{"id":6720,"date":"2020-12-14T16:11:21","date_gmt":"2020-12-14T16:11:21","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/?post_type=chapter&p=6720"},"modified":"2020-12-14T16:11:21","modified_gmt":"2020-12-14T16:11:21","slug":"assignment-equilibrium","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/chapter\/assignment-equilibrium\/","title":{"raw":"Assignment: Equilibrium","rendered":"Assignment: Equilibrium"},"content":{"raw":"
    \r\n \t
  1. For each of the following reactions, determine whether the value of the equilibrium constant favors the formation of reactants, products, or both sides equally.<\/li>\r\n<\/ol>\r\na) Br2<\/sub>(g) + Cl<\/span>2<\/sub>(g)\u00a0 \u2194\u00a02 BrCl(g)\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 \u00a0\u00a0\u00a0\u00a0\u00a0 K<\/span>eq<\/sub> = 3 x 10<\/span>6<\/sup>\r\n\r\nb) H2<\/sub>(g) + Br2<\/sub>(g) \u2194\u00a0<\/span>\u00a02 HBr(g)\u00a0\u00a0\u00a0\u00a0\u00a0 \u00a0\u00a0\u00a0\u00a0\u00a0 Keq<\/sub> = 1.15\r\n\r\nc) I2<\/sub>(g) \u2194\u00a0<\/span>\u00a0I(g) + I(g)\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 \u00a0\u00a0\u00a0\u00a0\u00a0 Keq<\/sub> = 4.5 x 10-7<\/sup>\r\n\r\n \r\n\r\n2. Molecular chlorine decomposes into atoms according to the reaction:\r\n\r\n \r\n\r\nCl2<\/sub> (g)\u2194\u00a0<\/span> \u00a02 Cl (g)\r\n\r\n \r\n\r\nThe equilibrium constant for the reaction at 25\u00b0C is 1.4 x 10-38<\/sup>.\u00a0 Would many chlorine atoms be present at this temperature?\u00a0 Explain how you can determine this.\r\n\r\n3. For the following reaction at equilibrium at 2000\u00b0C, the concentration of N2 and O2 are both 4.8 M.\r\n\r\n \r\n\r\nN2<\/sub>(g) + O2<\/sub>(g) \u2194\u00a0<\/span>\u00a02 NO(g)\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 Keq<\/sub> = 6.3 x 10-4<\/sup>\r\n\r\n \r\n\r\nCalculate the concentration of NO at equilibrium. Show your work; pay careful attention to exponents.\r\n\r\n4. CaCO3<\/sub> (chalk) can produce solid CaO and CO2<\/sub> gas when heated. If 6.0 moles of carbon dioxide forms in a 4.500 L reaction vessel, what is the equilibrium constant for this reaction?\r\n\r\n5.\u00a0 Le Chatelier's Principle states that if a stress is applied to a reversible reaction at equilibrium, the reaction will undergo a shift in order to re-establish its equilibrium. Consider the following exothermic reversible reaction at equilibrium:\r\n2 A \u2194B + C\r\nIn which direction (left or right) would the following stresses cause the system to shift?\r\na. decrease the concentration of A\r\nb. increase the concentration of B\r\nc. lower the temperature\r\n\r\n6.\u00a0Chemical engineers use Le Chat\u00ealier\u2019s principle to predict shifts in chemical system at equilibrium resulting from changes in reaction conditions. Predict<\/strong> the changes needed to maximize the yield of product in each of the following industrial chemical systems:\r\n
      \r\n \t
    1. a) the production of ethene (ethylene)<\/li>\r\n<\/ol>\r\nC2<\/sub>H6<\/sub>(g) + energy \u2194C2<\/sub>H4<\/sub>(g) + H2<\/sub>(g)\r\n
        \r\n \t
      1. b) the production of methanol<\/li>\r\n<\/ol>\r\nCO(g) + 2H2<\/sub>(g) \u2194 CH3<\/sub>OH(g) + energy\r\n\r\n \r\n
          \r\n \t
        1. Acetic acid, HC2<\/sub>H3<\/sub>O2<\/sub>, is in equilibrium with its ions:<\/li>\r\n<\/ol>\r\nHC2<\/sub>H3<\/sub>O2<\/sub>(aq) \u2194\u00a0H+(aq) + C2<\/sub>H3<\/sub>O2<\/sub>-<\/sup>(aq)\u00a0\u00a0\u00a0\u00a0 Keq = 1.8 x 10-5<\/sup>\r\n\r\nAt equilibrium, the concentration of the ions are:\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 [H+] = 1.33 x 10-3<\/sup> M\r\n\r\n[C2<\/sub>H3<\/sub>O2<\/sub>-<\/sup>] = 1.33 x10-3<\/sup> M\r\n\r\nCalculate the concentration of the acid, HC2<\/sub>H3<\/sub>O2<\/sub>.\r\n\r\n \r\n\r\n8.Sulfuric acid is the most common commercial acid, with millions of tons produced each year. The second step in the production involves the oxidation of sulfur dioxide gas catalyzed with V2<\/sub>O5<\/sub>(s),\r\n\r\n2SO2<\/sub>(g) + O2<\/sub>(g) \u21942 SO3<\/sub>(g)\u00a0\u00a0\u00a0\u00a0\u00a0 DH<\/em>\u00b0 = -198 kJ\r\n\r\na) Set-up<\/strong> the equilibrium law for this reaction.\r\n\r\nb) List<\/strong> three stresses that could shift the equilibrium to the products side of the reaction.\r\n\r\nc) If the equilibrium constant, K<\/em>eq<\/sub>, for the above reaction at a given temperature is 4 x 103<\/sup>, what is the constant (Keq<\/sub><\/em>) for the reverse reaction (the decomposition of sulfur trioxide)?\r\n\r\n \r\n\r\n \r\n\r\n \r\n\r\n ","rendered":"
            \n
          1. For each of the following reactions, determine whether the value of the equilibrium constant favors the formation of reactants, products, or both sides equally.<\/li>\n<\/ol>\n

            a) Br2<\/sub>(g) + Cl<\/span>2<\/sub>(g)\u00a0 \u2194\u00a02 BrCl(g)\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 \u00a0\u00a0\u00a0\u00a0\u00a0 K<\/span>eq<\/sub> = 3 x 10<\/span>6<\/sup><\/p>\n

            b) H2<\/sub>(g) + Br2<\/sub>(g) \u2194\u00a0<\/span>\u00a02 HBr(g)\u00a0\u00a0\u00a0\u00a0\u00a0 \u00a0\u00a0\u00a0\u00a0\u00a0 Keq<\/sub> = 1.15<\/p>\n

            c) I2<\/sub>(g) \u2194\u00a0<\/span>\u00a0I(g) + I(g)\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 \u00a0\u00a0\u00a0\u00a0\u00a0 Keq<\/sub> = 4.5 x 10-7<\/sup><\/p>\n

             <\/p>\n

            2. Molecular chlorine decomposes into atoms according to the reaction:<\/p>\n

             <\/p>\n

            Cl2<\/sub> (g)\u2194\u00a0<\/span> \u00a02 Cl (g)<\/p>\n

             <\/p>\n

            The equilibrium constant for the reaction at 25\u00b0C is 1.4 x 10-38<\/sup>.\u00a0 Would many chlorine atoms be present at this temperature?\u00a0 Explain how you can determine this.<\/p>\n

            3. For the following reaction at equilibrium at 2000\u00b0C, the concentration of N2 and O2 are both 4.8 M.<\/p>\n

             <\/p>\n

            N2<\/sub>(g) + O2<\/sub>(g) \u2194\u00a0<\/span>\u00a02 NO(g)\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 Keq<\/sub> = 6.3 x 10-4<\/sup><\/p>\n

             <\/p>\n

            Calculate the concentration of NO at equilibrium. Show your work; pay careful attention to exponents.<\/p>\n

            4. CaCO3<\/sub> (chalk) can produce solid CaO and CO2<\/sub> gas when heated. If 6.0 moles of carbon dioxide forms in a 4.500 L reaction vessel, what is the equilibrium constant for this reaction?<\/p>\n

            5.\u00a0 Le Chatelier’s Principle states that if a stress is applied to a reversible reaction at equilibrium, the reaction will undergo a shift in order to re-establish its equilibrium. Consider the following exothermic reversible reaction at equilibrium:
            \n2 A \u2194B + C
            \nIn which direction (left or right) would the following stresses cause the system to shift?
            \na. decrease the concentration of A
            \nb. increase the concentration of B
            \nc. lower the temperature<\/p>\n

            6.\u00a0Chemical engineers use Le Chat\u00ealier\u2019s principle to predict shifts in chemical system at equilibrium resulting from changes in reaction conditions. Predict<\/strong> the changes needed to maximize the yield of product in each of the following industrial chemical systems:<\/p>\n

              \n
            1. a) the production of ethene (ethylene)<\/li>\n<\/ol>\n

              C2<\/sub>H6<\/sub>(g) + energy \u2194C2<\/sub>H4<\/sub>(g) + H2<\/sub>(g)<\/p>\n

                \n
              1. b) the production of methanol<\/li>\n<\/ol>\n

                CO(g) + 2H2<\/sub>(g) \u2194 CH3<\/sub>OH(g) + energy<\/p>\n

                 <\/p>\n

                  \n
                1. Acetic acid, HC2<\/sub>H3<\/sub>O2<\/sub>, is in equilibrium with its ions:<\/li>\n<\/ol>\n

                  HC2<\/sub>H3<\/sub>O2<\/sub>(aq) \u2194\u00a0H+(aq) + C2<\/sub>H3<\/sub>O2<\/sub>–<\/sup>(aq)\u00a0\u00a0\u00a0\u00a0 Keq = 1.8 x 10-5<\/sup><\/p>\n

                  At equilibrium, the concentration of the ions are:\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 [H+] = 1.33 x 10-3<\/sup> M<\/p>\n

                  [C2<\/sub>H3<\/sub>O2<\/sub>–<\/sup>] = 1.33 x10-3<\/sup> M<\/p>\n

                  Calculate the concentration of the acid, HC2<\/sub>H3<\/sub>O2<\/sub>.<\/p>\n

                   <\/p>\n

                  8.Sulfuric acid is the most common commercial acid, with millions of tons produced each year. The second step in the production involves the oxidation of sulfur dioxide gas catalyzed with V2<\/sub>O5<\/sub>(s),<\/p>\n

                  2SO2<\/sub>(g) + O2<\/sub>(g) \u21942 SO3<\/sub>(g)\u00a0\u00a0\u00a0\u00a0\u00a0 DH<\/em>\u00b0 = -198 kJ<\/p>\n

                  a) Set-up<\/strong> the equilibrium law for this reaction.<\/p>\n

                  b) List<\/strong> three stresses that could shift the equilibrium to the products side of the reaction.<\/p>\n

                  c) If the equilibrium constant, K<\/em>eq<\/sub>, for the above reaction at a given temperature is 4 x 103<\/sup>, what is the constant (Keq<\/sub><\/em>) for the reverse reaction (the decomposition of sulfur trioxide)?<\/p>\n

                   <\/p>\n

                   <\/p>\n

                   <\/p>\n

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