**LE CHATELIER’S PRINCIPLE** Le Chatelier’s Principle states that when a system at equilibrium is subjected to a stress, the system will shift its equilibrium point in order to relieve the stress. Complete the following chart by writing left, right, or none for equilibrium shift, and decreases, increases, or remains the same for the concentrations of reactants and products, and for the value of K. **12.6 kcal + H₂(g) + I₂(g) ⇄ 2HI(g)** | Stress | Equilibrium Shift | [H₂] | [I₂] | [HI] | K_eq | |-------------------------|-------------------|-------------|----------------|-----------|------------------| | 1. Add H₂ | right | ___ | decreases | increases | Remains the same | | 2. Add I₂ | | | | | | | 3. Add HI | | | | | | | 4. Remove H₂ | | ___ | | | | | 5. Remove I₂ | | | ___ | | | | 6. Remove HI | | | | ___ | | | 7. Increase Temperature | | | | | | | 8. Decrease Temperature | | | | | | | 9. Increase Pressure | | | | | | | 10. Decrease Pressure | | | | | |

2. Consider the following equilibrium. Which way will the system shift, if at all? How would the following changes affect the partial pressures of each gas at the new equilibrium, if at all? How will the equilibrium constant change, if at all?

Write the chemical equation for the dissolving of lithium sulfate and use it to determine the equilibrium expression (Ksp) for the dissolving lithium sulfate

O KINETICS AND EQUILIBRIUM Calculating an equilibrium constant from a partial equilibrium... 0/5 Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 75.0 L tank with 21. mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 6.3 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = 0 II