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 ...
... -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, Clausius-C ...
... 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, Clausius-C ...
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 ...
... 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 o C. The two reagents react to form PC ...
... 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 o 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 state. 機械工程系 陳俊勳老師 ...
... 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 state. 機械工程系 陳俊勳老師 ...
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 = – ...
... 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 ...
... 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 ...
P2-Equilibrium Activity
... 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 ...
... 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 ...
Lecture I
... 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. ...
... 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) ...
... • 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 functions. o To apply thermodynamic chemistry to the resolution of significant problems such as energy changes in chemical reactions, phase chan ...
... Objective of the course: o To acquire the foundations and terminology which characterize the thermodynamic chemistry of material balances in terms of state functions. o To apply thermodynamic chemistry to the resolution of significant problems such as energy changes in chemical reactions, phase chan ...
Subject:
... 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 ...
... 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 ...
Lecture3_Module_19_2..
... 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 ...
... 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 incre ...
... 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 incre ...
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 ...
... 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, [FeSCN]2+(aq) PC 1.2 Changes in equilibrium position ar ...
... 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, [FeSCN]2+(aq) 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 ...
... • 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 ...
Kc and Kp Conversions Hess`s Law in Equilibrium Constants
... The equilibrium constant of a reaction that has been multiplied by a number is the equilibrium constant raised to a power that is equal to that number. ...
... The equilibrium constant of a reaction that has been multiplied by a number is the equilibrium constant raised to a power that is equal to that number. ...
