Write the equilibrium constant expressions for Kc and for Kp. determne acide base

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Write the equilibrium constant expressions for Kc and for Kp. determne acide base

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CHEM 135 chapter 15 homework (chemical equilibrium) 1. Write the equilibrium constant expressions for Kc and for Kp for these reactions: a. 2NO2(g) +7H2(g) → 2NH3(g) + 4H2O(l) b. 2ZnS(s) + 3O2(g) → 2ZnO(s) + 2SO2(g) c. C(s) + CO2(g) → 2CO(g) d. C6H5COOH(aq) → C6H5COO- (aq) + H+(aq) 2. Given the following reaction: 2H2(g) + S2(g) → 2H2S(g) Calculate Kc for the reaction if there are 2.50 moles H2 , 1.35 x 10-5 moles S2 , and 8.70 moles H2S in a 12.0 liter flask at equilibrium. 3. A reaction vessel contains 0.25 M NH3, 0.11 M N2, and 1.91 M H2 at equilibrium. Calculate Kc for the following reactions: a. N2(g) + 3H2(g) → 2NH3(g) b. ½ N2(g) + 3/2 H2(g) → NH3(g) 4. The pressure of the carbon dioxide in the following reaction mixture is 0.105 atm at 350 oC. CaCO3(s) → CaO(s) + CO2(g) Calculate Kp and Kc for the reaction. 5. Phosgene gas (COCL2), 3.00 x 10-2 mol, was placed in a 1.50 L container. It was heated to 800. K. At equilibrium the pressure of CO was found to be 0.497 atm. Calculate the equilibrium constant Kp for this reaction. COCl2(g) → Cl2(g) + CO(g) 6. Define reaction quotient. How does it differ from equilibrium constant? 7. A sample of NO2 gas heated to 1000 K decomposes: 2NO2 (g) → 2NO(g) + O2(g) The equilibrium constant Kp is 158. Analysis shows that the partial pressure of O2 is 0.25 atm at equilibrium. Calculate the partial pressure of NO and NO2 at equilibrium. 8. The dissociation of molecular iodine into iodine atoms is represented as I2(g) → 2I(g) Kc = 3.80 x 10-5 at 1000. K Suppose you start with 0.0456 moles of I2 in a 2.30 L flask. What are the concentrations of each of the gases at equilibrium? 9. Consider this equilibrium process at 686 oC: CO2(g) + H2(g) → CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.050M, [H2] = 0.045M, [CO2] = 0.086M, and [H2O] = 0.040M. a. Calculate Kc for the reaction at 686 oC. b. If the concentration of CO2 were raised to 0.50 mol/L by the addition of CO2, what will be the concentrations of each the gases when equilibrium is reestablished? 10. List 4 factors that can shift the position of an equilibrium. Which one can alter the value of the equilibrium constant? 11. Consider the equilibrium reaction: SO2(g) + Cl2(g) → SO2Cl2(g) H = +2.1 kJ/mol Predict how the equilibrium would change if; a. Cl2 was added to the system b. SO2Cl2 was removed from the system c. SO2 was removed from the system d. Heat was added to the system 12. What effects does an increase of pressure have on each of these systems at equilibrium? a. A(s) -> 2B(s) b. 2A(l) → B(l) c. A(s) → B(g) d. A(g) → B(g) e. A(g) → 2B(g) 13. Consider the reaction: 2SO2(g) + O2(g) → 2SO3(g) H = -198.2 kJ/mol Comment on the which way the equilibrium would shift if we were to: a: increase the temperature b: decrease the volume of the container c: add SO2 to the container d: add a catalyst e: add helium to the container (at constant volume) 14. What are the names and formulas of the conjugate bases of these acids? a. HNO2 b. H2SO4 c. H2S d. HCN e. HCOOH (formic acid) 15. Identify the acid-base conjugate pairs in each of these reactions. (Put an A under each acid and a B under each base.) a. CH3COO- + HCN → CH3COOH + CN- b. HCO3- + HCO3- → H2CO3 + CO32- c. H2PO4- + NH3 → HPO42- + NH4+ d. HClO + CH3NH2 → ClO- + CH3NH3+ e. CO32- + H2O → HCO3- + OH- f. CH3COO- + H2O → CH3COOH + OH- 16. Calculate the hydrogen ion concentration in moles per liter for each of these solutions. a. A solution whose pH is 5.20. b. A solution whose pH is 16.00 c. A solution whose hydroxide concentration is 3.7 x 10-9. 17. Calculate the pH of water at 40oC, given that the Kw is 3.8 x 10-14 at this temperature. 18. Complete this table for a solution. pH [H+] Solution is
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