Ch 13 QUIZ - AP Chemistry

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Ch 13 QUIZ - AP Chemistry

Name:_______________________________ Date:_________________ Hr:____AP CHEMISTRYCh 13Chemical EquilibriumQUIZ_____ 3. Given the equilibrium, A 2 (g) + 4 C(g) ↔ 2 AC 2 (g), K 1 = 4.8. It follows that, for thereaction, AC 2 (g) ↔ ½ A 2 (g) + 2 C(g), K 2 = ?a.b. 2.4c. d. √_____ 4. The HOCl(aq) produced in a solution of NaOCl can react further to produce smallamounts of chlorine, Cl 2 (aq), in water according to the equation:HOCl(aq) + H + (aq) + Cl - (aq) ↔ Cl 2 (aq) + H 2 O(l)Which of the following, when added to this system at equilibrium, would decrease theconcentration of Cl 2 in the solution?a. NaClb. NaOHc. H 2 SO 4d. HOCl_____ 5. Methanol can be produced in a reaction between carbon monoxide and hydrogenaccording to the following equation:CO(g) + 2 H 2 (g) ↔ CH 3 OH(g)∆H = -90 kJWhich one of the following changes would occur when a catalyst is added to an equilibriummixture of carbon monoxide, hydrogen, and methanol?a. The value of ∆H would increase.b. The amount of methanol would increase.c. The temperature of the surroundings would increase.d. The rates of both the forward and reverse reaction would increase.2014Page 2 of 8


Name:_______________________________ Date:_________________ Hr:____AP CHEMISTRYCh 13Chemical EquilibriumQUIZ8. (4 points) Ethyl acetate is synthesized in a non-reacting solvent according to the reactionbelow. All four liquids are soluble in this non-reacting solvent.CH 3 COOH + C 2 H 5 OH ↔ CH 3 CO 2 C 2 H 5 + H 2 O K c = 2.2acetic acid ethanol ethyl acetate water duh!For which of the following sets of conditions (a-d) is the system at equilibrium? For those thatare not at equilibrium, in which direction will the system shift? Justify each response.[CH 3 COOH] [C 2 H 5 OH] [CH 3 CO 2 C 2 H 5 ] [H 2 O]a. 0.010 0.010 0.22 0.10b. 0.020 0.10 0.22 0.0020c. 0.044 6.0 0.080 0.12d. 0.88 10.0 4.4 4.42014Page 5 of 8


Name:_______________________________ Date:_________________ Hr:____AP CHEMISTRYCh 13Chemical EquilibriumQUIZ9. (10 points) What will happen to the number of moles of SO 3 (increases, decreases, stays thesame) in equilibrium with SO 2 and O 2 in each of the following cases for the reaction given?Justify each response using Le Châtelier’s principle, but do not simply quote it as a substitutefor a proper chemical explanation.2 SO 3 (g) ↔ 2 SO 2 (g) + O 2 (g) ∆H 0 = +197 kJa. Oxygen gas is added.b. The volume of the reaction container is decreased.c. Argon gas is added.d. The temperature is decreased.e. Gaseous sulfur dioxide is removed.2014Page 6 of 8


Name:_______________________________ Date:_________________ Hr:____AP CHEMISTRYCh 13Chemical EquilibriumQUIZ10. (9 points) Nitric oxide and bromine at initial partial pressures of 98.4 and 41.3 torr,respectively, were allowed to react at 300. K. At equilibrium the total pressure was 110.5 torr.The reactions is:2 NO(g) + Br 2 (g) ↔ 2 NOBr(g)a. Calculate the value of K p .b. What would be the equilibrium partial pressures of NO and Br 2 , if both gases wereinjected into an evacuated flask such that NO and Br 2 each have an initial partialpressure of 220. torr? The equilibrium partial pressure of NOBr is known to be 181.8torr.2014Page 7 of 8


Name:_______________________________ Date:_________________ Hr:____AP CHEMISTRYCh 13Chemical EquilibriumQUIZ11. (9 points) At 125 o C, K p = 0.25 (when pressures were measured in atmospheres) for thereaction:2 NaHCO 3 (s) ↔ Na 2 CO 3 (s) + CO 2 (g) + H 2 O(g)A 1.00-L flask containing 10.0 g of NaHCO 3 is evacuated and heated to 125 o C.a. Calculate the partial pressures of CO 2 and H 2 O after equilibrium is established.b. Calculate the masses of NaHCO 3 and Na 2 CO 3 present at equilibrium.c. Calculate the minimum container volume necessary for all 10.0 g of the NaHCO 3to decompose at this temperature.I affirm that the work shown on this quiz is entirely my own effort and that no resources other than those specifiedwere used.____________________________________Student Signature2014Page 8 of 8

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