Reaction Quotient - Predicting Reaction

The video tutorial explains the concept of the reaction quotient (QC) and its role in determining the direction of chemical reactions. QC is similar to the equilibrium constant (KC) but is used when reactions are not at equilibrium. The tutorial covers how to calculate QC using the concentrations of products and reactants, and how to use QC to predict whether a reaction will proceed forward or in reverse. It also discusses the comparison between QC and KC, explaining that if QC is less than KC, the reaction favors the forward direction, while if QC is greater, the reverse reaction is favored. The video concludes with a visual representation of these concepts.

What is the main difference between the reaction quotient (QC) and the equilibrium constant (KC)?

• QC is calculated only at equilibrium.

• QC is calculated when reactions are not at equilibrium.

• KC is only applicable to gaseous reactions.

• KC is used to predict reaction direction.

How does QC help in understanding chemical reactions?

• It measures the pressure of the reaction.

• It indicates whether a reaction is at equilibrium.

• It predicts the speed of the reaction.

• It determines the temperature of the reaction.

What happens when QC is less than KC?

• No net reaction occurs.

• The reverse reaction is favored.

• The forward reaction is favored.

• The reaction is at equilibrium.

If QC equals KC, what can be inferred about the reaction?

• The reaction will proceed in the forward direction.

• The reaction will proceed in the reverse direction.

• The reaction is at equilibrium with no net change.

• The reaction will stop completely.

When QC is greater than KC, which direction is favored?

• Reverse reaction is favored.

• Forward reaction is favored.

• No reaction occurs.

• Both directions are equally favored.