# Drill – 5/28 1. Write the equilibrium expression for sulfuric acid.

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Drill – 5/28 1. Write the equilibrium expression for sulfuric acid

Drill – 5/31/11 In the reaction Heat + 2CO(g) + O 2 (g) ↔ 2CO 2 (g) Which way would equilibrium shift: a.If [CO] increases b.If temperature decreases c.If CO 2 is removed

Le Châtelier’s Principle

If a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress. Stress is anything that upsets equilibrium – concentration, pressure, or temperature.

Concentration Measure of molarity (moles/L) If you ↑ concentration of a reactant, equilibrium will shift toward the products. If you ↓ concentration of a reactant, equilibrium will shift toward the reactants.

CO(g) + 3H 2 (g) ↔ CH 4 (g) + H 2 O(g) CO(g) H 2 O(g)

Pressure PV=nRTIdeal Gas Law: PV=nRT If ↑ P then ↑ n, which means more number of atoms. If ↑ P, then the equilibrium will shift toward the side with fewer moles of gas.

CO(g) + 3H 2 (g) ↔ CH 4 (g) + H 2 O(g) 4 moles of gas 2 moles of gas Note: If moles of gaseous reactant = moles of gaseous product, then no shift in equilibrium will occur from a change in pressure

Temperature Think of heat as a reactant or a product. CO(g) + 3H 2 (g) ↔ CH 4 (g) + H 2 O(g) + heat Is this Exothermic or Endothermic?

heat CO(g) + 3H 2 (g) ↔ CH 4 (g) + H 2 O(g) + heat

Le Châtelier’s Principle If a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress. – Concentration – Pressure – Temperature Note: Only temperature affects K. The larger the value of K, the more product at equilibrium.

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