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Lecture 41/28/05
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Quiz 2 1. Given the following reaction: 2 H 2 S (g) ↔ 2 H 2 (g) + S 2 (g) Calculate K c and K p at 1400 K if at equilibrium a flask contains 1 M H 2 S, 0.06 M H 2, and 0.06 M S 2.
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For the reaction: CO (g) + H 2 O (g) ↔ CO 2 (g) + H 2 (g) If a reaction vessel at 673 K is charged with an equimolar mixture of CO and steam such that P CO =P H2O =2.00 atm. What are the partial pressures at equilibrium? K p = 10 at 673 K
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For the reaction: CO (g) + H 2 O (g) ↔ CO 2 (g) + H 2 (g) If a reaction vessel at 673 K is charged with an equimolar mixture of CO and steam such that P CO =P H2O =2.00 atm and H 2 is added so that P H2 =0.15 atm. What are the partial pressures at equilibrium? K p = 10 at 673 K
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Le Chatelier’s Principle If a system is at equilibrium and is disturbed, it will shift the equilibrium to counteract the disturbance. Ways to disturb equilibrium: Add or remove product or reactant Change the pressure or volume Change the temperature Consider Q vs. K
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Add or Remove Product or reactant Add a substance and system will shift to reduce it Remove substance and system will try and replenish it
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Haber Process N 2 (g) + 3 H 2 (g) ⇄ 2 NH 3 (g)
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Volume or pressure change Reducing volume shifts system to lower number of moles (affects partial pressure) Increasing volume shifts system to increase number of moles (affects partial pressure) If you increase total pressure without increasing partial pressures (by adding an inert gas), then it does
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