Slide 1
... • At any given temperature, density does not change. • No matter how much or how little C2H5OH is present, its concentration remains constant. • Therefore, the term in the denominator is a constant and can be combined with K. ...
... • At any given temperature, density does not change. • No matter how much or how little C2H5OH is present, its concentration remains constant. • Therefore, the term in the denominator is a constant and can be combined with K. ...
Unit 3: 1 Equilibrium and the Constant, K
... Learning objective 6.1 The student is able to, given a set of experimental observations regarding physical, chemical, biological, or environmental processes that are reversible, construct an explanation that connects the observations to the reversibility of the underlying chemical reactions or proc ...
... Learning objective 6.1 The student is able to, given a set of experimental observations regarding physical, chemical, biological, or environmental processes that are reversible, construct an explanation that connects the observations to the reversibility of the underlying chemical reactions or proc ...
sch103manual - university of nairobi staff profiles
... state as ice, liquid state as water and in the gaseous state as steam. The physical properties of a substance often depend on the state of the substance. In this section, we will review the states of matter and then look at the behavior of gases. Gases are much simpler than liquids or solids. Molecu ...
... state as ice, liquid state as water and in the gaseous state as steam. The physical properties of a substance often depend on the state of the substance. In this section, we will review the states of matter and then look at the behavior of gases. Gases are much simpler than liquids or solids. Molecu ...
Chemical Equilibrium
... ability to affect the equilibrium. Chemical equilibria can be shifted by changing the conditions that the system experiences. We say that we “stress” the equilibrium. When we stress the equilibrium, the chemical reaction is no longer at equilibrium, and the reaction starts to move back toward equilib ...
... ability to affect the equilibrium. Chemical equilibria can be shifted by changing the conditions that the system experiences. We say that we “stress” the equilibrium. When we stress the equilibrium, the chemical reaction is no longer at equilibrium, and the reaction starts to move back toward equilib ...
Chapter 15: Chemical Equilibrium
... increases). Eventually, a state of chemical equilibrium is reached where the rate of the forward reaction is equal to the rate of the reverse reaction: Rate (forward) = Rate (reverse) kforward[Fe3+][SCN-] = kreverse[FeSCN2+] When this equilibrium state is achieved, the concentrations of all the spec ...
... increases). Eventually, a state of chemical equilibrium is reached where the rate of the forward reaction is equal to the rate of the reverse reaction: Rate (forward) = Rate (reverse) kforward[Fe3+][SCN-] = kreverse[FeSCN2+] When this equilibrium state is achieved, the concentrations of all the spec ...
Chapter 15
... of the reaction products is physically separated from a reaction mixture as a gas (the reaction of a metal carbonate with acid, for example, Figure 15.X), a single reaction arrow is used. The Equilibrium State In Chapter 12, we described the nature of a dynamic equilibrium between a liquid and its v ...
... of the reaction products is physically separated from a reaction mixture as a gas (the reaction of a metal carbonate with acid, for example, Figure 15.X), a single reaction arrow is used. The Equilibrium State In Chapter 12, we described the nature of a dynamic equilibrium between a liquid and its v ...
5548-4.pdf
... orders of magnitude. When the coatings contain predominantly y phase, the error will be low as variation of interdiffusion coefficient with composition is not high. However, when the h phase is formed by heat treatment, the assumption can introduce appreciable error. Hence, Sarkhel and Seigle [4], i ...
... orders of magnitude. When the coatings contain predominantly y phase, the error will be low as variation of interdiffusion coefficient with composition is not high. However, when the h phase is formed by heat treatment, the assumption can introduce appreciable error. Hence, Sarkhel and Seigle [4], i ...
CHAPTER 18
... Some reactions favor products, and others reactants. In equilibrium, the concentrations of reactants and products ...
... Some reactions favor products, and others reactants. In equilibrium, the concentrations of reactants and products ...
chapter 16
... absorb energy overall as it takes place. If this energy comes from the motion (kinetic energy) of the reactants, the particles in the system will be moving more slowly after the reaction than before. The system will have less thermal energy, and the temperature will decrease. Because the system is a ...
... absorb energy overall as it takes place. If this energy comes from the motion (kinetic energy) of the reactants, the particles in the system will be moving more slowly after the reaction than before. The system will have less thermal energy, and the temperature will decrease. Because the system is a ...
GRAPHITE
... heat in the absence of oxygen) of polymer precursor fibers. Polyacrylonitrile (PAN), rayon, pitch, coal tar or petroleum asphalt may be used as precursor materials. Pyrolysis results in transformation of the precursor polymer material to graphite, crystal layers of which are linked in bundles orient ...
... heat in the absence of oxygen) of polymer precursor fibers. Polyacrylonitrile (PAN), rayon, pitch, coal tar or petroleum asphalt may be used as precursor materials. Pyrolysis results in transformation of the precursor polymer material to graphite, crystal layers of which are linked in bundles orient ...
102MSJc14 - Louisiana Tech University
... concentrations and equilibrium concentrations (Section 14 3). 7. Make qualitative predictions about the extent of reaction based upon equilibrium constant values; that is, be able to predict whether a reaction product favored or reactant favored based on the size of the equilibrium constant (Section ...
... concentrations and equilibrium concentrations (Section 14 3). 7. Make qualitative predictions about the extent of reaction based upon equilibrium constant values; that is, be able to predict whether a reaction product favored or reactant favored based on the size of the equilibrium constant (Section ...
chem 102 class notes - Louisiana Tech University
... concentrations and equilibrium concentrations (Section 14 3). 7. Make qualitative predictions about the extent of reaction based upon equilibrium constant values; that is, be able to predict whether a reaction product favored or reactant favored based on the size of the equilibrium constant (Section ...
... concentrations and equilibrium concentrations (Section 14 3). 7. Make qualitative predictions about the extent of reaction based upon equilibrium constant values; that is, be able to predict whether a reaction product favored or reactant favored based on the size of the equilibrium constant (Section ...
Spontaneous Change: Entropy and Gibbs Energy
... Notice that, for the situation just discussed, the state of the system can be described in two ways. At the macroscopic level, the state of the system is described by specifying the total energy, U, and the length, L, of the box. At the molecular level, the state of the system is described in terms ...
... Notice that, for the situation just discussed, the state of the system can be described in two ways. At the macroscopic level, the state of the system is described by specifying the total energy, U, and the length, L, of the box. At the molecular level, the state of the system is described in terms ...
TOPIC 11 Further equilibrium 11.1 Chemical equilibrium
... When making solution A, 25 cm3 of the NaOH solution reacts with 25 cm3 of the CH3COOH solution. This forms some ethanoate ions, CH3COO-(aq), and leaves some unreacted ethanoic acid molecules, CH3COOH. CH3COOH(aq) + OH−(aq) → CH3COO−(aq) + H2O(l) So, solution A contains a mixture of a weak acid, CH3C ...
... When making solution A, 25 cm3 of the NaOH solution reacts with 25 cm3 of the CH3COOH solution. This forms some ethanoate ions, CH3COO-(aq), and leaves some unreacted ethanoic acid molecules, CH3COOH. CH3COOH(aq) + OH−(aq) → CH3COO−(aq) + H2O(l) So, solution A contains a mixture of a weak acid, CH3C ...
Chapter 1 Introduction: Matter and Measurement
... measurements, the Celsius and Kelvin scales are most often used. • The Celsius scale is based on the properties of water. – 0C is the freezing point of water. – 100C is the boiling point of water. Matter And Measurement © 2009, Prentice-Hall, Inc. ...
... measurements, the Celsius and Kelvin scales are most often used. • The Celsius scale is based on the properties of water. – 0C is the freezing point of water. – 100C is the boiling point of water. Matter And Measurement © 2009, Prentice-Hall, Inc. ...
full text pdf
... where the energy required to mill the material is passed through the intersecting streams of compressed air. The milling effect is obtained by collisions of particles itself and with the mill chamber walls. An equipped separator provided a product with a narrow particle size distribution. The 160 UP ...
... where the energy required to mill the material is passed through the intersecting streams of compressed air. The milling effect is obtained by collisions of particles itself and with the mill chamber walls. An equipped separator provided a product with a narrow particle size distribution. The 160 UP ...
chemical equilibrium type 1
... technique that is used to determine whether a reaction it truly at equilibrium is to approach equilibrium starting with reactants in one experiment and starting with products in another. If the same value of the reaction quotient is observed when the concentrations stop changing in both experiments, ...
... technique that is used to determine whether a reaction it truly at equilibrium is to approach equilibrium starting with reactants in one experiment and starting with products in another. If the same value of the reaction quotient is observed when the concentrations stop changing in both experiments, ...
14.1 Dynamic Equilibrium, Keq , and the Mass Action Expression
... When making assumptions, if a reaction has a relatively small keq and a relatively large initial reactant concentration, then the concentration change (x) can often be neglected without introducing significant error. This does not mean x = 0, because then this would mean there is no reaction. It mea ...
... When making assumptions, if a reaction has a relatively small keq and a relatively large initial reactant concentration, then the concentration change (x) can often be neglected without introducing significant error. This does not mean x = 0, because then this would mean there is no reaction. It mea ...
Equilibrium - pedagogics.ca
... In this case, increasing the temperature causes the position of equilibrium to be shifted to the left, i.e. there is less ammonia present at equilibrium at the higher temperature. The effect of a temperature change on a system at equilibrium can be now considered in terms of Le Chatelier’s principle ...
... In this case, increasing the temperature causes the position of equilibrium to be shifted to the left, i.e. there is less ammonia present at equilibrium at the higher temperature. The effect of a temperature change on a system at equilibrium can be now considered in terms of Le Chatelier’s principle ...
SCH4U Exam Review
... 2. Aluminum reacts readily with chlorine gas to produce AlCl3. What is the enthalpy change when 1.0kg of Al reacts with excess Cl2? 2Al + 3Cl2 2AlCl3 + 1408kJ ANS: 2.6x104 kJ 3. If the enthalpy of a system increases by 100 kJ, what must be true about the enthalpy of the surroundings? Explain. 4. W ...
... 2. Aluminum reacts readily with chlorine gas to produce AlCl3. What is the enthalpy change when 1.0kg of Al reacts with excess Cl2? 2Al + 3Cl2 2AlCl3 + 1408kJ ANS: 2.6x104 kJ 3. If the enthalpy of a system increases by 100 kJ, what must be true about the enthalpy of the surroundings? Explain. 4. W ...
The shock tube as wave reactor for kinetic studies and material
... under diffusion free conditions, because it provides a nearly one-dimensional ¯ow, with practically instantaneous heating of reactants. The temperature range under which the reaction could be studied can be extended far beyond that of the conventional ¯ow reactor (1000 K). The shock tube technique h ...
... under diffusion free conditions, because it provides a nearly one-dimensional ¯ow, with practically instantaneous heating of reactants. The temperature range under which the reaction could be studied can be extended far beyond that of the conventional ¯ow reactor (1000 K). The shock tube technique h ...
Kinetic isotope effects of 12CH3D+OH and 13CH3D+OH from 278 to
... no gas leaked back from the chamber into the gas line. Spectra were recorded at each filling step. The procedure was repeated until the mix had a final pressure of 933 hPa. Two experiments were conducted at each of the temperatures 278, 288, 298, and 313 K for each of the two heavy methane isotopolo ...
... no gas leaked back from the chamber into the gas line. Spectra were recorded at each filling step. The procedure was repeated until the mix had a final pressure of 933 hPa. Two experiments were conducted at each of the temperatures 278, 288, 298, and 313 K for each of the two heavy methane isotopolo ...
KINETICS questions
... (a) (i) Determine the order for each of the reactants, NO and H2, from the data given and show your reasoning. (ii) Write the overall rate law for the reaction. (b) Calculate the value of the rate constant, k, for the reaction. Include units. (c) For experiment 2, calculate the concentration of NO r ...
... (a) (i) Determine the order for each of the reactants, NO and H2, from the data given and show your reasoning. (ii) Write the overall rate law for the reaction. (b) Calculate the value of the rate constant, k, for the reaction. Include units. (c) For experiment 2, calculate the concentration of NO r ...
Answer
... Between experiments (1) and (2), [NO2]0 is kept constant and [CO]0 is halved. There is no effect on the rate. The rate is not dependent on [CO]0. It is zero order with respect to CO. Between experiments (2) and (3), [CO]0 is kept constant and [NO]0 is doubled. This causes the rate to increase by a f ...
... Between experiments (1) and (2), [NO2]0 is kept constant and [CO]0 is halved. There is no effect on the rate. The rate is not dependent on [CO]0. It is zero order with respect to CO. Between experiments (2) and (3), [CO]0 is kept constant and [NO]0 is doubled. This causes the rate to increase by a f ...