For the equilibrium reaction: H2(g) + I2(g) ⇌ 2HI(g), what is the effect of addi
Practice Questions
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
Questions & Step-by-Step Solutions
For the equilibrium reaction: H2(g) + I2(g) ⇌ 2HI(g), what is the effect of adding more I2?
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.
Le Chatelier's Principle – When a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium.
