For the equilibrium reaction: H2(g) + I2(g) ⇌ 2HI(g), what is the effect of adding more I2?
Practice Questions
1 question
Q1
For the equilibrium reaction: H2(g) + I2(g) ⇌ 2HI(g), what is the effect of adding more I2?
Equilibrium shifts to the right
Equilibrium shifts to the left
No effect
Equilibrium constant changes
Adding more I2 increases its concentration, which shifts the equilibrium to the right to produce more HI.
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 I2?
Solution: Adding more I2 increases its concentration, which shifts the equilibrium to the right to produce more HI.
Steps: 7
Step 1: Identify the reaction: H2(g) + I2(g) ⇌ 2HI(g).
Step 2: Understand that this reaction can reach a state of balance called equilibrium.
Step 3: Recognize that equilibrium means the rates of the forward reaction (H2 and I2 forming HI) and the reverse reaction (HI breaking back into H2 and I2) are equal.
Step 4: When you add more I2, you increase the amount of I2 in the reaction.
Step 5: According to Le Chatelier's principle, if you change the concentration of a reactant (like I2), the equilibrium will shift to counteract that change.
Step 6: Since we added more I2, the equilibrium will shift to the right to use up the extra I2.
Step 7: Shifting to the right means more HI will be produced.
