NYOS Charter School
... 14. Which of the following is true of equilibria reactions in chemistry? a. reactions with a large, positive Keq proceed very quickly b. all particle movement stops when equilibrium is reached c. particles are continuously moving back and forth between reactants and products d. the state of equilibr ...
... 14. Which of the following is true of equilibria reactions in chemistry? a. reactions with a large, positive Keq proceed very quickly b. all particle movement stops when equilibrium is reached c. particles are continuously moving back and forth between reactants and products d. the state of equilibr ...
Chemical reactions
... Reaction products = substances formed in a chemical reaction. They are written in the right term of the equation Because in a chemical reaction, the nature of atoms of the substances is not changed, the chemical equations are equalized so that the number of atoms of a certain element from the left t ...
... Reaction products = substances formed in a chemical reaction. They are written in the right term of the equation Because in a chemical reaction, the nature of atoms of the substances is not changed, the chemical equations are equalized so that the number of atoms of a certain element from the left t ...
syllabus for entrance examination - NTU.edu
... Reference should be made to application of the principles of kinetics and equilibria to this process. ...
... Reference should be made to application of the principles of kinetics and equilibria to this process. ...
09 Stoichiometry WS Stoichiometry WS
... 10. A car battery produces electrical energy with the following chemical reaction: Pb(s) + PbO2(s) + 2H2SO4(aq) 2PbSO4(s) + 2H2O(l) If the battery loses 340. g of lead in this reaction, how many moles of lead(II) sulfate are produced? 11. In a space shuttle, the CO2 that the crew exhales is removed ...
... 10. A car battery produces electrical energy with the following chemical reaction: Pb(s) + PbO2(s) + 2H2SO4(aq) 2PbSO4(s) + 2H2O(l) If the battery loses 340. g of lead in this reaction, how many moles of lead(II) sulfate are produced? 11. In a space shuttle, the CO2 that the crew exhales is removed ...
Chemistry 21 A - El Camino College
... a) positive ions are called ____________________________________________ b) negative ions are called ____________________________________________ 16. Reactions represented in the following equations take place in water solutions. Write each reaction in total ionic form, then identify spectator ions ...
... a) positive ions are called ____________________________________________ b) negative ions are called ____________________________________________ 16. Reactions represented in the following equations take place in water solutions. Write each reaction in total ionic form, then identify spectator ions ...
double-replacement reaction
... Predicting whether a reaction will occur In a single-replacement reaction, a more active metal displaces a less active metal according to the activity series. • In a double-replacement reaction, two aqueous solutions produce a precipitate of an insoluble compound. ...
... Predicting whether a reaction will occur In a single-replacement reaction, a more active metal displaces a less active metal according to the activity series. • In a double-replacement reaction, two aqueous solutions produce a precipitate of an insoluble compound. ...
AP Chemistry Test Review
... 34) Calculate K by doing ICE box problems 35) acid/base definitions…Bronsted-Lowry = acids donate protons; Lewis= acids accept e- pair 36) calculate pH, pOH, [H+], [OH−] 37) acid equilibrium problems…ICE box…remember pH can be used to find [H+]. 38) salt pH…example: Na2CO3 = slightly basic; Al(NO3)3 ...
... 34) Calculate K by doing ICE box problems 35) acid/base definitions…Bronsted-Lowry = acids donate protons; Lewis= acids accept e- pair 36) calculate pH, pOH, [H+], [OH−] 37) acid equilibrium problems…ICE box…remember pH can be used to find [H+]. 38) salt pH…example: Na2CO3 = slightly basic; Al(NO3)3 ...
inorganic-chemistry-gp-i-alkali-metals
... These are reaction which are given by the second group metals and so are important. The Uses are important of the potassium superoxide- it is used as a absorber of the carbon dioxide and releasing di oxygen gas, which makes it helpful for use in space capsules, submarines to function. Also is used ...
... These are reaction which are given by the second group metals and so are important. The Uses are important of the potassium superoxide- it is used as a absorber of the carbon dioxide and releasing di oxygen gas, which makes it helpful for use in space capsules, submarines to function. Also is used ...
Reactions (The Basics)
... Important stuff! Four abbreviations are used to indicate physical states of chemicals: shown as subscripts in the chemical equation ...
... Important stuff! Four abbreviations are used to indicate physical states of chemicals: shown as subscripts in the chemical equation ...
Cluster Fragmentation and Catalysis
... In recent years, there has been a mounting interest in the use of lanthanide ions for biochemical applications. Many organolanthanide complexes have found their way into mainstream science with varied uses. For example, many lanthanide-chelate complexes have been used as contrast agents for MRI, as ...
... In recent years, there has been a mounting interest in the use of lanthanide ions for biochemical applications. Many organolanthanide complexes have found their way into mainstream science with varied uses. For example, many lanthanide-chelate complexes have been used as contrast agents for MRI, as ...
CHEM_2nd_Semester_Final_R eview
... 40. What happens to atoms or molecules as their temperature is increased? 41. Describe heat flow. 42. What is the difference between an exothermic reaction and an endothermic reaction? 43. Draw an energy diagram for an endothermic and exothermic reaction. 44. Are the following changes of state exoth ...
... 40. What happens to atoms or molecules as their temperature is increased? 41. Describe heat flow. 42. What is the difference between an exothermic reaction and an endothermic reaction? 43. Draw an energy diagram for an endothermic and exothermic reaction. 44. Are the following changes of state exoth ...
Chemistry 2nd Semester Final Exam Review Chemical Bonds Give
... 40. What happens to atoms or molecules as their temperature is increased? 41. Describe heat flow. 42. What is the difference between an exothermic reaction and an endothermic reaction? 43. Draw an energy diagram for an endothermic and exothermic reaction. 44. Are the following changes of state exoth ...
... 40. What happens to atoms or molecules as their temperature is increased? 41. Describe heat flow. 42. What is the difference between an exothermic reaction and an endothermic reaction? 43. Draw an energy diagram for an endothermic and exothermic reaction. 44. Are the following changes of state exoth ...
2nd Semester Final Review
... 40. What happens to atoms or molecules as their temperature is increased? 41. Describe heat flow. 42. What is the difference between an exothermic reaction and an endothermic reaction? 43. Draw an energy diagram for an endothermic and exothermic reaction. 44. Are the following changes of state exoth ...
... 40. What happens to atoms or molecules as their temperature is increased? 41. Describe heat flow. 42. What is the difference between an exothermic reaction and an endothermic reaction? 43. Draw an energy diagram for an endothermic and exothermic reaction. 44. Are the following changes of state exoth ...
How are Molecules Depicted? - Belle Vernon Area School District
... E level of an atom and determines the chemical properties Lewis Structure = a structure in which e- are represented by dots: dot pairs or dashes b/t 2 atomic symbols represents pairs in covalent bonds ...
... E level of an atom and determines the chemical properties Lewis Structure = a structure in which e- are represented by dots: dot pairs or dashes b/t 2 atomic symbols represents pairs in covalent bonds ...
Practice with Chemical Equilibrium (Chapter 14) (Due 2/17)
... Practice with Chemical Equilibrium (Chapter 14) (Due 2/17) Here are four additional practice exercises concerning chemical equilibrium (Chapter 14). See your instructor if you have questions. Note that for these questions, the symbol "=" is used to indicate a reversible reaction. Your textbook uses ...
... Practice with Chemical Equilibrium (Chapter 14) (Due 2/17) Here are four additional practice exercises concerning chemical equilibrium (Chapter 14). See your instructor if you have questions. Note that for these questions, the symbol "=" is used to indicate a reversible reaction. Your textbook uses ...
CHM 101
... The reactants in a chemical change have 487 kJ of energy. The change they undergo has a H = -157 kJ. The activation energy for the reaction is 570 kJ. a. Draw the energy vs reaction progress graph on the axes above paying attention to all values. Label a point that represents all products and one t ...
... The reactants in a chemical change have 487 kJ of energy. The change they undergo has a H = -157 kJ. The activation energy for the reaction is 570 kJ. a. Draw the energy vs reaction progress graph on the axes above paying attention to all values. Label a point that represents all products and one t ...
HONORS: UNIT 2B: Antacids Below are the class objectives
... balancing equations Write and balance chemical equations predicting product(s) in a reaction using the reference tables Write and balance ionic & net ionic equations** Investigate variables that affect the rate of a reaction (nature of reactants, concentration, surface area, and temperature Explain ...
... balancing equations Write and balance chemical equations predicting product(s) in a reaction using the reference tables Write and balance ionic & net ionic equations** Investigate variables that affect the rate of a reaction (nature of reactants, concentration, surface area, and temperature Explain ...
ENZYMES
... a. _______ Add more enzyme b. _______ Add more substrate c. _______ Adjust pH to optimal level (Optimal Means Perfect Conditions) d. _______ Freezing e. _______ Increase temperature slightly ...
... a. _______ Add more enzyme b. _______ Add more substrate c. _______ Adjust pH to optimal level (Optimal Means Perfect Conditions) d. _______ Freezing e. _______ Increase temperature slightly ...
A.P. Chemistry
... 2Na(s) + Cl2(g) 2NaCl(s) oxidation: 2 Na 2Na+1 + 2ereduction: Cl2 + 2e- 2Cl-1 Example: Write the half-reactions for the following reaction: 2Al(s) + 3I2(s) 2AlI3(s) ...
... 2Na(s) + Cl2(g) 2NaCl(s) oxidation: 2 Na 2Na+1 + 2ereduction: Cl2 + 2e- 2Cl-1 Example: Write the half-reactions for the following reaction: 2Al(s) + 3I2(s) 2AlI3(s) ...
synthesis reaction
... nitric acid, HNO3, magnesium nitrate and carbonic acid form. Carbonic acid then breaks down into water and carbon dioxide. Which two types of reactions take place in this process? A: Double-replacement and decomposition Single-replacement reactions can take place with nonmetals. In the following equ ...
... nitric acid, HNO3, magnesium nitrate and carbonic acid form. Carbonic acid then breaks down into water and carbon dioxide. Which two types of reactions take place in this process? A: Double-replacement and decomposition Single-replacement reactions can take place with nonmetals. In the following equ ...
10 TEST 2 (of 3)
... Use the ideal gas law (PV = nRT) to calculate the ideal gas law constant R at standard temperature and pressure (273 K, 1.00 atm) assuming a molar volume of 22.4 L. ...
... Use the ideal gas law (PV = nRT) to calculate the ideal gas law constant R at standard temperature and pressure (273 K, 1.00 atm) assuming a molar volume of 22.4 L. ...
CH 115 Exam 2 - UAB General Chemistry Supplemental Instruction
... Multiple Choice (5 percent each, no partial credit) Assume the chemical equations on this exam are NOT balanced unless stated otherwise. 1. Balance the equation and give the stoichiometric coefficient for HCl ...
... Multiple Choice (5 percent each, no partial credit) Assume the chemical equations on this exam are NOT balanced unless stated otherwise. 1. Balance the equation and give the stoichiometric coefficient for HCl ...
Lewis acid catalysis
In Lewis acid catalysis of organic reactions, a metal-based Lewis acid acts as an electron pair acceptor to increase the reactivity of a substrate. Common Lewis acid catalysts are based on main group metals such as aluminum, boron, silicon, and tin, as well as many early (titanium, zirconium) and late (iron, copper, zinc) d-block metals. The metal atom forms an adduct with a lone-pair bearing electronegative atom in the substrate, such as oxygen (both sp2 or sp3), nitrogen, sulfur, and halogens. The complexation has partial charge-transfer character and makes the lone-pair donor effectively more electronegative, activating the substrate toward nucleophilic attack, heterolytic bond cleavage, or cycloaddition with 1,3-dienes and 1,3-dipoles.Many classical reactions involving carbon–carbon or carbon–heteroatom bond formation can be catalyzed by Lewis acids. Examples include the Friedel-Crafts reaction, the aldol reaction, and various pericyclic processes that proceed slowly at room temperature, such as the Diels-Alder reaction and the ene reaction. In addition to accelerating the reactions, Lewis acid catalysts are able to impose regioselectivity and stereoselectivity in many cases.Early developments in Lewis acid reagents focused on easily available compounds such as TiCl4, BF3, SnCl4, and AlCl3. The relative strengths of these (and other) Lewis acids may be estimated from NMR spectroscopy by the Childs method or the Gutmann-Beckett method. Over the years, versatile catalysts bearing ligands designed for specific applications have facilitated improvement in both reactivity and selectivity of Lewis acid-catalyzed reactions. More recently, Lewis acid catalysts with chiral ligands have become an important class of tools for asymmetric catalysis.Challenges in the development of Lewis acid catalysis include inefficient catalyst turnover (caused by catalyst affinity for the product) and the frequent requirement of two-point binding for stereoselectivity, which often necessitates the use of auxiliary groups.