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1. What is chemical equilibrium ?
2. What are the characteristics of equilibrium?
3. What is the ICE method ?
4. What is the Haber process ?
5. What is the law of mass action ?
6. Describe what it is to have strong intermolecular force?
7. What is Le Chatellier's principle?
8. What are the factors that affect principle ?
9. What is the contact process?
10. Explain Vapor pressure.

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How The Haber Process Works (Le Chatelier's Principle)

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This video covers physical and chemical equilibrium. This video is suitable for both the old and new chemistry syllabus. 7.1.1 Outline the characteristics of chemical and physical systems in a state of equilibrium.

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Understanding Chemical Equilibrium and Equilibrium Constant Kc

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Learn the basics of chemical equilibrium and help yourself study for chemistry tests on equilibrium. Skip to 0:40 to learn how to find if a system is at equilibrium. Skip to 1:20 to learn how to calculate the value of K. Though we try to accurately teach this information, we are still human.

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They tend to have lower enthalpy of vaporization , higher vapor pressure, lower boiling point

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They have higher enthalpy of vaporization , lower vapor pressure , and higher boiling point

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Vapor Pressure- is the pressure exerted by the particles in the vapor phase on it's liquid at equilibrium.

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Vapor Pressure- is the pressure exerted by the particles in the vapor phase on it's liquid at equilibrium.

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Contact process - production of sulfuric acid 

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Contact process - production of sulfuric acid 

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Haber process- is the production of ammonia. 

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Haber process- is the production of ammonia. 

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Pressure-As pressure goes down it shift towards larger numbers of moles of gas. As pressure goes down it shift towards smaller numbers of moles of gas

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Pressure-As pressure goes down it shift towards larger numbers of moles of gas. As pressure goes down it shift towards smaller numbers of moles of gas

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Temperature- As temperature goes up it shift towards the endothermic side (right) and as it goes down it shift towards the exothermic side (left)

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Temperature- As temperature goes up it shift towards the endothermic side (right) and as it goes down it shift towards the exothermic side (left)

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Concentration- if you add reactants then it will shift to the right , if you remove reactants then it will shift to the left. If you add products it will shift to the left , if you remove products they shift to the right.

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Concentration- if you add reactants then it will shift to the right , if you remove reactants then it will shift to the left. If you add products it will shift to the left , if you remove products they shift to the right.

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Le Chatelier's principle-  When a change ( stress) is applied to a system at equilibrium , the system will shift its equilibrium position to counteract the effect of the disturbance.

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Le Chatelier's principle-  When a change ( stress) is applied to a system at equilibrium , the system will shift its equilibrium position to counteract the effect of the disturbance.

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ICE Method- The initial change in equilibrium which is used for solving equilibrium problems ( where the equilibrium concentration in unknown) is affectionately referred to as the ICE method.

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ICE Method- The initial change in equilibrium which is used for solving equilibrium problems ( where the equilibrium concentration in unknown) is affectionately referred to as the ICE method.

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Equilibrium Expression-  Kc or Keq . It is a measure to extent to which a reaction occurs ; it varies with temperature ( and the only with temp) and is unitless.

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Equilibrium Expression-  Kc or Keq . It is a measure to extent to which a reaction occurs ; it varies with temperature ( and the only with temp) and is unitless.

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aA + bB <-> cC + dD at equilibrium

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E. Directional - The same equilibrium mixture will result under the same conditions , no matter whether the reaction is started with all reactants ,all products, or a mixture of both.  

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E. Directional - The same equilibrium mixture will result under the same conditions , no matter whether the reaction is started with all reactants ,all products, or a mixture of both.  

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D. Macroscopic- Observable properties such as color and density; these do not change as they depend on the concentrations of the components in the mixture.

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D. Macroscopic- Observable properties such as color and density; these do not change as they depend on the concentrations of the components in the mixture.

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c. Concentration- They are being produced and destroyed at an equal rate

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c. Concentration- They are being produced and destroyed at an equal rate

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B. Closed System -prevents exchange of matter with surroundings , so equilibrium is achieved where both reactants and products can react and recombine with each other 

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B. Closed System -prevents exchange of matter with surroundings , so equilibrium is achieved where both reactants and products can react and recombine with each other 

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A. Dynamic - The reaction has not stopped ; the forward and backward reactions are still occurring ( same rate)

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exists when the forward &' reverse rxns/ processes occur at exactly the same rate