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The Equilibrium Constant Part II

In this segment, students find out if their calculation for the equilibrium constant of ammonia was correct. The teacher asks the students to list examples that illustrate why chemical equilibrium is important in everyday life.

In this segment, students find out if their calculation for the equilibrium constant of ammonia was correct. The teacher asks the students to list examples that illustrate why chemical equilibrium is important in everyday life.

Premiere Date: August 16, 2016 | Runtime: 00:04:00

Support Materials

Toolkit

Unit 10C Note Taking Guide & Segment Questions
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Unit 10C Practice Problems 1- Calculating the Equilibrium Constant
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Crosscutting Concepts

Patterns

Observed patterns of forms and events guide organization and classification, and they prompt questions about relationships and the factors that influence them.

Vocabulary

chemical equilibrium - a state that is reached when the rate of the forward reaction equals the rate of the reverse reaction.

dynamic equilibrium - a state of equilibrium in which two opposing processes occur simultaneously with no net change. 

equilibrium - a condition in which all acting influences are canceled by others, resulting in a stable, balanced, or unchanging system. 

equilibrium constant (ksubeq) - the ratio of the concentration of products divided by the concentration of reactants. 

Le Chatelier's Principle - a principle that states that when the equilibrium of a system is disturbed or stressed, the system adjusts to reestablish equilibrium by minimizing or countering the stress.

static equilibrum - a state of equilibrium in which no movement occurs. 

The Haber Process - the process of synthesizing ammonia from nitrogen and hydrogen gases.

 

Georgia Standards of Excellence

SC4Obtain, evaluate, and communicate information about how to refine the design of a chemical system by applying engineering principles to manipulate the factors that affect a chemical reaction.

SC4.aPlan and carry out an investigation to provide evidence of the effects of changing concentration, temperature, and pressure on chemical reactions. (Clarification statement: Pressure should not be tested experimentally.)

SC4.bConstruct an argument using collision theory and transition state theory to explain the role of activation energy in chemical reactions. (Clarification statement: Reaction coordinate diagrams could be used to visualize graphically changes in energy (direction flow and quantity) during the progress of a chemical reaction.)

SC4.dRefine the design of a chemical system by altering the conditions that would change forward and reverse rates and the amount of products at equilibrium. (Clarification statement: Emphasis is on the application of LeChatelier’s principle.)

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