batch of reactants 4.20mol Al was mixed with 1.75mol Fe2O3. Which reactant, if any, was the limiting reactant? Calculate the mass of iron (in grams) that can be formed from this mixture of reactants. How do we approach this question – firstly determine what has been asked of you. ...
... Suppose that in one batch of reactants 4.20mol Al was mixed with 1.75mol Fe2O3. Which reactant, if any, was the limiting reactant? Calculate the mass of iron (in grams) that can be formed from this mixture of reactants. How do we approach this question – firstly determine what has been asked of you. ...
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.