Today’s Objective LO 6.5 The student can, given data (tabular, graphical, etc.) from which the state of a system at equilibrium can be obtained, calculate.

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Presentation transcript:

Today’s Objective LO 6.5 The student can, given data (tabular, graphical, etc.) from which the state of a system at equilibrium can be obtained, calculate the equilibrium constant, K.

Using the equilibrium constant For the next several weeks, you will be using ICE tables and K expressions in tandem. In some problems, you’ll have enough information to complete the ICE table. You will then be able to solve for K. In other problems, you’ll use the numeric value of K to find the appropriate value for completing the ICE table.

Ex. 1: 2 NH3(g) N2(g) + 3 H2(g) At a certain temperature, 4.0 mol NH3 is introduced into a 2.0 L container and the NH3 partially dissociates. At equilibrium, 2.0 mol NH3 remains. What is the value of Kc for the reaction?

Ex. 2: S8(g) 4 S2(g) A sample of S8(g) is placed in an empty rigid container at 1325 K at an initial pressure of 1.00 atm, where it decomposes to S2 (g). Determine the value of Kp if the partial pressure of S8 at equilibrium is 0.25 atm.

Ex. 3: 0.017 mol of n-butane is placed in a 0.50 L container and allowed to come to equilibrium with its isomer isobutane. KC at 250C is 2.5. What are the equilibrium concentrations of the two isomers?

Ex. 4: SO2(g) + NO2(g) SO3(g) + NO(g) At a certain temperature, Kc = 3.75. Determine the equilibrium concentrations if the initial concentration of both SO3 and NO is 0.800 M.