For the equilibrium reaction: H2(g) + I2(g) ⇌ 2HI(g), what is the effect of adding more HI?
Practice Questions
1 question
Q1
For the equilibrium reaction: H2(g) + I2(g) ⇌ 2HI(g), what is the effect of adding more HI?
Shifts to the right
Shifts to the left
No change
Increases the rate of reaction
Adding more HI increases the concentration of products, which shifts the equilibrium to the left to form more reactants.
Questions & Step-by-step Solutions
1 item
Q
Q: For the equilibrium reaction: H2(g) + I2(g) ⇌ 2HI(g), what is the effect of adding more HI?
Solution: Adding more HI increases the concentration of products, which shifts the equilibrium to the left to form more reactants.
Steps: 6
Step 1: Identify the reaction: H2(g) + I2(g) ⇌ 2HI(g).
Step 2: Understand that H2 and I2 are reactants, and HI is the product.
Step 3: Recognize that adding more HI increases the amount of product in the reaction.
Step 4: Apply Le Chatelier's principle, which states that if a change is made to a system at equilibrium, the system will adjust to counteract that change.
Step 5: Since we added more HI (the product), the system will try to reduce the concentration of HI.
Step 6: To reduce HI, the equilibrium will shift to the left, favoring the formation of more reactants (H2 and I2).
