Module code SC-2242 Module Title Chemical Thermodynamics and
... -obtain information about the properties of materials from phase diagrams
- apply thermodynamic concepts to understand the properties of mixtures
and solution phase equilibria
Higher order: 10% - present the results of a practical investigation in a concise manner.
- analyse the experimental d ...
CHM 111: General Physical Chemistry 3 Units
... empirical gas laws, Ideal Gas Equation of State, qualitative treatment of kinetic theory of gases,
real gases and deviations from ideal gas laws; liquid, macroscopic properties of liquids,
evaporation, vapor pressure and its variation with temperature, boiling point, heat of vaporization,
Title - Iowa State University
... 3. Which of the following statements about catalysts is false?
a. A catalyst will speed up the rate of a reaction.
b. Catalysts are used in very many commercially important chemical reactions.
c. Catalytic converters are examples of heterogeneous catalysts.
d. A catalyst can cause a nonspontaneous r ...
Practice with Chemical Equilibrium (Chapter 14) (Due 2/17)
... See your instructor if you have questions. Note that for these questions, the symbol "=" is
used to indicate a reversible reaction. Your textbook uses a double-headed arrow.
1. Suppose that equal molar amounts of PCl3 and Cl2 are added to a 2.00 L vessel at 250
C. The two reagents react to form PC ...
2.1 A thermodynamics system and the control volume Chapter 2
... Note：Allow heat to flow in and out.
Mechanical equilibrium P will not changes
with time (Variation in height is negligible)
Chemical equilibrium (Chapter 16)
Thermodynamic equilibrium: when a system is in
equilibrium regarding all possible changes of
Exercises Chem Eqm
... 7.1(a) K = 2.85 x 10-6; (b) ∆rGo = +240 kJ mol-1; (c) ∆rG = 0
7.4(a) Mole fractions A: 0.087, B: 0.370, C: 0.196, D: 0.348, Total: 1.001; (b) Kx – 0.33; (c) p = 0.33; (d)
∆rGo = + 2.8 x 103 J mol-1.
7.6(a) ∆rHo = +2.77 kJ mol-1, ∆rSo = -16.5 J K-1 mol-1
7.9(a) χB = 0.904, χI = 0.096
7.11(a) ∆rGo = – ...
Chemical Equilibrium II
... identical, thus no ____ (macroscopic) change is observed. However,
individual components are actively being transformed at the
microscopic level. Guldberg and Waage showed that the rate of the
reaction in either direction is proportional to what they called the
“active masses” of the various compone ...
... Not all chemical reactions reach completion where the limiting reactant is consumed completely.
In fact, most chemical reactions that occur in living systems never reach completion. Rather, they produce
some amount of product then appear to stop reacting in the forward direction, never fully consumi ...
... When a system is at equilibrium, its state is defined
entirely by the state variables, and not by the
history of the system.
The properties of the system can be described by an
equation of state which specifies the relationship
between these variables.
Big Idea 6
... • Assume reaction occurs in the forward direction.
• Some strategies:
– Perfect square
– Quadratic equation
– 5% rule
(used when K is very small-compared to initial concentration)
Physical Chemistry III
... Objective of the course:
o To acquire the foundations and terminology which characterize the
thermodynamic chemistry of material balances in terms of state
o To apply thermodynamic chemistry to the resolution of significant
problems such as energy changes in chemical reactions, phase chan ...
... Big Idea/Theme: Understanding how effective collisions encourage chemical reactions and how pressure, temperature and concentration
affects the progression of equilibrium in a reversible reaction
Learning Targets: (“I can” or “I will” statements)
I will understand the factors that affect the rate of ...
... when a stream containing variable amounts of
Al3+ mixes 1:1 with a stream containing 200μM
PO43- that is buffered to pH 6,5.
Assume the solution is in equilibrium with AlPO4
Equilibrium Review worksheet
... substances involved in this equilibrium. The vessel is heated to 650 °C. Determine the equilibrium
amount concentrations of each substance, organizing your values in an ICE table. (Hint: use the
value of Kc to determine which side of the reaction is favored, and therefore which substances will
ChE 215, Physical Chemistry
... The objective of this course is to introduce the basic topics in Kinetics, Thermodynamics
and Statistical Mechanics. In fact this course present collection of distinct topics
particularly useful to chemical engineering students. The basic principles in the course
are demonstrated by six experiments ...
Wanganui High School
... asked to write K expressions use K, if KC then write KC!
o Do I need the state symbols? Not for this Unit Standard but if you are putting them in, put
them ALL in, and put them in the right place, inside the ] bracket eg [H2(g)]3 9 [H2)](g)3 8,
PC 1.2 Changes in equilibrium position ar ...
Topics 7 and 17 Outlines
... • The reaction quotient (Q) measures the relative amount of products and reactants present during a reaction at a
particular point in time. Q is the equilibrium expression with non-equilibrium concentrations. The position of the
equilibrium changes with changes in concentration, pressure, and temper ...
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.