Watch all ten videos and complete each quiz to earn your certificate.

 

 Links to help with video quizzes:

• Interactive Periodic Table (The Royal Society of Chemistry)
• Desmos: Free Online Scientific Calculator

Chemical reactions don’t always go to completion. Reversible reactions are reactions that can “go in both directions.” Reactants can form products, and under the right conditions, products can reform reactants. The Haber-Bosch process is used to illustrate the concept of reversible reactions.

 

After watching this video, CLICK HERE for Quiz 1: Reversible Reactions & Equilibrium. 

What’s going on in a reversible reaction? Over the course of a chemical reaction, we hit a point where the rate of reactants forming products equals the rate at which products are reforming the reactants. This is called the Equilibrium point of a reaction.

 

After watching this video, CLICK HERE for Quiz 2: What is Equilibrium? 

What happens if conditions change when a reaction reaches equilibrium? When a change is made to the surroundings of a chemical reaction, the equilibrium will shift (or adjust) to compensate for that change until a new equilibrium is established. Throughout this video, examples of shifts and how they affect the equilibrium of a reaction are discussed.

 

After watching this video, CLICK HERE for Quiz 3: Shifts in Equilibrium. 

In a reversible reaction, increasing amounts of reactants or products can cause a shift in equilibrium. Additionally, due to the “Common Ion Effect,” increasing ions that are part of a reversible reaction can also cause an equilibrium shift.

 

After watching this video, CLICK HERE for Quiz 4: Le Châtelier-like Shifts. 

Solving for the equilibrium constant, Keq, involves dividing the concentrations of products of a chemical reaction by the concentrations of reactants. Most often, we find that equilibrium reactions are either occurring in solution or involve reactions occurring with gases.

 

After watching this video, CLICK HERE for Quiz 5: Equilibrium constant, Keq. 

Under the conditions of a given chemical reaction, the ratio of products to reactants are used to calculate the equilibrium constant of that reaction. The value of the calculated constant will reveal whether the reaction favors a shift toward the products or toward the reactants.

 

After watching this video, CLICK HERE for Quiz 6: Keq Calculations. 

A known Keq value allows for the calculation of the amounts of both reactants and products that will be present when a reaction reaches equilibrium. RICE tables: reaction, initial amount, change, equilibrium amount; (often referred to as ICE tables), are a useful organization tool for calculating amounts at equilibrium.

 

After watching this video, CLICK HERE for Quiz 7: RICE Tables. 

When equilibrium reactions involve pressure, the equilibrium constant ‘Kp’ is used. Examples for calculating Kp are presented in this video.

 

After watching this video, CLICK HERE for Quiz 8: Equilibrium constant, Kp. 

The reaction quotient, Q, helps determine which side of a reversible reaction (reactants or products) is being favored under given conditions. Knowing the value of Q is helpful when setting up the RICE table (ICE table). Examples for comparing Q and Keq values are presented in this video.

 

After watching this video, CLICK HERE for Quiz 9: Reaction Quotient, Q. 

The product concentrations of the reversible reaction will be used to calculate the equilibrium constant, Ksp. A real-world example related to both Ksp and the common ion effect is used for the example calculations presented in this video.

 

After watching this video, CLICK HERE for Quiz 10: Solubility Product Constant, Ksp. 

After you watch all 10 videos and take the quizzes, CLICK HERE for the Understanding Equilibrium Certificate.

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