NC Standards
Chm.3.1 Understand the factors affecting rate of reaction and chemical equilibrium.
Chm.3.1.1 Explain the factors that affect the rate of a reaction (temperature, concentration, particle size and presence of a catalyst).
• Understand qualitatively that reaction rate is proportional to number of effective collisions.
• Explain that nature of reactants can refer to their complexity and the number of bonds that must be broken and reformed in the course of reaction.
• Explain how temperature (kinetic energy), concentration, and/or pressure affects the number of collisions.
• Explain how increased surface area increases number of collisions.
• Explain how a catalyst lowers the activation energy, so that at a given temperature, more molecules will have energy equal to or greater than the activation energy.
Chm.3.1.2 Explain the conditions of a system at equilibrium.
• Define chemical equilibrium for reversible reactions.
• Distinguish between equal rates and equal concentrations.
• Explain equilibrium expressions for a given reaction.
• Evaluate equilibrium constants as a measure of the extent that the reaction proceeds to completion.
Chm.3.1.3 Infer the shift in equilibrium when a stress is applied to a chemical system (Le Chatelier’s Principle).
• Determine the effects of stresses on systems at equilibrium. (Adding/ removing a reactant or product; adding/removing heat; increasing/decreasing pressure)
• Relate the shift that occurs in terms of the order/disorder of the system.
Chm.3.1.1 Explain the factors that affect the rate of a reaction (temperature, concentration, particle size and presence of a catalyst).
• Understand qualitatively that reaction rate is proportional to number of effective collisions.
• Explain that nature of reactants can refer to their complexity and the number of bonds that must be broken and reformed in the course of reaction.
• Explain how temperature (kinetic energy), concentration, and/or pressure affects the number of collisions.
• Explain how increased surface area increases number of collisions.
• Explain how a catalyst lowers the activation energy, so that at a given temperature, more molecules will have energy equal to or greater than the activation energy.
Chm.3.1.2 Explain the conditions of a system at equilibrium.
• Define chemical equilibrium for reversible reactions.
• Distinguish between equal rates and equal concentrations.
• Explain equilibrium expressions for a given reaction.
• Evaluate equilibrium constants as a measure of the extent that the reaction proceeds to completion.
Chm.3.1.3 Infer the shift in equilibrium when a stress is applied to a chemical system (Le Chatelier’s Principle).
• Determine the effects of stresses on systems at equilibrium. (Adding/ removing a reactant or product; adding/removing heat; increasing/decreasing pressure)
• Relate the shift that occurs in terms of the order/disorder of the system.
Vocabulary
activation energy
chemical equilibrium
collision theory
entropy
equilibrium constant
free energy
inhibitor
intermediate
law of disorder
Le Chatlier's principle
rate
reversible reaction
spontaneous reaction
chemical equilibrium
collision theory
entropy
equilibrium constant
free energy
inhibitor
intermediate
law of disorder
Le Chatlier's principle
rate
reversible reaction
spontaneous reaction
Rates of Reaction
Learning Target(s)
I can explain the factors that affect the rate of a reaction (temperature, concentration, particle size and presence of a catalyst).
chem_jan_2__2_.pptx | |
File Size: | 138 kb |
File Type: | pptx |
Rate of Reaction
Reversible Reactions & Equilibrium
Learning Target(s)
I can explain the conditions of a system at equilibrium.
I can infer the shift in equilibrium when a stress is applied to a chemical system (Le Chatelier’s Principle).
I can infer the shift in equilibrium when a stress is applied to a chemical system (Le Chatelier’s Principle).
chem_jan_2.pptx | |
File Size: | 88 kb |
File Type: | pptx |