IB chemistry

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Rate of reaction is dependent on the concentration of reactants. So the forward reaction starts fast but slows as the reaction gets less concentrated.

In an equilibrium reaction not all reactants become products.

NEED TO INCLUDE FORWARD AND REVERSE ARROWS IN EQUATIONS

Equilibrium can only happen at the following conditions:

  1. Closed system – none of the products or reactants can escape the system
  2. Constant temperature – T does not change throughout the reaction
  3. Constant pressure (for gases) 
  4. No change in macroscopic properties – color, pH, concentration…

Reactants and products in the same phase = homogeneous

Reactants and products in different phases= heterogeneous

only temperature affects the magnitude of the equilibrium constant. Pressure would not affect KC, but would be able to shift the equilibrium. 

If the KC is much larger than 1, the reaction goes almost to completion because the concentration of products must be higher than the concentration of reactants. If the KC is much smaller than 1, the reaction hardly proceeds because the concentration of reactants is much higher than the concentration

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