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1 Name: Name: Name: Name: Worksheet 10: Q, Adding Equations, Equilibrium Calculations, and Le Châtelier Objectives: To be able to calculate Q, the reaction quotient, and know what it means. To be able to combine equilibrium equations to get a new equation, manipulating the K s to get the new K. To be able to perform equilibrium calculations using an I.C.E. table when necessary. To be able to use Le Châtelier s principle to determine which way an equilibrium will shift when it is disturbed. Reaction Quotient Q: Q is calculated exactly like K, but when the system is not necessarily at equilibrium. If Q < K the system will shift towards the right (product side) so as to achieve equilibrium. If Q > K the system will shift towards the left (reactant side) so as to achieve equilibrium. If Q = K the system is at equilibrium. Adding Equations: What adding equilibrium equations multiply their K s. When reversing an equation take the reciprocal of it s K. When multiplying an equation through by some number raise it s K to that power. Equilibrium Calculations: When solving an equation it is sometimes useful to neglect the unknown (x) compared to a number that it is being added to or subtracted from. We use the rule of thumb that it is a valid approximation if the value of the unknown (x) is less than about 5% of the number it was neglected with respect to. Le Châtelier: When a species is removed from an equilibrium the equilibrium will shift towards the side of the species that was removed. When a species is added to an equilibrium the equilibrium will shift away from the side the species was added to. When thermal energy is added to an equilibrium the equilibrium will shift towards the right (products) if it is an endothermic reaction and towards the left (reactants) if it is an exothermic reaction. If there gaseous species involved in a reaction and the volume is decreased (pressure increased) at constant temperature the equilibrium will shift towards the side with fewer gaseous species. If there gaseous species involved in a reaction and the volume is increased (pressure decreased) at constant temperature the equilibrium will shift towards the side with more gaseous species. Page 1 of 6
2 1.) For the following reaction K = 1.79 at 225 o C. If moles of PCl 5 is placed into a 1.75 L container at 225 o C, what will the equilibrium concentrations of all species present? [PCl 5 ] equil = M [PCl 3 ] equil = M [Cl 2 ] equil = M 2.) N 2 O 4 (g) and NO 2 (g) are mixed together in a rigid container. The following reaction occurs: The total pressure at equilibrium is 1.88 atm. Calculate the partial pressures of dinitrogen tetroxide and nitrogen dioxide at equilibrium. = atm = atm Page 2 of 6
3 3.) Answer the following questions based on the reaction: a.) What will happen if the volume is increased at constant temperature? b.) CaO is added to the mixture. c.) Some CaCO 3 is removed from the mixture. d.) Some CO 2 is added to the mixture. e.) A drop of HCl(aq) is added to the mixture. Write a balanced chemical equation describing what happens. f.) A drop of NaOH(aq) is added to the mixture. Write a balanced chemical equation describing what happens. Page 3 of 6
4 4.) Answer the following questions based on this reaction: a.) How will the equilibrium shift if water is added, doubling the volume? b.) How will the equilibrium shift if AgNO 3 (aq) is added (AgSCN is insoluble)? c.) How will the equilibrium shift if NaOH(aq) is added (Fe(OH) 3 is insoluble)? d.) How will the equilibrium shift if Fe(NO 3 ) 3 (aq) is added? 5.) K = for the following reaction at 25 o C. Calculate the reaction quotient Q if 2.04 g of H 2 O, 3.14 g Cl 2 O, and 2.77 g of HOCl are place in a 150. ml container. Is the system at equilibrium? If not, which way will it shift to achieve equilibrium? Q = Equilibrium? Direction? Page 4 of 6
5 6.) At one temperature K = 4.54 x 10 4 for the following reaction. Calculate the concentrations of FeSCN 2+, Fe 3+, and SCN at equilibrium if the solution is initially 1.59 M FeSCN 2+. [FeSCN 2+ ] = M [Fe 3+ ] = M [SCN ] = M Page 5 of 6
6 7.) At a certain temperature K = 1.59 x 10 5 for the following decomposition reaction: If 60.0 grams of NO and 70.9 grams of Cl 2 are placed into a 250. ml flask, calculate the equilibrium concentrations of NOCl, Cl 2, and NO. [NOCl] = M [Cl 2 ] = M [NO] = M Page 6 of 6
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