Dr. Baxley`s Equilibrium Worksheet
... b. If a closed container at 25ºC contained 12.7 g NH4HS and some NH3 gas with a partial pressure of 0.510 atm and H2S gas with a partial pressure of 1.14 atm, will the reaction produce more solid, or will it produce more gases, in order to reach equilibrium? ...
... b. If a closed container at 25ºC contained 12.7 g NH4HS and some NH3 gas with a partial pressure of 0.510 atm and H2S gas with a partial pressure of 1.14 atm, will the reaction produce more solid, or will it produce more gases, in order to reach equilibrium? ...
C2 Knowledge PowerPoint
... Simple molecule – simple covalently bonded structures, e.g. HCl or H2O Giant covalent structure – huge numbers of atoms held together by a network of covalent ...
... Simple molecule – simple covalently bonded structures, e.g. HCl or H2O Giant covalent structure – huge numbers of atoms held together by a network of covalent ...
Document
... Simple molecule – simple covalently bonded structures, e.g. HCl or H2O Giant covalent structure – huge numbers of atoms held together by a network of covalent ...
... Simple molecule – simple covalently bonded structures, e.g. HCl or H2O Giant covalent structure – huge numbers of atoms held together by a network of covalent ...
FirstSemesterReviewHonors
... 1. Be able to write word equations for chemical reactions. Example: When baking soda (sodium bicarbonate) is heated, it decomposes, forming the products sodium carbonate, carbon dioxide, and water. 2. Know how to balance chemical equations: a. P + O2 -> P4O10 b. Fe2O3 +H2 -> Fe +H2O 3. Know how to ...
... 1. Be able to write word equations for chemical reactions. Example: When baking soda (sodium bicarbonate) is heated, it decomposes, forming the products sodium carbonate, carbon dioxide, and water. 2. Know how to balance chemical equations: a. P + O2 -> P4O10 b. Fe2O3 +H2 -> Fe +H2O 3. Know how to ...
Average Atomic Mass
... Chemical Composition Moles Avogadro’s Number Molar Mass Percent Composition Empirical Formula Molecular Formula 62. Calculate the molar mass of magnesium phosphate. 63. How many moles are in 7.23 grams of strontium oxide? 64. How many moles are in 3.02 x 1023 atoms of zinc? 65. How many grams are i ...
... Chemical Composition Moles Avogadro’s Number Molar Mass Percent Composition Empirical Formula Molecular Formula 62. Calculate the molar mass of magnesium phosphate. 63. How many moles are in 7.23 grams of strontium oxide? 64. How many moles are in 3.02 x 1023 atoms of zinc? 65. How many grams are i ...
Reaction Rate review questions
... ii) What is the value of ∆H for the forward reaction? ∆H = +30 the reverse reaction? ∆H = -30 iii) What is the energy of the activated complex? 120kJ 31. Which of the five factors that affect the rate of a reaction is illustrated in each of the following: a) Food is sometimes frozen before it is use ...
... ii) What is the value of ∆H for the forward reaction? ∆H = +30 the reverse reaction? ∆H = -30 iii) What is the energy of the activated complex? 120kJ 31. Which of the five factors that affect the rate of a reaction is illustrated in each of the following: a) Food is sometimes frozen before it is use ...
Slide 1
... •Property of matter that describes a substances ability to participate in chemical reactions. (Change into new matter.) –Flammability •ability to burn •Burning wood creates ash and smoke ...
... •Property of matter that describes a substances ability to participate in chemical reactions. (Change into new matter.) –Flammability •ability to burn •Burning wood creates ash and smoke ...
HERE
... 15) Which property is an example of a chemical property? A) the ability to burn B) the ability to melt C) the ability to dissolve D) the ability to evaporate 16) During a physical science lab investigating chemical reactions, several students placed an antacid tablet in a zip-lock bag. They recorded ...
... 15) Which property is an example of a chemical property? A) the ability to burn B) the ability to melt C) the ability to dissolve D) the ability to evaporate 16) During a physical science lab investigating chemical reactions, several students placed an antacid tablet in a zip-lock bag. They recorded ...
s - chem116
... each atom comprises. Use the total mass of each type of atom determined before, then divide by the formula weight. ...
... each atom comprises. Use the total mass of each type of atom determined before, then divide by the formula weight. ...
Chapter 2 Matter and Change
... • Distillation - a liquid is boiled to produce a vapor which is condensed into a liquid Other ways? distillation • How to perform simple distillation in the chemistry lab | Wonder How To ...
... • Distillation - a liquid is boiled to produce a vapor which is condensed into a liquid Other ways? distillation • How to perform simple distillation in the chemistry lab | Wonder How To ...
Unit Description - Honors Chemistry
... Define physical change and list several common physical changes. Define chemical change and list several indications that a chemical change has taken place. Apply the law of conservation of mass to chemical reactions. Contrast mixtures and substances. Classify mixtures as homogeneous or he ...
... Define physical change and list several common physical changes. Define chemical change and list several indications that a chemical change has taken place. Apply the law of conservation of mass to chemical reactions. Contrast mixtures and substances. Classify mixtures as homogeneous or he ...
Document
... • Five important types of redox reactions • combustion: burning in air. The products of complete combustion of carbon compounds are CO2 and H2O. • respiration: the process by which living organisms use O2 to oxidize carbon-containing compounds to produce CO2 and H2O. The importance of these reaction ...
... • Five important types of redox reactions • combustion: burning in air. The products of complete combustion of carbon compounds are CO2 and H2O. • respiration: the process by which living organisms use O2 to oxidize carbon-containing compounds to produce CO2 and H2O. The importance of these reaction ...
200 Things to Know to Pass the Chemistry Regents
... 19. Elements are pure substances composed of atoms with the same atomic number. They cannot be decomposed. A compound differs from an element in that a compound Has a homogeneous composition has one set of properties Has a heterogeneous composition can be decomposed 20. Binary compounds are substanc ...
... 19. Elements are pure substances composed of atoms with the same atomic number. They cannot be decomposed. A compound differs from an element in that a compound Has a homogeneous composition has one set of properties Has a heterogeneous composition can be decomposed 20. Binary compounds are substanc ...
200 Ways to Pass the Chemistry
... 19. Elements are pure substances composed of atoms with the same atomic number. They cannot be decomposed. A compound differs from an element in that a compound Has a homogeneous composition has one set of properties Has a heterogeneous composition can be decomposed 20. Binary compounds are substanc ...
... 19. Elements are pure substances composed of atoms with the same atomic number. They cannot be decomposed. A compound differs from an element in that a compound Has a homogeneous composition has one set of properties Has a heterogeneous composition can be decomposed 20. Binary compounds are substanc ...
200things2know
... 19. Elements are pure substances composed of atoms with the same atomic number. They cannot be decomposed. A compound differs from an element in that a compound Has a homogeneous composition has one set of properties Has a heterogeneous composition can be decomposed 20. Binary compounds are substanc ...
... 19. Elements are pure substances composed of atoms with the same atomic number. They cannot be decomposed. A compound differs from an element in that a compound Has a homogeneous composition has one set of properties Has a heterogeneous composition can be decomposed 20. Binary compounds are substanc ...
LECTURE PPT: Chapter 8
... 1. LO: Recognize the numerical relationship between chemical quantities in a balanced chemical equation. 2. LO: Carry out mole-to-mole conversions between reactants and products based on the numerical relationship between chemical quantities in a balanced chemical equation. 3. LO: Carry out mass-to- ...
... 1. LO: Recognize the numerical relationship between chemical quantities in a balanced chemical equation. 2. LO: Carry out mole-to-mole conversions between reactants and products based on the numerical relationship between chemical quantities in a balanced chemical equation. 3. LO: Carry out mass-to- ...
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 © 2009, Prentice-Hall, 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 © 2009, Prentice-Hall, Inc. ...
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 © 2009, Prentice-Hall, 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 © 2009, Prentice-Hall, Inc. ...
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.