Predicting direction of reaction

The video tutorial explains how to predict the direction of reversible reactions using the example of hydrogen iodide formation. It discusses the concept of equilibrium constant (KC) and reaction quotient (QC), showing how to adjust reactant and product concentrations to achieve equilibrium. The tutorial also covers Haber's process for ammonia production, illustrating how to favor backward reactions by altering concentrations. Key concepts include equilibrium, reaction direction, and concentration adjustments.

What is the equilibrium constant (KC) value for the reaction involving hydrogen iodide formation?

What is the significance of QC being less than KC in the context of the reaction discussed?

Explain how the concentration changes affect the QC and KC values in the reaction of hydrogen iodide formation.

Describe the conditions under which the reaction reaches equilibrium according to the text.

In Haber's process, what changes are required to achieve equilibrium based on the given concentrations?