Equilibrium Graphs Grade 12: Concentration - Exploring System Response

🔑 The previous lesson explored the formation of ammonia through a reaction between nitrogen and hydrogen.

⚖️ The system reaches equilibrium when the rate becomes constant.

🔀 Changing the concentration of nitrogen disrupts the equilibrium, causing the system to react and restore equilibrium.

🔍 The forward reaction is favored over the reverse reaction due to the consumption of nitrogen and hydrogen.

⬆️ The amount of ammonia increases as the forward reaction is favored, indicating the system reaching equilibrium.

🔄 The rate graph shows that the forward reaction spikes upwards and settles at a higher level, while the reverse reaction remains relatively unchanged.

🔑 Increasing pressure, concentration, or temperature speeds up the reaction.

🔄 Decreasing pressure, concentration, or temperature slows down the reaction.

📈📉 Changes in concentration directly affect the reaction rate.

🧪 According to Le Chatelier's principle, decreasing the concentration of hydrogen causes the system to favor the reverse reaction, resulting in an increase in nitrogen and a decrease in ammonia (NH3).

⏳ When analyzing the rate graph, it is observed that the overall rate decreases when the concentration, pressure, or temperature is reduced.

📉 The changes in concentration and rate depicted in the graphs showcase the impact of Le Chatelier's principle on the equilibrium of the chemical reaction.

🔑 In the equilibrium graph for concentration, decreasing the concentration favors the reverse reaction and slows down the forward reaction.

📉 The forward reaction slows down the most when the concentration decreases.

Decreasing a variable affects the equilibrium system the most.

Two different ways to change the equilibrium system.

Graphical representation of the system's reaction to changes in equilibrium.