le Chatelier's Principle says that this equilibrium will shift (in the forward or reverse direction) to overcome any change made to the system. For example, if more reagent is added, the equilibrium shifts in the forward direction to decrease this amount of reagent. As a consequence, more product is made. The "aim" is to re-establish dynamic equilibrium.
Friday 28 June 2013
Dynamic Equilibrium and le Chatelier's Principle
A dynamic equilibrium is a reaction which is reversible and the rate of reaction in the forward direction is the same as the rate of reaction in the reverse direction.
le Chatelier's Principle says that this equilibrium will shift (in the forward or reverse direction) to overcome any change made to the system. For example, if more reagent is added, the equilibrium shifts in the forward direction to decrease this amount of reagent. As a consequence, more product is made. The "aim" is to re-establish dynamic equilibrium.
le Chatelier's Principle says that this equilibrium will shift (in the forward or reverse direction) to overcome any change made to the system. For example, if more reagent is added, the equilibrium shifts in the forward direction to decrease this amount of reagent. As a consequence, more product is made. The "aim" is to re-establish dynamic equilibrium.
Tuesday 11 June 2013
Bond Enthalpies
pp143-144 Beginning Chemistry
This is also a pretty good website which could help: http://www.kentchemistry.com/links/Kinetics/BondEnergy.htm
Monday 10 June 2013
Friday 7 June 2013
Endothermic vs. Exothermic
Today, we did four simple experiments to see that some reactions absorb heat energy (feel cold) while others release heat energy (feel warm/hot).
- NaOH + water = increase in temperature (exothermic)
- Ammonium chloride + water = decrease in temperature (endothermic)
- HCl + NaOH solutions = increase in temperature
- Ammonium thiocyanate + barium hydroxide = decrease in temperature
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