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6. Macroscopic equilibrium states and state variables (Hiroshi
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 ...
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Le Chatelier`s Principle Notes

4. Which of the following describes how a Keq value is related to the
4. Which of the following describes how a Keq value is related to the

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Unit 5 • What Do Atoms Look Like
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 ...
(General Equilibrium) Part 1
(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 matter of Equilibrium
A matter of Equilibrium

chemical equilibrium
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 ...
Chemical Thermodynamics: Principles and Applications Brochure
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 ...
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exercise on Chapter 13 - Louisiana Tech University

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2.4 Chemical equilibria
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Material Equilibrium

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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. ...
Chapter 7 Review
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) ...
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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 ...
Dr. Baxley`s Equilibrium Worksheet
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... 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 ...
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Chapter 12 – Static equilibrium and Elasticity Lecture 1

Test review
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 ...
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... 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
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
Lecture 2: Stability analysis for ODEs
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 ...
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Thermodynamic equilibrium

Thermodynamic equilibrium is an axiomatic concept of classical thermodynamics. It is an internal state of a single thermodynamic system, or a relation between several thermodynamic systems connected by permeable walls. In thermodynamic equilibrium there are no net macroscopic flows of matter or of energy, either within a system or between systems. In a system in its own state of internal thermodynamic equilibrium, no macroscopic change occurs. Systems in mutual thermodynamic equilibrium are simultaneously in mutual thermal, mechanical, chemical, and radiative equilibria. Systems can be in one kind of mutual equilibrium, though not in others. In thermodynamic equilibrium, all kinds of equilibrium hold at once and indefinitely, until disturbed by a thermodynamic operation. In a macroscopic equilibrium, almost or perfectly, exactly balanced microscopic exchanges occur; this is part of the notion of macroscopic equilibrium.An isolated thermodynamic system in its own state of internal thermodynamic equilibrium has a uniform temperature. If its surroundings impose some unchanging long range force field on it, it may consist of one phase or may exhibit several spatially unchanging internal phases. If its surroundings impose no long range force field on it, then either (1) it is spatially homogeneous, with all intensive properties being uniform; or (2) it has several internal phases, which may exhibit indefinitely persistent continuous spontaneous microscopic or mesoscopic fluctuations.In non-equilibrium systems, by contrast, there are net flows of matter or energy. If such changes can be triggered to occur in a system in which they are not already occurring, it is said to be in a metastable equilibrium.It is an axiom of thermodynamics that when a body of material starts from a non-equilibrium state of non-homogeneity or chemical non-equilibrium, and, by a thermodynamic operation, is then isolated, it spontaneously evolves towards its own internal state of thermodynamic equilibrium. This axiom is presupposed by the second law of thermodynamics, which restricts what can happen when a system, having reached thermodynamic equilibrium, with a well defined entropy, is subject to a thermodynamic operation.
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