๐ The previous lesson explored the formation of ammonia through a reaction between nitrogen and hydrogen.
โ๏ธ The system reaches equilibrium when the rate becomes constant.
๐ Changing the concentration of nitrogen disrupts the equilibrium, causing the system to react and restore equilibrium.
๐ The forward reaction is favored over the reverse reaction due to the consumption of nitrogen and hydrogen.
โฌ๏ธ The amount of ammonia increases as the forward reaction is favored, indicating the system reaching equilibrium.
๐ The rate graph shows that the forward reaction spikes upwards and settles at a higher level, while the reverse reaction remains relatively unchanged.
๐ Increasing pressure, concentration, or temperature speeds up the reaction.
๐ Decreasing pressure, concentration, or temperature slows down the reaction.
๐๐ Changes in concentration directly affect the reaction rate.
๐งช 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).
โณ When analyzing the rate graph, it is observed that the overall rate decreases when the concentration, pressure, or temperature is reduced.
๐ 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.
๐ In the equilibrium graph for concentration, decreasing the concentration favors the reverse reaction and slows down the forward reaction.
๐ 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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