(General Equilibrium) Part 1
... -The value for the concentrations of solids and liquids are incorporated into the value of Kc. C. Units for Kc – Kc is expressed without units. This is because formally, the value that is put into the Kc expression is not the molar concentration, but the ratio of the concentration to a reference con ...
... -The value for the concentrations of solids and liquids are incorporated into the value of Kc. C. Units for Kc – Kc is expressed without units. This is because formally, the value that is put into the Kc expression is not the molar concentration, but the ratio of the concentration to a reference con ...
word-doc Practice for the final exam!
... d. pure substance e. solid 3. If matter is uniform throughout, cannot be separated into other substances by physical processes, but can be decomposed into other substances by chemical processes, it is ________. a. a heterogeneous mixture b. an element c. a homogeneous mixture d. a compound e. a mixt ...
... d. pure substance e. solid 3. If matter is uniform throughout, cannot be separated into other substances by physical processes, but can be decomposed into other substances by chemical processes, it is ________. a. a heterogeneous mixture b. an element c. a homogeneous mixture d. a compound e. a mixt ...
Notes: Kinetics and Equilibrium
... this terrible accident. Condition number one requires that the train must collide with the bus. Condition number two requires that the train and bus collide with enough energy for the reaction to occur, meaning the train must hit the bus with enough energy, not merely tap the bus. The third conditio ...
... this terrible accident. Condition number one requires that the train must collide with the bus. Condition number two requires that the train and bus collide with enough energy for the reaction to occur, meaning the train must hit the bus with enough energy, not merely tap the bus. The third conditio ...
Utah - Wavefunction, Inc.
... matter how they are rearranged; the total mass stays the same. Although energy can be absorbed or released in a chemical reaction, the total amount of energy and matter in it remains constant. Many reactions attain a state of equilibrium. Many ordinary activities, such as baking, involve chemical re ...
... matter how they are rearranged; the total mass stays the same. Although energy can be absorbed or released in a chemical reaction, the total amount of energy and matter in it remains constant. Many reactions attain a state of equilibrium. Many ordinary activities, such as baking, involve chemical re ...
Here
... We must learn to balance these equations, and there are some simple guidelines… • These equations must have the same number and type of symbols on each side of the equation (we cannot destroy the elements involved or mass!!) • If we want to change the number of symbols on either side, we must put la ...
... We must learn to balance these equations, and there are some simple guidelines… • These equations must have the same number and type of symbols on each side of the equation (we cannot destroy the elements involved or mass!!) • If we want to change the number of symbols on either side, we must put la ...
Module 3 -- Lesson 4
... If a reactant or a product is added to a system at equilibrium, the system will shift away from the added component. If a reactant or product is removed, the system will shift toward the removed component. Returning to the Haber process as an example, if the pressure is increased, more product is fo ...
... If a reactant or a product is added to a system at equilibrium, the system will shift away from the added component. If a reactant or product is removed, the system will shift toward the removed component. Returning to the Haber process as an example, if the pressure is increased, more product is fo ...
Key concepts of chemistry from high school chemistry
... thought to be the least divisible form of matter, is comprised of three key subatomic particles. According to modern atomic theory, an atom contains protons and neutrons within a compa ...
... thought to be the least divisible form of matter, is comprised of three key subatomic particles. According to modern atomic theory, an atom contains protons and neutrons within a compa ...
Chapter 4_part 1
... *Greater atomic number => higher priority If two groups are the same consider the next atom and so on … ...
... *Greater atomic number => higher priority If two groups are the same consider the next atom and so on … ...
Chemistry Fall Final Study Guide Concepts
... C3H8+ 5O2 → 3 CO2 + 4H2O 23. 10. How many moles of O2, oxygen, will produce 2.5 moles of H2O, water? 2.5 moles H2O x 5 moles O2 = 3.1 moles O2 4 moles H2O 24. How many grams of O2, oxygen, will be needed to react 1.50 moles of C3H8, propane? 1.50 moles C3H8 x 5 moles O2 x 32g O2 = 240.g O2 1mole C3H ...
... C3H8+ 5O2 → 3 CO2 + 4H2O 23. 10. How many moles of O2, oxygen, will produce 2.5 moles of H2O, water? 2.5 moles H2O x 5 moles O2 = 3.1 moles O2 4 moles H2O 24. How many grams of O2, oxygen, will be needed to react 1.50 moles of C3H8, propane? 1.50 moles C3H8 x 5 moles O2 x 32g O2 = 240.g O2 1mole C3H ...
Document
... Silicon carbide (SiC) is made from sand (silicon dioxide, SiO2) and carbon at high T. CO is also formed. If 100.0 kg of sand are reacted and 55.0 kg SiC are formed, what is the percent yield? SiO2(s) + 3 C(s) → SiC(s) + 2 CO(g) Convert kg SiO2 to moles: ...
... Silicon carbide (SiC) is made from sand (silicon dioxide, SiO2) and carbon at high T. CO is also formed. If 100.0 kg of sand are reacted and 55.0 kg SiC are formed, what is the percent yield? SiO2(s) + 3 C(s) → SiC(s) + 2 CO(g) Convert kg SiO2 to moles: ...
Stoichiometry of Chemical Reactions
... balancing a chemical equation. Consider as an example the reaction between one methane molecule (CH4) and two diatomic oxygen molecules (O2) to produce one carbon dioxide molecule (CO2) and two water molecules (H2O). The chemical equation representing this process is provided in the upper half of Fi ...
... balancing a chemical equation. Consider as an example the reaction between one methane molecule (CH4) and two diatomic oxygen molecules (O2) to produce one carbon dioxide molecule (CO2) and two water molecules (H2O). The chemical equation representing this process is provided in the upper half of Fi ...
section_2_review_set
... 17. What seven elements are found in groups of two in nature? 18. What element is found in nature in groups of four? 19. What element is found in nature in groups of eight? 20. What two elements are liquid at room temperature? 21. What five elements are reactive gases? 22. Identify the following ele ...
... 17. What seven elements are found in groups of two in nature? 18. What element is found in nature in groups of four? 19. What element is found in nature in groups of eight? 20. What two elements are liquid at room temperature? 21. What five elements are reactive gases? 22. Identify the following ele ...
Masterton and Hurley Chapter 3
... • In the laboratory, substances are weighed on balances, in units of grams • The mole allows us to relate the number of grams of a substance to the number of atoms or molecules of a substance ...
... • In the laboratory, substances are weighed on balances, in units of grams • The mole allows us to relate the number of grams of a substance to the number of atoms or molecules of a substance ...
Application of the Purdue Ontology for Pharmaceutical Engineering
... 2.1. Material Ontology (POME) There had been some work done to describe materials in an explicit manner including the Standard for the Exchange of Product Data STEP (ISO 10303) and OntoCAPE, which included descriptions of phases, chemical components and reactions (Yang and Marquardt, 2004). However, ...
... 2.1. Material Ontology (POME) There had been some work done to describe materials in an explicit manner including the Standard for the Exchange of Product Data STEP (ISO 10303) and OntoCAPE, which included descriptions of phases, chemical components and reactions (Yang and Marquardt, 2004). However, ...
"Introduction" Kinetics in Process Chemistry: Case Studies Baran Group Meeting Mike DeMartino
... Defluorinated product (8) increased with the aging of the hydrogenation mixture at a rate of < 0.01 area % per hr. This needed to be worked out, and a goal was set for < 0.1 area % total. It was thought that hydrogen mass transfer effects could be responsible for variable kinetics observed in the hy ...
... Defluorinated product (8) increased with the aging of the hydrogenation mixture at a rate of < 0.01 area % per hr. This needed to be worked out, and a goal was set for < 0.1 area % total. It was thought that hydrogen mass transfer effects could be responsible for variable kinetics observed in the hy ...
Thermochemistry only Sp 12 unit I
... ΔHf°= - 74.9 kj/mole The above elements are in their standard states. ΔHf° are important since they can be used to calculate heats of reaction that are not conveniently measured directly Example 1: For the reaction: Fe2O3 (s) + 3 CO(g) 2 Fe (s) + 3 CO2 (g) , the value of ΔHrxn is -23.5 kj. The sta ...
... ΔHf°= - 74.9 kj/mole The above elements are in their standard states. ΔHf° are important since they can be used to calculate heats of reaction that are not conveniently measured directly Example 1: For the reaction: Fe2O3 (s) + 3 CO(g) 2 Fe (s) + 3 CO2 (g) , the value of ΔHrxn is -23.5 kj. The sta ...
Eighth Grade Review - PAMS-Doyle
... • Neutrons can be determined by subtracting the atomic mass from the atomic number. ...
... • Neutrons can be determined by subtracting the atomic mass from the atomic number. ...
Midterm 1 Spring 2004
... 15. (7 points) A solid powder is known to be a mixture of NaCl and Na2CO3, but the relative amounts of each compound in the sample are unknown. Sodium carbonate reacts with hydrochloric acid according to the equation: Na2CO3(aq) +2 HCl(aq) ? 2NaCl(aq) + H2O(l)+CO2(g) A solution of the mixture is pre ...
... 15. (7 points) A solid powder is known to be a mixture of NaCl and Na2CO3, but the relative amounts of each compound in the sample are unknown. Sodium carbonate reacts with hydrochloric acid according to the equation: Na2CO3(aq) +2 HCl(aq) ? 2NaCl(aq) + H2O(l)+CO2(g) A solution of the mixture is pre ...
- Cypress HS
... Many chemical reactions, especially those of organic substances, do not go to completion. Rather, they come to a point of chemical equilibrium before the reactants are fully converted to products. At the point of equilibrium, the concentrations of all reactants remain constant with time. The positio ...
... Many chemical reactions, especially those of organic substances, do not go to completion. Rather, they come to a point of chemical equilibrium before the reactants are fully converted to products. At the point of equilibrium, the concentrations of all reactants remain constant with time. The positio ...
Regents_Chem_Core_for_review
... III.3 The empirical formula of a compound is the simplest whole-number ratio of atoms of the elements in a compound. It may be different from the molecular formula, which is the actual ratio of atoms in a molecule of that compound. (3.3d) III.4 In all chemical reactions there is a conservation of m ...
... III.3 The empirical formula of a compound is the simplest whole-number ratio of atoms of the elements in a compound. It may be different from the molecular formula, which is the actual ratio of atoms in a molecule of that compound. (3.3d) III.4 In all chemical reactions there is a conservation of m ...
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.