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Entry Task: Jan 11 th Friday

Entry Task: Jan 11 th Friday. Turn in Equilibrium Lab. Agenda. Discuss any problems with the equilibrium lab Self check on Ch. 15 sec. 1-4 HW: Ch. 15 sec. 5-6 reading notes. Write the equilibrium expression ( K eq ) for the following reactions .

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Entry Task: Jan 11 th Friday

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  1. Entry Task: Jan 11th Friday Turn in Equilibrium Lab

  2. Agenda • Discuss any problems with the equilibrium lab • Self check on Ch. 15 sec. 1-4 • HW: Ch. 15 sec. 5-6 reading notes

  3. Write the equilibrium expression (Keq) for the following reactions. • BaSO4(s)  Ba2+(aq) + SO42-(aq) • 2 Hg(s) + O2(g)  2 HgO(s)

  4. 1) Write the equilibrium expression (Keq) for the following reactions. • 2 NaHCO3(s)  Na2CO3(s) + CO2(g) + H2O(g) • CaCO3(s) + 2 HCl(aq)  CaCl2(aq) + CO2(g) + H2O(l)

  5. For each of the following, you MUST write the Keq expression, substitute in the values, then solve. 2) SO3(g) + H2O(g)  H2SO4(l)At equilibrium, the [SO3] = 0.400 M and the [H2O] = 0.480 M. Calculate the value of the equilibrium constant. Kc= 0.192

  6. For each of the following, you MUST write the Keq expression, substitute in the values, then solve. 3) PCl5(s) + H2O(g)  2 HCl(g) + POCl3(g)A 2.0 L flask at equilibrium at 100oC contains 0.075 mol of PCl5, 0.050 mol of H2O, 0.750 mol of HCl, and 0.500 mol of POCl3. Calculate the Keq for the reaction. Change into molarity 0.050mol/2.0L = 0.025 M H2O 0.075mol/2.0L = 0.0375 M HCl 0.500mol/2.0L = 0.25 M POCl3 Kc= 1.41 x 10-2

  7. For each of the following, you MUST write the Keq expression, substitute in the values, then solve. 4) 2 NO2(g)  N2O4(g). If 2.00 moles of NO2 and 1.60 moles of N2O4 are present in a 4.00 L flask at equilibrium, what is the equilibrium constant? Change into molarity 2.00mol/4.0L = 0.5 M 1.60mol/4.0L = 0.4 M Kc= 1.6

  8. For each of the following, you MUST write the Keq expression, substitute in the values, then solve. 5) H2(g) + I2(g)  2 HI(g).If, at equilibrium, [H2] = 0.200 M and [I2] = 0.200 M, what is the concentration of HI in the 5.0 L flask? Keq = 55.6 at 250oC. Kc= 1.49

  9. For each of the following, you MUST include an ICE table and the Keq expression.   • A reaction vessel had 1.95 M CO and 1.25 M H2O introduced into it. After an hour, equilibrium was reached according to the equation: • CO2(g) + H2(g)  CO(g) + H2O(g) • Analysis showed that 0.85 M of CO2 was present at equilibrium. What is the equilibrium constant for this reaction? CO2 CO H2 H2O  0 M 0 M 1.95M 1.25M 0.85 0.85 -0.85 -0.85 0.85M 0.85M 1.1M 0.4M

  10. CO2 CO H2 H2O  0 M 0 M 1.95M 1.25M 0.85 0.85 -0.85 -0.85 0.85M 0.85M 1.1M 0.4M Use the equilibrium concentrations to find Kc- plug n chug Kc= 0.61

  11. For each of the following, you MUST include an ICE table and the Keq expression.   • 2 SO2(g) + O2(g)  2 SO3(g) • Into a 2.00 L container is placed 1.00 mol of SO2(g) and 1.00 mol of O2(g). At equilibrium, [SO3] = 0.150 M. Calculate the equilibrium constant for this reaction. Change into molarity 1.00mol/2.0L = 0.5 M SO2 1.00mol/2.0L = 0.5 M O2

  12. For each of the following, you MUST include an ICE table and the Keq expression.   • 2 SO2(g) + O2(g)  2 SO3(g) • Into a 2.00 L container is placed 1.00 mol of SO2(g) and 1.00 mol of O2(g). At equilibrium, [SO3] = 0.150 M. Calculate the equilibrium constant for this reaction. SO2 2SO3 O2  0.0M 0.5 M 0.5 M -0.075 -0.075 0.150 0.425M 0.425M 0.150M 1 molO2 2 mol of SO3I 0.150 mol SO3 L = 0.075M Same goes for SO2

  13. SO2 2SO3 O2  0.0M 0.5 M 0.5 M -0.075 -0.075 0.150 0.425M 0.425M 0.150M Use the equilibrium concentrations to find Kc- plug n chug Kc= 12.5

  14. For each of the following, you MUST include an ICE table and the Keq expression.   • 2 NOCl(g)  2 NO(g) + Cl2(g) • When 0.50 mol of NOCl was put into a 1.0 L flask and allowed to reach equilibrium, 0.10 mol of Cl2 was found. What is Keq for this reaction? Change into molarity 0.50mol/1.0L = 0.5 M NOCl 0.10mol/1.0L = 0.1 M Cl2

  15. For each of the following, you MUST include an ICE table and the Keq expression.   • 2 NOCl(g)  2 NO(g) + Cl2(g) • When 0.50 mol of NOCl was put into a 1.0 L flask and allowed to reach equilibrium, 0.10 mol of Cl2 was found. What is Keq for this reaction? NOCl  Cl2 NO 0.0M 0.5 M 0.0 M 0.1 0.1 -0.2 0.30M 0.1M 0.1M 2molNOCl 1 mol of NO 0.1 mol NO L = 0.2

  16. NOCl  Cl2 NO 0.0M 0.5 M 0.0 M 0.1 0.1 -0.2 0.30M 0.1M 0.1M Use the equilibrium concentrations to find Kc- plug n chug Kc= 0.11

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