6. Macroscopic equilibrium states and state variables (Hiroshi
... and P are not spatially uniform (i.e., T (r,t ) , P (r,t ) , n ( t ) ). A prime example of a system always ...
... and P are not spatially uniform (i.e., T (r,t ) , P (r,t ) , n ( t ) ). A prime example of a system always ...
4. Which of the following describes how a Keq value is related to the
... following must be true for the forward reaction? A. Enthalpy change favours products and entropy is increasing. B. Enthalpy change favours reactants and entropy is increasing. C. Enthalpy change favours products and entropy is decreasing. D. Enthalpy change favours reactants and entropy is decreasin ...
... following must be true for the forward reaction? A. Enthalpy change favours products and entropy is increasing. B. Enthalpy change favours reactants and entropy is increasing. C. Enthalpy change favours products and entropy is decreasing. D. Enthalpy change favours reactants and entropy is decreasin ...
Unit 5 • What Do Atoms Look Like
... Arrhenius only dealt with aqueous solutions. When NH3 and HCl meet in the air, a proton (H+) is transferred from the HCl to the NH3. The two resulting ions immediately are attracted to each other to form the solid, NH4Cl(s) which we see as smoke. HCl(g) is a B-L acid because it donates a proton. NH3 ...
... Arrhenius only dealt with aqueous solutions. When NH3 and HCl meet in the air, a proton (H+) is transferred from the HCl to the NH3. The two resulting ions immediately are attracted to each other to form the solid, NH4Cl(s) which we see as smoke. HCl(g) is a B-L acid because it donates a proton. NH3 ...
(General Equilibrium) Part 1
... a. In equilibrium mixture: ________________ b. Reaction proceeds almost to completion. (product favored) c. Position of reaction is _________________ 2. Small value of Kc ( < 10-3) a. In equilibrium mixture: ________________ b. Reaction hardly proceeds at all. (reactant favored) c. Position of the r ...
... a. In equilibrium mixture: ________________ b. Reaction proceeds almost to completion. (product favored) c. Position of reaction is _________________ 2. Small value of Kc ( < 10-3) a. In equilibrium mixture: ________________ b. Reaction hardly proceeds at all. (reactant favored) c. Position of the r ...
chemical equilibrium
... • Construct the balanced equation, including state symbols (aq), (g) etc. • Determine the number of moles of each species at equilibrium • Divide moles by the volume (in dm3) to get the equilibrium concentrations in mol dm-3 (If no volume is quoted, use a V; it will probably cancel out) • From the e ...
... • Construct the balanced equation, including state symbols (aq), (g) etc. • Determine the number of moles of each species at equilibrium • Divide moles by the volume (in dm3) to get the equilibrium concentrations in mol dm-3 (If no volume is quoted, use a V; it will probably cancel out) • From the e ...
Chemical Thermodynamics: Principles and Applications Brochure
... historical interest. The text is written in an informal but rigorous style, including ancedotes about some of the great thermodynamicists (with some of whom the authors have had a personal relationship), and focuses on "real" systems in the discussion and figures, in contrast to the generic examples ...
... historical interest. The text is written in an informal but rigorous style, including ancedotes about some of the great thermodynamicists (with some of whom the authors have had a personal relationship), and focuses on "real" systems in the discussion and figures, in contrast to the generic examples ...
exercise on Chapter 13 - Louisiana Tech University
... Louisiana Tech University, Chemistry 102 POGIL Exercise on Chapter 14. Chemical Equilibrium 1 Why? ...
... Louisiana Tech University, Chemistry 102 POGIL Exercise on Chapter 14. Chemical Equilibrium 1 Why? ...
Water Chemistry 3
... Thermodynamics tells us where the system should go at equilibrium, and kinetics tells us how fast. • Definition of Equilibrium 1) A system at equilibrium has none of its properties changing with time, no matter how long it is observed 2) A system at equilibrium will return to that state after being ...
... Thermodynamics tells us where the system should go at equilibrium, and kinetics tells us how fast. • Definition of Equilibrium 1) A system at equilibrium has none of its properties changing with time, no matter how long it is observed 2) A system at equilibrium will return to that state after being ...
2.4 Chemical equilibria
... Eventually, the rates of the two reactions will become equal. A and B will be converting into C and D at exactly the same rate as C and D convert back into A and B again. ...
... Eventually, the rates of the two reactions will become equal. A and B will be converting into C and D at exactly the same rate as C and D convert back into A and B again. ...
Physical chemistry 1
... 4. Describe simple electrochemical and thermodynamic measurements; 5. Experimentally determine certain physical variables; 6. Apply calculation in solving physical and chemical problems. ...
... 4. Describe simple electrochemical and thermodynamic measurements; 5. Experimentally determine certain physical variables; 6. Apply calculation in solving physical and chemical problems. ...
Chapter 7 Review
... For the reaction CO(g) + 2 H2(g) <---> CH3OH(g) + heat; [CO(g)] = 0.025 mol/L, [H2(g) ] = 0.050 mol/L and [CH3OH(g)] = 0.0063 mol/L a) b) ...
... For the reaction CO(g) + 2 H2(g) <---> CH3OH(g) + heat; [CO(g)] = 0.025 mol/L, [H2(g) ] = 0.050 mol/L and [CH3OH(g)] = 0.0063 mol/L a) b) ...
chapter15-burno.1348..
... Significance of the Equilibrium Constant The significance of the equilibrium constant lies in the fact that for a chemical reaction taking place at a particular temperature T, the equilibrium constant (KC or Kp) has a particular numerical value. This means that no matter what the starting concentra ...
... Significance of the Equilibrium Constant The significance of the equilibrium constant lies in the fact that for a chemical reaction taking place at a particular temperature T, the equilibrium constant (KC or Kp) has a particular numerical value. This means that no matter what the starting concentra ...
Dr. Baxley`s Equilibrium Worksheet
... At 450.˚C, Kc = 6.30. An unknown quantity of NH3 is placed in a reaction flask (with no N2 or H2) and is allowed to come to equilibrium at 450. °C. The equilibrium concentration of H2 is then determined to be 0.342 M. Determine the initial concentration of NH3 placed in the flask. (NOTE that you do ...
... At 450.˚C, Kc = 6.30. An unknown quantity of NH3 is placed in a reaction flask (with no N2 or H2) and is allowed to come to equilibrium at 450. °C. The equilibrium concentration of H2 is then determined to be 0.342 M. Determine the initial concentration of NH3 placed in the flask. (NOTE that you do ...
Test review
... _____ 3. Equal masses of three different ideal gases, X, Y, and Z, are mixed in a sealed rigid container. The total pressure is measured to be 9.0 atm. If the temperature of the system remains constant, which of the following statements about the partial pressure of gas X is correct? (A) It depends ...
... _____ 3. Equal masses of three different ideal gases, X, Y, and Z, are mixed in a sealed rigid container. The total pressure is measured to be 9.0 atm. If the temperature of the system remains constant, which of the following statements about the partial pressure of gas X is correct? (A) It depends ...
Ch. 16 Study Guide
... expression. Unknown x values can be discarded in any addition/subtraction operation but not from any multiplication/division operation. When checking whether or not the assumption is valid, the percentage difference should be 5% or less. 23. Successive approximations can be used if the 5% rule is no ...
... expression. Unknown x values can be discarded in any addition/subtraction operation but not from any multiplication/division operation. When checking whether or not the assumption is valid, the percentage difference should be 5% or less. 23. Successive approximations can be used if the 5% rule is no ...
Cheat Sheet for Chemical Equilibrium
... • Given: Initial Concentrations and asked whether a precipitate will form: Calculate Q (no ICE chart needed) and compare with Ksp: o Q>Ksp, precipitate will form o Q=Ksp, at equilibrium o Q
... • Given: Initial Concentrations and asked whether a precipitate will form: Calculate Q (no ICE chart needed) and compare with Ksp: o Q>Ksp, precipitate will form o Q=Ksp, at equilibrium o Q
Lecture 2: Stability analysis for ODEs
... for a model. If the model’s behavior changes when we make small changes to the equations, then we probably can’t trust the model’s predictions very well. Note also that we have our first example of a model with two equilibrium points, one of which is stable while the other is unstable. It is instruc ...
... for a model. If the model’s behavior changes when we make small changes to the equations, then we probably can’t trust the model’s predictions very well. Note also that we have our first example of a model with two equilibrium points, one of which is stable while the other is unstable. It is instruc ...