🔑 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.
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