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Chemical Equilibrium: Keq

Chemical Equilibrium: Keq. 2H 2 S(g)  2H 2 (g) + S 2 (g) At 1130 o C the following equilibrium concentrations are as follows: H 2 S = 0.15 M; H 2 = 0.01 M; S 2 = 0.051 M. Calculate K eq. Chemical Equilibrium: Keq. H 2 (g) + I 2 (g)  2HI(g)

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Chemical Equilibrium: Keq

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  1. Chemical Equilibrium: Keq 2H2S(g)  2H2(g) + S2(g) At 1130oC the following equilibrium concentrations are as follows: H2S = 0.15 M; H2 = 0.01 M; S2 = 0.051 M. Calculate Keq.

  2. Chemical Equilibrium: Keq H2(g) + I2(g)  2HI(g) What is the equilibrium concentration of HI for the above reaction given the following information: H2(g) equilibrium conc. = 2.0M; I2(g) equilibrium conc. = 3.0M; Keq=51

  3. Chemical Equilibrium: Keq At 900K, a 4.00 L reaction vessel originally contained 0.55 mols SO3(g). Once equilibrium was reached, 0.12 mols of O2(g) was made. Calculate the Keq given the following equation: 2SO3(g)  2SO2(g) + O2(g)

  4. Chemical Equilibrium: Keq A 1.00 M sample of HI is heated in a sealed container to 510oC. At equilibrium, a 0.14 M concentration of each of the products (H2 & I2) is present. Calculate the Keq.

  5. Chemical Equilibrium: Keq At 500K, a 1.00 L reaction vessel originally contained 0.045 mols NO2(g). Once equilibrium was reached, 0.0020 mols of O2(g) was made. Calculate the Keq given the following equation: 2NO2(g)  2NO(g) + O2(g)

  6. Shifts: Le Chatelier The following system is in equilibrium: Heat + 2NH3(g) N2(g) + 3H2(g) 1. If more N2(g) were added, what effect on the equilibrium would there be? 2. If H2(g) could be selectively removed from the system, what effect would there be on the equilibrium?

  7. Le Chatelier For the system 2 SO2(g) + O2(g)2 SO3(g) , Predict the effect of each of the following changes on the value of the equilibrium constant and on the number of moles of SO3 present in the mixture at equilibrium. (a) Decreasing the volume of the system. (b) Adding oxygen to the equilibrium mixture. (c) Raising the temperature of the system.

  8. Le Chatelier C(s) + H2O(g)  CO(g) + H2(g) Ho = +131 kJ Additional H2(g) is added. The temperature of the system is increased. The volume of the container is decreased. 4. The graphite pellets are pulverized

  9. Solubility Product: Ksp At 25oC, a saturated solution of calcium hydroxide has a concentration of 0.0126 M. Calculate the Ksp.

  10. Solubility Product: Ksp The solubility of calcium sulfate is found to be 0.67 grams per liter of solution. Calculate the Ksp.

  11. Solubility Product: Ksp The Ksp for silver carbonate is 8.1 x 10-12 at 25oC. Calculate the molar solubility of this substance at this temperature.

  12. Solubility Product: Ksp Solid calcium nitrate is added to a 100.0 ml solution of 0.10 M KF until the reaction stops. How many grams of solid CaF2 is produced and what is the molar solubility of the of CaF2 (Ksp = 3.9 x 10-11)

  13. Solubility Product: Ksp At 25oC, the Ksp of silver carbonate, Ag2CO3 is 8.1 x 10-12. Calculate the molar concentrations of silver and carbonate ions at this temperature.

  14. Solubility Product: Ksp a) At 25 degrees the Ksp of magnesium carbonate (MgCO3) is 3.60 X 10-8. Calculate the molar concentration of Magnesium ions present in a saturated solution at this temperature. b) If you were asked to prepare a solution of this substance at this temp. by dissolving 0.240 grams MgCO3 into 10.0 L, would all the solute dissolve? If not, how much (in grams) would be leftundissolved?

  15. Solubility Product: Ksp If 0.01 L of a 0.00825 M solution of Na2SO4 is added to 0.29 L of a 0.00125 M solution of CaCl2, will a CaSO4 precipiate form, and if so how much? The Ksp for CaSO4 = 1.7 x 10-8

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