Equilibrium Expressions and Constants

The video tutorial covers writing and using equilibrium expressions, focusing on both concentration and pressure equilibrium expressions. It explains how to calculate equilibrium constants and interpret their values, including the effects of reversing reactions and changing stoichiometric coefficients.

What is the primary focus when writing a concentration equilibrium expression?

• Ignoring stoichiometric coefficients

• Including solids and liquids

• Using partial pressures of gases

• Using molarities of solutions

When writing a pressure equilibrium expression, which notation is used?

• Volume notation

• Molarity notation

• Partial pressure notation

• Square bracket notation

Why are liquids and solids excluded from equilibrium expressions?

• They are not part of the reaction

• They have no pressure or molarity

• They are always reactants

• They are always products

In a pressure equilibrium expression, what is the role of stoichiometric coefficients?

• They are used as exponents

• They are used as coefficients

• They are used as subscripts

• They are ignored

What is the first step in calculating an equilibrium constant?

• Calculating the reaction rate

• Writing the equilibrium expression

• Determining the reaction order

• Measuring the temperature

What does a small equilibrium constant (K) indicate about a reaction?

• The reaction is at equilibrium

• The reaction is spontaneous

• The reaction favors reactants

• The reaction favors products

What is the significance of a K value less than 0.01?

• The reaction favors reactants

• The reaction favors products

• The reaction is at equilibrium

• The reaction is fast

If a reaction is reversed, what happens to the equilibrium constant?

• It is halved

• It remains the same

• It is inverted

• It doubles

How does changing the stoichiometric coefficients affect the equilibrium constant?

• It lowers the constant

• It has no effect

• It inverts the constant

• It raises the constant to the power of the change

What happens to the equilibrium constant if the reaction direction is swapped?

• It doubles

• It remains unchanged

• It becomes zero

• It is inverted