Question

Consider the following system at equilibrium at 698 K: 2 HI (g) ⇌ H₂ (g) + I₂ (g). Indicate whether each individual change would favor the production of H₂ (g). Evaluate each change separately, assuming that all other conditions remain constant.

1) Increasing the temperature
2) Increasing the pressure
3) Increasing the volume
4) Adding HI
5) Removing I₂

Answer 1

When considering a system at equilibrium, increasing the temperature favors the production of H₂ (g), increasing the pressure favors the production of HI (g), increasing the volume favors the production of H₂ (g), adding HI favors the production of H₂ (g), and removing I₂ favors the production of HI (g).

Step-by-step explanation:

When considering a system at equilibrium, there are certain changes that can favor the production of one of the products, H₂ (g). Let's evaluate each change separately:

1. Increasing the temperature: Increasing the temperature of the reaction will shift the equilibrium to the left, favoring the production of H₂ (g) and reducing the concentration of HI (g) and I₂ (g).
2. Increasing the pressure: Since the reaction involves gases, increasing the pressure will favor the production of the side with fewer moles of gas. In this case, H₂ (g) and I₂ (g) each have 1 mole of gas, while HI (g) has 2 moles. Therefore, increasing the pressure will favor the production of HI (g).
3. Increasing the volume: Increasing the volume will have the opposite effect of increasing the pressure. It will favor the production of the side with more moles of gas. Therefore, increasing the volume will favor the production of H₂ (g).
4. Adding HI: If HI is added to the system, the equilibrium will shift to the left to consume the added HI and favor the production of H₂ (g) and I₂ (g).
5. Removing I₂: If I₂ is removed from the system, the equilibrium will shift to the right to compensate for the loss and favor the production of HI (g) and reduce the concentration of H₂ (g).