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Solving Equilibrium problems using the RICE method

Solving Equilibrium problems using the RICE method. General Method. Write the balanced equation for the reaction. Write the equilibrium expression using the law of mass action. List the initial concentrations. Calculate Q to determine the shift to equilibrium.

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Solving Equilibrium problems using the RICE method

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  1. Solving Equilibrium problems using the RICE method

  2. General Method • Write the balanced equation for the reaction. • Write the equilibrium expression using the law of mass action. • List the initial concentrations. • Calculate Q to determine the shift to equilibrium. • Define the change needed to reach equilibrium. • Substitute equilibrium concentrations and solve for the unknown.

  3. Solving for Equilibrium Concentration Consider this reaction at some temperature: H2O(g) + CO(g)  H2(g) + CO2(g) K = 2.0 Assume you start with 8 molecules of H2O and 6 molecules of CO. How many molecules of H2O, CO, H2, and CO2 are present at equilibrium? Here, we learn about “ICE” – the most important problem solving technique in the second semester. You will use it for the next 4 chapters!

  4. Solving for Equilibrium Concentration H2O(g) + CO(g)  H2(g) + CO2(g) K = 2.0 Step #1: We write the law of mass action for the reaction:

  5. Solving for Equilibrium Concentration Step #2: We “ICE” the problem, beginning with the Initial concentrations H2O(g) + CO(g)  H2(g) + CO2(g) 8 6 0 0 -x -x +x +x 8-x 6-x x x

  6. Solving for Equilibrium Concentration Step #3: We plug equilibrium concentrations into our equilibrium expression, and solve for x H2O(g) + CO(g)  H2(g) + CO2(g)

  7. Solving for Equilibrium Concentration Step #4: Substitute x into our equilibrium concentrations to find the actual concentrations H2O(g) + CO(g)  H2(g) + CO2(g)

  8. At a particular temperature, Kp = 0.25for the reactionN2O4 2NO2 • A flask containing only N2O4 at an initial pressure of 4.5 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases.

  9. At a particular temperature, Kp = 0.25for the reactionN2O4 2NO2 • A flask containing only NO2 at an initial pressure of 9.0 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases.

  10. Carbon monoxide reacts with steam to produce carbon dioxide and hydrogen. At 700 K, the equilibrium constant is 5.10. Calculate the equilibrium concentrations of all species if 3.00 mol of each component is mixed in 2.000 L flask.CO (g) + H2O (g)  CO2 (g) + H2 (g)

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