Question 1: Le Chatelier's Principle states that if a system at equilibrium experiences a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore equilibrium. How does this principle help us understand changes in atmospheric carbon dioxide levels?

Answer: It explains how the equilibrium between carbon dioxide absorption and release by oceans and other systems adjusts in response to changes such as increased CO2 levels, helping to regulate or amplify climate effects.

Question 1: Define Le Chatelier's Principle in your own words.

Answer: It is the principle that states a system at equilibrium will shift to counteract any imposed change, thereby restoring a new equilibrium.

Question 2: Which factors can cause a shift in chemical equilibrium? List at least three.

Answer: Changes in concentration, temperature, pressure, or the presence of a catalyst.

Question 1: The equilibrium constant (K) for the reaction CO2 + H2O ⇌ H2CO3 in ocean water is 1.4 × 10^-3 at 25°C. If the concentration of CO2 is increased from 0.03 mol/L to 0.06 mol/L, what is the expected shift in the equilibrium? Show your calculations.

Answer: As the concentration of CO2 increases, according to Le Chatelier's Principle, the system shifts to produce more H2CO3. The increased CO2 favors the formation of carbonic acid, shifting the equilibrium to the right.

Question 1: Design a simple experiment to demonstrate how increasing temperature affects the equilibrium of the reaction N2 + 3H2 ⇌ 2NH3 (ammonia synthesis). Include variables to control and safety precautions.

Answer: Students should suggest controlling temperature, pressure, and reactant concentrations, using proper protective gear, working in a well-ventilated area, and following lab safety guidelines. The experiment involves heating the reactants and observing changes in ammonia production.

Question 1: In a certain ocean region, the pH drops from 8.2 to 7.8 over a decade. Explain how Le Chatelier's Principle relates to this change and its effect on the carbonate equilibrium in seawater.

Answer: A decrease in pH indicates increased acidity, shifting the carbonate equilibrium to favor CO2 and bicarbonate ions, reducing carbonate ions essential for marine life. Le Chatelier's Principle explains how increased CO2 causes the equilibrium to shift, impacting ocean health.

Question 1: Explain how increasing atmospheric CO2 levels can lead to ocean acidification, using Le Chatelier's Principle to support your answer. (6 marks)

Answer: Increased atmospheric CO2 dissolves into oceans, raising CO2 concentration in seawater. According to Le Chatelier's Principle, this shifts the carbonate system equilibrium towards producing more carbonic acid, which lowers pH and causes ocean acidification. This process disrupts marine ecosystems dependent on stable carbonate levels.

Question 1: Describe how understanding Le Chatelier's Principle can help scientists develop methods to reduce ocean acidification caused by climate change.

Answer: Scientists can manipulate conditions such as reducing CO2 emissions, increasing alkalinity in seawater, or developing carbon capture technologies to shift equilibria and mitigate acidification effects, based on Le Chatelier's Principle.