Stoichiometry
... • It is impossible to weigh a single atom, but one can easily establish the weight of an atom relative to another • We must establish a standard: – An atom of carbon-12 (six protons, six neutrons, six electrons) has a mass of exactly 12 atomic mass units (u) – Therefore, 1 atomic mass unit (u) is eq ...
... • It is impossible to weigh a single atom, but one can easily establish the weight of an atom relative to another • We must establish a standard: – An atom of carbon-12 (six protons, six neutrons, six electrons) has a mass of exactly 12 atomic mass units (u) – Therefore, 1 atomic mass unit (u) is eq ...
2015 Academic Challenge CHEMISTRY TEST – STATE
... You are advised to use your time effectively and to work as rapidly as you can without losing accuracy. Do not waste your time on questions that seem too difficult for you. Go on to the other questions, and then come back to the difficult ones later if time remains. ...
... You are advised to use your time effectively and to work as rapidly as you can without losing accuracy. Do not waste your time on questions that seem too difficult for you. Go on to the other questions, and then come back to the difficult ones later if time remains. ...
Chemical Reactions: Introduction to Reaction Types
... elements, b) 1 element and 1 binary compound (consisting of 2 elements), or c) 2 binary compounds. The following are examples of combination reactions: The rusting of iron: 4Fe (s) + 3O2 (g) → 2Fe2O3 (s) The formation of one kind of acid rain: SO3 (g) + H2O (l) → H2SO4 (aq) 2. Decomposition: AB → A ...
... elements, b) 1 element and 1 binary compound (consisting of 2 elements), or c) 2 binary compounds. The following are examples of combination reactions: The rusting of iron: 4Fe (s) + 3O2 (g) → 2Fe2O3 (s) The formation of one kind of acid rain: SO3 (g) + H2O (l) → H2SO4 (aq) 2. Decomposition: AB → A ...
chemistry form iii - Covington Latin School
... Significant figures Units of measurement Elements and Compounds The elements and their composition Compounds and their composition Matter and Energy The properties of matter The properties of energy Periodic Table and Chemical Nomenclature Relationships among the elements and the periodic table The ...
... Significant figures Units of measurement Elements and Compounds The elements and their composition Compounds and their composition Matter and Energy The properties of matter The properties of energy Periodic Table and Chemical Nomenclature Relationships among the elements and the periodic table The ...
Tutorial 7
... Example 2:Electrogravimetry Ions that react with Ag+ can be determined electro-gravimetrically by deposition on a silver working anode: Ag(s) + X AgX(s) + eWhat will be the final mass of a silver anode used to electrolyze 75.00 mL of 0.0238 M KSCN if the initial mass of the anode is 12.463 g. ...
... Example 2:Electrogravimetry Ions that react with Ag+ can be determined electro-gravimetrically by deposition on a silver working anode: Ag(s) + X AgX(s) + eWhat will be the final mass of a silver anode used to electrolyze 75.00 mL of 0.0238 M KSCN if the initial mass of the anode is 12.463 g. ...
AP Chemistry Summer 2009
... write your final answer on the line provided on this sheet with sig figs and units. Staple your work to the back of this packet. 1. Stoichiometry refers to _____________________________________. _____________2. Given the following reaction: GeH4 + 3GeF4 4 GeF3H this reaction, how many moles of GeF ...
... write your final answer on the line provided on this sheet with sig figs and units. Staple your work to the back of this packet. 1. Stoichiometry refers to _____________________________________. _____________2. Given the following reaction: GeH4 + 3GeF4 4 GeF3H this reaction, how many moles of GeF ...
Definitions - Loreto Science
... • are particular types of dipole-dipole attractions between molecules in which hydrogen atoms are bonded to nitrogen, oxygen or fluorine. • The hydrogen atom carries a partial positive charge and is attracted to the electronegative atom in another molecule. Thus, H acts as a bridge between two elect ...
... • are particular types of dipole-dipole attractions between molecules in which hydrogen atoms are bonded to nitrogen, oxygen or fluorine. • The hydrogen atom carries a partial positive charge and is attracted to the electronegative atom in another molecule. Thus, H acts as a bridge between two elect ...
HONORS CHEMISTRY
... A solution containig 20.0 grams of sodium sulfite reacts with 7.00 cm3 of phophoric acid (d=1.83 g/cm3). Determine the following: a. the excess reactant and its mass. b. grams of water produced. c. moles of sodium phosphate produced. d. grams of sulfur dioxide produced. e. cubic decimeters of sulfur ...
... A solution containig 20.0 grams of sodium sulfite reacts with 7.00 cm3 of phophoric acid (d=1.83 g/cm3). Determine the following: a. the excess reactant and its mass. b. grams of water produced. c. moles of sodium phosphate produced. d. grams of sulfur dioxide produced. e. cubic decimeters of sulfur ...
Unit 2
... a) which elements are metals? _____________________________________ b) which elements are nonmetals? ___________________________________ c) which elements are metalloids? ___________________________________ 25) A compound has two boron atoms and six hydrogen atoms. a) what is its empirical formula? ...
... a) which elements are metals? _____________________________________ b) which elements are nonmetals? ___________________________________ c) which elements are metalloids? ___________________________________ 25) A compound has two boron atoms and six hydrogen atoms. a) what is its empirical formula? ...
Unit 2
... a) which elements are metals? _____________________________________ b) which elements are nonmetals? ___________________________________ c) which elements are metalloids? ___________________________________ 25) A compound has two boron atoms and six hydrogen atoms. a) what is its empirical formula? ...
... a) which elements are metals? _____________________________________ b) which elements are nonmetals? ___________________________________ c) which elements are metalloids? ___________________________________ 25) A compound has two boron atoms and six hydrogen atoms. a) what is its empirical formula? ...
AP Semestar Exam REVIEW
... ____ 22. Which of the following are strong bases: NH3, NaOH, Ba(OH)2, and HF? a. NH3 and HF b. NaOH and Ba(OH)2 c. NH3 and NaOH d. NaOH, Ba(OH)2, and HF e. NH3, NaOH, Ba(OH)2, and HF ____ 23. What is the net ionic equation for the reaction of lithium hydroxide with hydroiodic acid? a. H+ + I- HCl( ...
... ____ 22. Which of the following are strong bases: NH3, NaOH, Ba(OH)2, and HF? a. NH3 and HF b. NaOH and Ba(OH)2 c. NH3 and NaOH d. NaOH, Ba(OH)2, and HF e. NH3, NaOH, Ba(OH)2, and HF ____ 23. What is the net ionic equation for the reaction of lithium hydroxide with hydroiodic acid? a. H+ + I- HCl( ...
Honors Chemistry Semester 1 Exam Review
... 12. Which statement describes characteristics of an endothermic reaction? __The sign of H is positive, and the products have less potential energy than the reactants. __The sign of H is positive, and the products have more potential energy than the reactants. __The sign of H is negative, and the pro ...
... 12. Which statement describes characteristics of an endothermic reaction? __The sign of H is positive, and the products have less potential energy than the reactants. __The sign of H is positive, and the products have more potential energy than the reactants. __The sign of H is negative, and the pro ...
Just a Few Things 2012
... Homogeneous mixtures are called solutions. example: NaCl (aq), air Solid solutions are often between metals alloys Liquid solutions are transparent. ...
... Homogeneous mixtures are called solutions. example: NaCl (aq), air Solid solutions are often between metals alloys Liquid solutions are transparent. ...
mole
... hydrogen carbonate are reacted together. The products formed are aqueous sodium chloride, water, and carbon dioxide gas. Write a skeleton equation for this reaction. • Solid sodium hydrogen carbonate: NaHCO3(s) • Hydrochloric acid: HCl(aq) • Water: H2O(l) • Carbon dioxide gas: CO2(g) ...
... hydrogen carbonate are reacted together. The products formed are aqueous sodium chloride, water, and carbon dioxide gas. Write a skeleton equation for this reaction. • Solid sodium hydrogen carbonate: NaHCO3(s) • Hydrochloric acid: HCl(aq) • Water: H2O(l) • Carbon dioxide gas: CO2(g) ...
AP Chemistry Unit 3 Test Review Topics Covered: Gases Liquids
... 1) The density of an unknown gas is 4.20 grams per liter at 3.00 atmospheres pressure and 127 °C. What is the molecular weight of this gas? (R = 0.0821 liter-atm / mole-K) (A) 14.6 (B) 46.0 (C) 88.0 (D) 94.1 (E) 138 2) Two flexible containers for Gas are at the same temperature and pressure. One hol ...
... 1) The density of an unknown gas is 4.20 grams per liter at 3.00 atmospheres pressure and 127 °C. What is the molecular weight of this gas? (R = 0.0821 liter-atm / mole-K) (A) 14.6 (B) 46.0 (C) 88.0 (D) 94.1 (E) 138 2) Two flexible containers for Gas are at the same temperature and pressure. One hol ...
The Mole
... Saying that the atomic mass of magnesium is 24 means that its atoms are twice as heavy as those of some other element (carbon) with an atomic mass of 12. It is possible, however, to assign units to atomic, molecular, and formula masses. When the unit gram is used with an atomic mass, we define the g ...
... Saying that the atomic mass of magnesium is 24 means that its atoms are twice as heavy as those of some other element (carbon) with an atomic mass of 12. It is possible, however, to assign units to atomic, molecular, and formula masses. When the unit gram is used with an atomic mass, we define the g ...
Unit 7 Homework and Lab Packet
... 3. Add 50.0 ml of distilled water to the beaker. Swirl the beaker around to dissolve all of the copper(II)sulfate crystals. 4. Obtain two clean, dry iron nails from your teacher. If the nails are not clean, use a piece of sand paper or steel wool to make the surface of the nail shiny. Find the mass ...
... 3. Add 50.0 ml of distilled water to the beaker. Swirl the beaker around to dissolve all of the copper(II)sulfate crystals. 4. Obtain two clean, dry iron nails from your teacher. If the nails are not clean, use a piece of sand paper or steel wool to make the surface of the nail shiny. Find the mass ...
PPT - gserianne.com
... • atoms with the same atomic numbers but with different atomic weights • atoms with the same number of protons and electrons but a different number of neutrons • oxygen (atomic number 8) has the following isotopes (16O, 17O, 18O) • unstable isotopes (radioisotopes or radionuclides) are radioactive; ...
... • atoms with the same atomic numbers but with different atomic weights • atoms with the same number of protons and electrons but a different number of neutrons • oxygen (atomic number 8) has the following isotopes (16O, 17O, 18O) • unstable isotopes (radioisotopes or radionuclides) are radioactive; ...
Stoichiometry/Mass/Mole Relationships
... 10. ___ C6H12 + ___ O2 → ___ CO2 + ___ H2O 42 grams of cyclohexane burns in excess air to from carbon dioxide and water. How many grams of carbon dioxide and of water vapor are produced? ...
... 10. ___ C6H12 + ___ O2 → ___ CO2 + ___ H2O 42 grams of cyclohexane burns in excess air to from carbon dioxide and water. How many grams of carbon dioxide and of water vapor are produced? ...
File
... 10. Which of the following is true concerning the impact of increasing temperature on reaction rates? a. The number of collisions between reactant atoms is increased. b. The energy of each reactant atom is increased. c. The percentage of collisions with sufficient energy to cross the activation ener ...
... 10. Which of the following is true concerning the impact of increasing temperature on reaction rates? a. The number of collisions between reactant atoms is increased. b. The energy of each reactant atom is increased. c. The percentage of collisions with sufficient energy to cross the activation ener ...
AP Chem Chapter 16 Review Packet
... is no hope of causing the reaction to occur without coupling it to another process. For example, it has been proposed that the reaction can be promoted by first reacting silver with water to produce hydrogen and silver oxide. 2 Ag (s) + H2O (g) Ag2O (s) + H2 (g) and then decomposing the silver oxi ...
... is no hope of causing the reaction to occur without coupling it to another process. For example, it has been proposed that the reaction can be promoted by first reacting silver with water to produce hydrogen and silver oxide. 2 Ag (s) + H2O (g) Ag2O (s) + H2 (g) and then decomposing the silver oxi ...
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.