Equilibrium Written Response
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1 Equilibrium Written Response January Consider the following equilibrium: CS2 (g) + 3Cl2 (g) CCl4 (g) + S2Cl2 (g) H = -238 kj a) Sketch a potential energy diagram for the reaction above and label H. (2 marks) b) Some CS2 is added and equilibrium is then reestablished. State the direction of the equilibrium shift and the resulting change in [Cl2] (1 mark) c)the temperature is decreased and equilibrium is then reestablished. What will the effect be on the value of Keq? (1 mark) April State Le Chatelier s Principle. (2 marks)
2 3. Consider the following equilibrium: H2 (g) + I2 (g) 2HI (g) K eq = 7.1 X 10 2 At equilibrium, the [H 2] = 0.012mol/L and [HI] = 0.40 mol/l. What is the equilibrium concentration of I2? (2 marks) June Consider the following graph for the reaction: energy + N2O4 (g) 2NO2 (g) a) What is the stress imposed at time t1? (1 mark) b) What is the stress imposed at time t3? (1 mark) c) Calculate Keq for the equilibrium between t2 and t3. (2 marks)
3 August Consider the following equilibrium: H2 (g) + I2 (g) 2HI (g) K eq = 49 A 1.00 L container is initially filled with mol HI. Calculate the concentration of HI at equilibrium. January Consider the following diagram for a chemical system containing three substances represented by A, B and C: a) What feature of the graph indicates that the system reaches equilibrium? (1 mark) b) Write a balanced equation for the equilibrium reaction. (2 marks)
4 c) Calculate K eq at equilibrium. (2 marks) April Describe how enthalpy and entropy change, in the forward direction, as an exothermic reaction reaches equilibrium. Explain your reasoning. (2 marks) 3. Consider the graph below representing the following equilibrium: CH3CH2CH2CH3 (g) n-butane CH3CH(CH3)2 (g) isobutene Data for the graph was obtained from various equilibrium mixtures. Calculate the value of K eq for the equilibrium. (2 marks)
5 June Consider the following equilibrium system: N2 (g) + 3H2 (g) 2NH3 (g) + energy A 1.00 L container is filled with 5.0 mol NH3 and the system proceeds to equilibrium as indicated by the graph. a) Draw and label the graph for N2 and H2. (2 marks) b) Calculate the K eq for N2 (g) + 3H2 (g) 2NH3 (g) + energy (2 marks) 3. State Le Chatelier s Principle. (2 marks)
6 August Consider the following equilibrium: 4HCl ( g) + O2 (g) 2H2O (g) + 2Cl2 (g) + energy a) How does the entropy change in the forward direction? Explain your reasoning. (1 mark) b) How does the enthalpy change in the forward direction? Explain your reasoning. (1 mark) 3. Consider the following equilibrium: H2 (g) + I2 (g) 2HI ( g) Keq =1.2 x 10 2 A 2.0 L flask is filled with 0.10 mol HI. Calculate the concentration of H2 at equilibrium. (3 marks) January Consider the following equilibrium: HInd + H2O H3O + + Ind (yellow) (blue) The system is yellow and turns blue on the addition of NaOH. In terms of the forward and reverse reaction rates, explain why this shift occurs. (2 marks) 4. Consider the following equilibrium: Fe 3+ (aq) + SCN - (aq) FeSCN 2+ (aq) Initially, 50.0mL of 0.10M Fe 3+ is added to 30.0mL of 0.20M SCN - At equilibrium, the concentration of FeSCN 2+ is found to be 0.050M. Calculate the Keq for the reaction. (4 marks)
7 April Methanol, CH3OH, is produced industrially by the following reaction: CO(g) + 2H2(g) CH3OH(g) + heat a) State two different methods of shifting the equilibrium to the right. (1 mark) b) In terms of rates, explain why these methods cause the equilibrium to shift to the right. (1 mark) 4. Consider the following equilibrium: H2(g) + I2(g) 2HI(g) A 2.0L container is filled with mol of H2 and mol of I2. Equilibrium is reached after 15.0 minutes at which time there is mol of HI present. Sketch and label the graphs for the changes in concentrations of H2, I2 and HI for the time period of 0 to 30.0 minutes. (3 marks)
8 June Consider the observations for the following equilibrium: N 2 O 4(g) (colourless) 2NO 2(g) (brown) a) Sketch the potential energy curve on the graph below for this equilibrium. (1 mark) b) Explain the colour change using Le Chatelier s Principle. (1 mark) c) Other than changing temperature, what could be done to cause a shift to the left? (1 mark)
9 3. Consider the data obtained for the following equilibrium: Fe 3+ (aq) + SCN - (aq) FeSCN 2+ (aq) Calculate the [FeSCN 2+ ] in experiment #2. (3 marks) August Consider the following reaction: Fe 3+ (aq) + SCN - (aq) FeSCN 2+ (aq) (yellow) (colourless) (red) When a few drops of 6.0M NaOH is added to 25.0mL of the above system, a precipitate of Fe(OH)3 forms and the solution turns pale yellow. a) Explain this colour change in terms of Le Chatelier s Principle. (2 marks) b) Describe the effect on the rate of the reverse reaction as the color change occurs. (1 mark) 3. Consider the following equilibrium: 3I2 (g) + 3F2 (g) 2IF2(g) + I4F2 (g) Initially, 2.00 X 10-1 mol of I2 and 3.00 X 10-1 mol of F2 and put into a 10.00L flask. At equilibrium, [I4F2] is 2.00 X 10-3 M. Calculate the Keq. (4 marks)
10 January Consider the following equilibrium system: 2COF2(g) CO2 (g) + CF4 (g) Keq= 2.00 A 2.00 L container is filled with mol of COF2. Calculate the [COF2] at equilibrium. (5 marks) 3. Consider the following equilibrium system: Cu 2+ (aq) + 4Br - (aq) 2- CuBr 4 (aq) blue colourless green Cooling the equilibrium changes the colour from green to blue. What effect will the decrease in temperature have on K eq? Explain, using Le Chatelier s Principle. (2 marks) April A flask is initially filled with some HI. At equilibrium, the [HI] = 0.80 mol/l. What is the [H2] at equilibrium? (3 marks) 2HI (g) H 2(g) + I 2(g) Keq = Consider the following equilibrium system: 2NOCl (g) 2NO (g) + Cl2 (g) Keq= 1.6 X 10-5 A 1.00 L flask is filled with 0.20mol NOCl, 0.10mol NO and 0.10mol Cl2. State and show by calculation the direction in which the reaction proceeds to reach equilibrium. (4 marks)
11 June Write four statements that apply to all chemical equilibrium systems. (2 marks) 3. Consider the following equilibrium system: H2 (g) + Br2 (g) 2HBr (g) Keq= 14.8 A closed container was initially filled with equal moles of H2 and Br2. When equilibrium is reached, the [HBr]is mol/l. What was the initial [H2]? (4 marks) August Consider the following graph for the reaction: H2 (g) + I2 (g) 2HI (g) The temperature is increased at t1 and equilibrium is re-established at t2. a) On the above graph, sketch the line representing the [HI] between time t1 and t3. (1 mark) b) Calculate the value of Keq after t2. (2 marks)
12 3. Consider the following equilibrium system: 2SO2 (g) + O2(g) 2SO3 (g) A 1.00 L container is initially filled with 0.100mol SO mol O2. At equilibrium the O2 concentration is mol/l. Calculate the value of Keq. (4 marks) Written Response Answers January 1998
13 April June
14 August 1998
15 January
16 April June 1999
17 August Solution a) Entropy is decreasing. Five particles of gas (reactants) have more entropy than four particles of gas (products). (1 mark) b) Enthalpy is decreasing. The reaction is exothermic, so the enthalpy of the products is less than the enthalpy of the reactants. (1 mark) 3.
18 January Solution: Addition of OH- decreases [H3O + ], decreasing the reverse rate. Since the forward rate is greater than the reverse rate, the system shifts to the right. (2 marks) 4. April Solution: a) Any two of the following: (1 mark) ~ adding reactant ~ removing methanol ~ decreasing the temperature ~ increasing the pressure by decreasing the volume b) The shift occurs because rate (f) must be greater than rate (r) as a result of the stress. (1 mark)
19 4. June
20 3. August
21 3. January
22 3. April
23 June 2001
24 August 2001
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Equilibrium Written Response
Equilibrium Written Response January 1998 2. Consider the following equilibrium: CS2 (g) + 3Cl2 (g) CCl4 (g) + S2Cl2 (g) ΔH = -238 kj a) Sketch a potential energy diagram for the reaction above and label
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