Potential Energy Diagrams - Chemistry - Catalyst, Endothermic & Exothermic Reactions
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- Опубликовано: 5 сен 2024
- This chemistry video tutorial focuses on potential energy diagrams for endothermic and exothermic reactions. It also shows the effect of a catalyst on the forward and reverse activation energy. It describes the relationship of the enthalpy of a reaction with the potential energy difference of the reactants and products. It also shows you how to identify the transition state or activated complex as well as any intermediates. This video shows you how to draw a 2 step PE diagram and a 3 step potential energy diagram. In addition, it shows you how to identify the slow step or the rate determining step.
Chemical Kinetics - Initial Rate Method:
• Chemical Kinetics - In...
Rate Constant k - Find The Units:
• How To Determine The U...
Integrated Rate Laws - 1st & 2nd Order:
• Integrated Rate Laws -...
Reaction Rate Factors:
• Factors Affecting the ...
Collision Theory & Activation Energy:
• Collision Theory - Arr...
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Potential Energy Diagrams:
• Endothermic and Exothe...
Elementary Rate Laws:
• Elementary Rate Laws -...
Rate Laws of Reaction Mechanisms:
• Writing Rate Laws of R...
Intermediates & Catalysts:
• How To Identify The In...
Types of Catalysts:
• Homogeneous vs Heterog...
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The Equilibrium Expression:
• How To Write The Equil...
Calculating Kp From Kc:
• How To Calculate Kp Fr...
Chemical Equilibrium & Ice Tables:
• Chemical Equilibrium C...
Le Chatelier's Principle:
• Le Chatelier's Principle
Acids and Bases - Introduction:
• Acids and Bases - Basi...
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Can you answer this question? Do these diagrams show Internal energy or just the chemical potential energy? From thermodynamics I know that it's the change in Internal energy (without pressure or volume change) that equals heat exchange.
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how do u know the energy difference is completely driven by enthalpy and not entropy?
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What will be the activation energy of intermediate steps
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pls can we also find the change in enthalpy of an exothermic by subtracting the product directly from the reactant
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If a catalyst was applied to this, would it lower the activation energy of only the RDS?
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How you come to know that the products have more energy than the reactants?
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how do we know if something reaeases high energy?
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Is it product minus reactants or reactants minus products?
Is enthalpy change the same as change in energy??
I'm confused between these and would appreciate an explanation.
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Its always the Final - Initial... So, products minus reactants
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Two step reactions statrt from 7:05
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