CH302 Chapter 6 answers part 1&amp;2

# CH302 Chapter 6 answers part 1&amp;2 - Equilibrium...

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Equilibrium Constant Example 1 Write equilibrium constant expressions for the reaction at 500 o C. All reactants and products are gases at 500 o C. 4NH 3 (g) + 5O 2 (g) l 4NO (g) + 6H 2 O (g) K = [NO] 4 [ H 2 O ] 6 [ NH 3 ] 4 [ O 2 ] 5 Equilibrium Constant eg 2 H 2 (g) + I 2 (g) l 2HI (g) K = [HI] 2 [H 2 ] [I2] Write it multiplied by 4 and show K = [HI] 8 = K orig 4 [H 2 ] 4 [I2] 4 write it reversed and show K = 1/K orig Partial Pressures and the Equilibrium Constant If we express K in partial pressures, we denote it as K p : + , + , + , + , > @ > @ > @ > @ + , + , + , + , 2 O H 2 Cl O 4 HCl p 2 2 2 2 2 4 c g 2 g g 2 g 2 2 2 2 P P P P K and O H Cl O HCl K O + HCl 4 O H 2 + Cl 2 m o DOC Partial Pressures and the Equilibrium Constant + , + , + , + , + , + , + , + , + , + , + , K mol atm L 0.0821 R use Must (RT) K = K or (RT) K = K reaction for this so K K P P P P K 1 c p 1 - p c RT 1 p c 4 RT 1 5 RT 1 2 O H 2 Cl O 4 HCl 2 RT P 2 RT P RT P 4 RT P c 2 2 2 O 2 H 2 Cl 2 O HCl u

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Calculating an Equilibrium Constant (1) One liter of equilibrium mixture from the following system at a high temperature was found to contain 0.172 mole of phosphorus trichloride, 0.086 mole of chlorine, and 0.028
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