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CH302 Chapter 6 Notes part 3

# CH302 Chapter 6 Notes part 3 - CH302 Chapter 6 notes part 3...

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CH302 Chapter 6 notes part 3 Equilibrium Calculations We are now ready for the tricky stuff! Two main types: 1. Given K and initial concentrations, find equilibrium concentrations. 2. Given initial concentrations and one of the equilibrium concentrations, find K BOTH involve setting up ICE tables (Initial, Change, Equilibrium) What follows are several examples to be done in class. We had to get to this point to be able to 'put it all together' Use of K c to find Equilibrium Concentrations (1) K c = 3.00 for the following reaction at a given temperature. If 1.00 mole of SO 2 and 1.00 mole of NO 2 are put into an evacuated 2.00 L container and allowed to reach equilibrium, what will be the concentration of each compound at equilibrium? We set up an ICE table. I have included the one for this first example to help you. M M M M M M M M M M M M ___ ____ _____ ____ m Equilibriu ___ + ___ + ___ - __ - Change ___ ___ ____ ___ Initial NO SO NO SO (g) 3(g) 2(g) 2(g) + + Use of K c to find Equilibrium Concentrations (2) K = 49 for the following reaction at 450 o C. If 1.00 mole of HI is put into an evacuated 1.00-liter container and allowed to reach equilibrium, what will be the equilibrium concentration of each substance? Calculating an Equilibrium Constant (1) One mole of PCl 5 was introduced into an evacuated 1.00 liter container at some temperature. The system was allowed to reach equilibrium. At equilibrium 0.60 mole of PCl 3 was present in the container. Calculate K at this temperature. Calculating an Equilibrium Constant (2) At a given temperature 0.80 mole of N 2 and 0.90 mole of H 2 were placed in an evacuated 1.00-liter container. At equilibrium 0.20 mole of NH 3 was present. Calculate K c .

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CH302 Chapter 6 Notes part 3 - CH302 Chapter 6 notes part 3...

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