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ICE Tables

ICE Tables. I nitial (Concentrations) C hange E quilibrium (Concentrations).

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ICE Tables

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  1. ICE Tables Initial (Concentrations) Change Equilibrium (Concentrations)

  2. A mixture of 2.00 moles of H2(g) and 2.00 moles of I2(g) is placed in a 2.00 L container held at a constant temperature. After equilibrium is reached, 3.12 moles of HI(g) are found in the container. Calculate Kc for the reaction. H2(g) + I2(g) 2 HI(g)

  3. 0.850M cis-stilbene is placed in a closed container. Calculate the equilibrium concentrations of cis- and trans- stilbene, given the equilibrium constant below. cis-stilbenetrans-stilbene Kc = 24.0

  4. 2.0 mol of N2O4 and 4.0 mol NO2 are placed in a 2.0L container at 637K. Given the Kc value below, calculate the equilibrium concentrations of N2O4 and NO2. N2O4(g) 2NO2(g) Kc = 40.

  5. In air at 25C and 1.00 atm, [N2(g)] = 0.033M and [O2 (g)] = 0.00810 M. Taking the nitrogen and oxygen concentrations as initial values, calculate the equilibrium concentration of nitrogen monoxide that would exist in our atmosphere at 25C. N2(g) + O2(g) 2 NO(g) K= 4.8 x 10–31

  6. A reaction mixture initially contains PI2= 0.150 atm and PCl2 = 0.150 atm and PICl= 0.100 atm. Find the equilibrium partial pressures of all three substances. I2(g) + Cl2(g) 2ICl Kp = 81.9

  7. Kc and Kp 3H2(g) + N2(g) 2NH3(g) Kc = Kp= Kc (RT)Δn(gas) How would the value of Kp compare to that of Kc for the reaction above? Kp =

  8. Kc and Kp How would the value of Kp compare to that of Kc for the following reaction: CaCO3(s)CaO(s) + CO2(g)

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