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 initial QC value calculated for the reaction involving hydrogen iodide?

• 3.1

• 49

• 4.5

• 0.5

In the reaction involving hydrogen iodide, what needs to happen for QC to equal KC?

• Decrease hydrogen iodide concentration

• Increase hydrogen concentration

• Increase hydrogen iodide concentration

• Decrease iodine concentration

What is the KC value for Haber's process as mentioned in the video?

• 3.1

• 4.5

• 0.5

• 49

In Haber's process, what needs to happen to the concentration of ammonia to reach equilibrium?

• It should be increased

• It should be decreased

• It should remain constant

• It should be doubled

What is the QC value calculated for Haber's process?

• 0.5

• 4.5

• 3.1

• 49