Please do not remove this page. The periodic table, constants, and
... Consider the balanced equation given for the reaction of iodate ion with iodide ion in acidic solution: IO3– (aq) + 5 I– (aq) + 6 H+ (aq) 3 I2 (aq) + 3 H2O (l) At a particular instant in time, the value of ∆[I–]/∆t = 4.0 x 10–3 M•s–1. What is the value of ∆[I2]/∆t at the same instant in ...
... Consider the balanced equation given for the reaction of iodate ion with iodide ion in acidic solution: IO3– (aq) + 5 I– (aq) + 6 H+ (aq) 3 I2 (aq) + 3 H2O (l) At a particular instant in time, the value of ∆[I–]/∆t = 4.0 x 10–3 M•s–1. What is the value of ∆[I2]/∆t at the same instant in ...
Power Point for Equilibrium
... • The instant the pressure increases, the system is not at equilibrium and the concentration of both gases has increased. • The system moves to reduce the number moles of gas (i.e. the forward reaction is favored). • A new equilibrium is established in which the mixture is lighter because colorless ...
... • The instant the pressure increases, the system is not at equilibrium and the concentration of both gases has increased. • The system moves to reduce the number moles of gas (i.e. the forward reaction is favored). • A new equilibrium is established in which the mixture is lighter because colorless ...
Introduction to Kinetics and Equilibrium
... Kinetics and equilibrium are two of the most important areas in chemistry Entire books and important areas in chemistry. Entire books and courses at the undergraduate and graduate level are devoted to them. Chemical kinetics – the study of the rates of chemical processes Equilibrium ‐ the cond ...
... Kinetics and equilibrium are two of the most important areas in chemistry Entire books and important areas in chemistry. Entire books and courses at the undergraduate and graduate level are devoted to them. Chemical kinetics – the study of the rates of chemical processes Equilibrium ‐ the cond ...
Gizmos: Types of Reactions
... Introduction: Chemical equations show how compounds and elements react with one another. An element is a substance consisting of one kind of atom, such as aluminum (Al) or oxygen gas (O2). A compound is a substance made of more than one kind of atom, such as water (H2O) or table salt (NaCl). Questio ...
... Introduction: Chemical equations show how compounds and elements react with one another. An element is a substance consisting of one kind of atom, such as aluminum (Al) or oxygen gas (O2). A compound is a substance made of more than one kind of atom, such as water (H2O) or table salt (NaCl). Questio ...
Chapter 14…Kinetic Theory
... How many grams of NaNO3 will dissolve at 30C? Which substance is least soluble at 10C? Which two substances have the same solubility at 72C? 80 grams of KBr placed in 60C creates a (saturated/unsaturated/supersaturated) solution. When Be(NO3)2 (aq) and NaOH (aq) are mixed together, the resulting ...
... How many grams of NaNO3 will dissolve at 30C? Which substance is least soluble at 10C? Which two substances have the same solubility at 72C? 80 grams of KBr placed in 60C creates a (saturated/unsaturated/supersaturated) solution. When Be(NO3)2 (aq) and NaOH (aq) are mixed together, the resulting ...
Chemical Equilibrium Equilibrium A state where the reactants and
... 1) the tendency of the reaction to ___________ (but not the _______________) 2) whether a given set of concentrations represent an __________________ condition 3) the equilibrium position that will be achieved from a given set of __________ concentrations. The Extent of a Reaction The tendency for ...
... 1) the tendency of the reaction to ___________ (but not the _______________) 2) whether a given set of concentrations represent an __________________ condition 3) the equilibrium position that will be achieved from a given set of __________ concentrations. The Extent of a Reaction The tendency for ...
Practice Questions Section 2
... Write balanced chemical equations for each of the following. Pay close attention to the physical states! Also - you must include the charge when writing ions, otherwise your answer is incorrect. Do not balance these equations using fractions for coefficients. sulfur dioxide gas combines with oxygen ...
... Write balanced chemical equations for each of the following. Pay close attention to the physical states! Also - you must include the charge when writing ions, otherwise your answer is incorrect. Do not balance these equations using fractions for coefficients. sulfur dioxide gas combines with oxygen ...
nomenclature review
... ________ Magnesium chloride is dissolved in water. ________ Hydrochloric acid neutralizes sodium hydroxide to form sodium chloride and water. 13. Why are phase changes considered only physical changes? 14. Sketch an example of the following at the molecular level: a. a gaseous compound b. a mixture ...
... ________ Magnesium chloride is dissolved in water. ________ Hydrochloric acid neutralizes sodium hydroxide to form sodium chloride and water. 13. Why are phase changes considered only physical changes? 14. Sketch an example of the following at the molecular level: a. a gaseous compound b. a mixture ...
1 Unit 11-12: Equilibrium and Acid/Bases Notes Colligative
... ‐ With kinetics, we saw that the rate of the forward reaction slows (neg sign) because the reactants are being used up, the opposite applies for the reverse reaction ‐ Once some of the products form, they can react together to form “reactants.” Their rate of reaction starts slow (rate reverse), ...
... ‐ With kinetics, we saw that the rate of the forward reaction slows (neg sign) because the reactants are being used up, the opposite applies for the reverse reaction ‐ Once some of the products form, they can react together to form “reactants.” Their rate of reaction starts slow (rate reverse), ...
Chemistry 2nd Semester Final Exam Review Chemical Bonds Give
... 24. What gas is produced when an acid reacts with a metal? 25. What is the Arrhenius definition for acids and bases? 26. What is the Brønsted-Lowry definition for acids and bases? 27. Describe the dissociation (ionization) of strong acids and bases versus weak acids and bases. 28. List the 6 strong ...
... 24. What gas is produced when an acid reacts with a metal? 25. What is the Arrhenius definition for acids and bases? 26. What is the Brønsted-Lowry definition for acids and bases? 27. Describe the dissociation (ionization) of strong acids and bases versus weak acids and bases. 28. List the 6 strong ...
2nd Semester Final Review
... 24. What gas is produced when an acid reacts with a metal? 25. What is the Arrhenius definition for acids and bases? 26. What is the Brønsted-Lowry definition for acids and bases? 27. Describe the dissociation (ionization) of strong acids and bases versus weak acids and bases. 28. List the 6 strong ...
... 24. What gas is produced when an acid reacts with a metal? 25. What is the Arrhenius definition for acids and bases? 26. What is the Brønsted-Lowry definition for acids and bases? 27. Describe the dissociation (ionization) of strong acids and bases versus weak acids and bases. 28. List the 6 strong ...
Examination 1 - Idaho State University
... The 2nd and 3rd Laws of Thermodynamics focus on the entropy which is a measure of the randomness or disorder. The entropy can tell us about what processes are spontaneous or naturally possible. A statement of the 2nd Law of thermodynamics is that for any irreversible process the entropy of the unive ...
... The 2nd and 3rd Laws of Thermodynamics focus on the entropy which is a measure of the randomness or disorder. The entropy can tell us about what processes are spontaneous or naturally possible. A statement of the 2nd Law of thermodynamics is that for any irreversible process the entropy of the unive ...
ExamView - Untitled.tst
... ____ 13. Thomson made his discovery about the atom during an experiment using a. thermal energy. c. cathode rays b. kinetic energy. d. X rays. ____ 14. In _____ atomic model, negative electrons orbit the positively charged nucleus. a. Dalton’s c. Rutherford’s b. Thomson’s d. Democritus’s ____ 15. Wh ...
... ____ 13. Thomson made his discovery about the atom during an experiment using a. thermal energy. c. cathode rays b. kinetic energy. d. X rays. ____ 14. In _____ atomic model, negative electrons orbit the positively charged nucleus. a. Dalton’s c. Rutherford’s b. Thomson’s d. Democritus’s ____ 15. Wh ...
SPRING 2002 Test 2 1. Which of the following statements is
... A. At equilibrium, the concentrations of all species are constant B. The value of the equilibrium constant depends on the temperature C. At equilibrium, the reaction has stopped D. At equilibrium, the forward and reverse reactions are happening at the same rate E. Pure solids are not included in the ...
... A. At equilibrium, the concentrations of all species are constant B. The value of the equilibrium constant depends on the temperature C. At equilibrium, the reaction has stopped D. At equilibrium, the forward and reverse reactions are happening at the same rate E. Pure solids are not included in the ...
A matter of Equilibrium
... 2 pump in extra H2 …. …. then the reaction will be driven to the __________ 3 remove some of the ammonia…. …. then the reaction will be driven to the __________ 4 Increase the volume of the container…. …. then the reaction will be driven to the __________ ...
... 2 pump in extra H2 …. …. then the reaction will be driven to the __________ 3 remove some of the ammonia…. …. then the reaction will be driven to the __________ 4 Increase the volume of the container…. …. then the reaction will be driven to the __________ ...
Chemical Equilibrium – Le Chatelier`s Principle
... However, the value of Kc will depend on the ionic strength. All equilibrium constants depend on temperature and pressure (or volume). In this laboratory we will study Le Châtelier's Principle If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or partial p ...
... However, the value of Kc will depend on the ionic strength. All equilibrium constants depend on temperature and pressure (or volume). In this laboratory we will study Le Châtelier's Principle If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or partial p ...
Bonding 1. Which one of the following is most likely to be an ionic
... is 4.0. Starting with equimolar quantities of H2 and I2 and no HI, when equilibrium was established, 0.20 moles of HI was present. How much H2 was used to start the reaction? a. 0.10 mol b. 0.23 mol c. 0.20 mol d. 4.0 mol e. Need to know the volume of the reaction vessel. 8. At a certain temperature ...
... is 4.0. Starting with equimolar quantities of H2 and I2 and no HI, when equilibrium was established, 0.20 moles of HI was present. How much H2 was used to start the reaction? a. 0.10 mol b. 0.23 mol c. 0.20 mol d. 4.0 mol e. Need to know the volume of the reaction vessel. 8. At a certain temperature ...
Chemical equilibrium
In a chemical reaction, chemical equilibrium is the state in which both reactants and products are present in concentrations which have no further tendency to change with time. Usually, this state results when the forward reaction proceeds at the same rate as the reverse reaction. The reaction rates of the forward and backward reactions are generally not zero, but equal. Thus, there are no net changes in the concentrations of the reactant(s) and product(s). Such a state is known as dynamic equilibrium.