Equilibrium Constants and Reactions

The video tutorial explains equilibrium constants, their expressions, and factors affecting them. It covers how to write equilibrium constant expressions, the role of stoichiometric coefficients, and the impact of temperature on equilibrium. Examples of different equilibrium systems are provided, highlighting the importance of gases and solutions in these expressions. The tutorial concludes with a summary and encourages further exploration of industrial equilibrium processes.

What does a larger equilibrium constant (Kc) indicate about the position of equilibrium?

• More reactants than products

• More products than reactants

• Equal amounts of reactants and products

• No reaction occurs

Which of the following is NOT included in an equilibrium constant expression?

• Concentrations

• Solids

• Aqueous solutions

• Gases

How are stoichiometric coefficients used in equilibrium constant expressions?

• They are added to the concentrations

• They are subtracted from the concentrations

• They are ignored

• They are used as exponents for the concentrations

In the reaction N2 + 3H2 ⇌ 2NH3, how is the equilibrium constant expression written?

• [NH3]^2 / ([N2][H2]^3)

• [N2][H2]^3 / [NH3]^2

• [NH3] / ([N2][H2])

• [N2][H2] / [NH3]

Why is carbon not included in the equilibrium constant expression for a reaction where it is a solid?

• Its concentration is constant

• It is not reactive

• It is a catalyst

• Its concentration changes

What happens to the equilibrium constant if the temperature of an exothermic reaction is increased?

• It increases

• It decreases

• It remains the same

• It becomes zero

According to Le Chatelier's principle, what happens when more reactants are added to a system at equilibrium?

• The system shifts to produce more reactants

• The equilibrium constant changes

• The system shifts to produce more products

• The reaction stops

Which factor is the only one that can change the value of the equilibrium constant?

• Pressure

• Volume

• Concentration

• Temperature

If Kc is less than 1, what does this indicate about the reaction at equilibrium?

• Equal amounts of reactants and products

• More products than reactants

• More reactants than products

• No reaction occurs

What should you focus on when interpreting the size of Kc in an exam?

• Memorizing reaction equations

• Calculating exact values

• Understanding the position of equilibrium

• Predicting reaction rates