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Chemical equilibrium

Chemical equilibrium. Lab goes on p. 126-129 Start this on p. 130!!!!!!. Forward and reverse reactions. Both the forward and reverse reactions have a reaction rate. Chemical equilibrium is reached when the rates of the forward and reverse reactions are equal. Le Chatelier’s Principle.

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Chemical equilibrium

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  1. Chemical equilibrium Lab goes on p. 126-129 Start this on p. 130!!!!!!

  2. Forward and reverse reactions • Both the forward and reverse reactions have a reaction rate. • Chemical equilibrium is reached when the rates of the forward and reverse reactions are equal.

  3. Le Chatelier’s Principle • We can disrupt a reaction’s equilibrium by changing parts of the reaction or the conditions of the reaction. (change temperature, add reactants, add products, etc.) • When we do this, the reaction has to make up for the difference, so it “shifts” the equilibrium to make up for the change.

  4. Effect of changing concentrationA + B  C + D

  5. Examples • For the following equations, predict the direction that the equilibrium will shift based on the change made to the reactants and products. • CH4 + 2O2  CO2 + H2O • Add CH4 – • Remove O2 – • Remove CO2 – • Add H2O –

  6. Effect of changing temperature N2 + 3H2  2NH3 + 92 kJ • Exothermic reactions (heat is a product)

  7. Endothermic reactions: heat is a reactant CaCO3 + 556 kJ  CaO + CO2

  8. Review • For the following equation, decide which direction the EQ will shift based on the change made. N2O4 + heat  2NO2 add N2O4 = add NO2 = decrease temp =

  9. Change in Pressure • Changes in pressure only affect gases (g) • Remember from EL 7 that pressure and volume are inversely related, so they are opposites.

  10. Examples P4(s) + 6Cl2(g)  4PCl3(l) add P4 = remove PCl3 = increase pressure = increase volume = add Cl2 =

  11. 4NH3(g) + 5 O2 (g)  4NO(g) + 6H2O (g) remove NH3 = increase volume = increase pressure = add O2 = add NO = remove H2O =

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