17.1 Introduction to Dynamic Equilibrium (Video)
- Page ID
- 342552
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Video Topics
Two opposing processes taking place at equal rates. Some reactions are reversible For the reaction: N2(g) + 3 H2(g) - 2 NH3(g) We must now consider that the reverse reaction is also taking place: 2 NH3(g) - N2(g) + 3 H2(g) As we mix N2 and H2 the forward reaction occurs but as NH3 is formed the reverse reaction starts to occur. With time the forward reaction starts to slow due to decreasing concentration of N2 and H2 and the reverse reaction speeds up due to the increasing concentration of NH3. When the rates of the two reactions equal each other dynamic equilibrium occurs. This fact is expressed as: Kc = {NH3}2 = 3.6 x 108 @ 298 K {N2}{H2}3 This ratio is called the equilibrium constant expression and it is equal to a number, which is constant for the reaction (Kc). Some consequences 1) Once DE is reached the amounts of reactants and products remain the same. 2) In no case is any of the reacting species completely consumed. The equilibrium concentration of N2(g) was found to be 1.0 x 10-4.
Link to Video
Introduction to Dynamic Equilibrium: https://youtu.be/4AJbFuzW2cs
Attribution
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Prof. Steven Farmer (Sonoma State University)