Practice Exam 1

# Practice Exam 1 - CHM 2046 Gower Sections Exam 1...

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CHM 2046 Gower Sections Exam 1 ANSWERS (Form Code A) Fall 2009 Notes and Potentially Useful Data : The double-arrow symbol used in this exam ( ↔) refers to a reversible reaction K w = 1.0 x 10 –14 R = 0.0821 lit•atm/mol•K 1. The equilibrium constant K p for the given reaction is 0.13 at 830ºC. In one experiment 2.00 mol SO 2 and 2.00 mol O 2 were initially present in a flask. What must the total pressure at equilibrium be in order to have an 65.0 percent yield of SO 3 ? 2SO 2(g) + O 2(g) 2SO 3(g) (1) 65.8 atm (2) 132 atm (3) 263 atm (4) 328 atm (5) 526 atm 2. The following equilibrium constants were determined at 1123 K: C (s) + CO 2(g) 2CO (g) K p = 1.3 x 10 14 CO (g) + Cl 2(g) COCl 2(g) K p = 6.0 x 10 –3 Calculate the equilibrium constant K p at 1123 K for the following reaction. C (s) + CO 2(g) + 2Cl 2(g) 2COCl 2(g) (1) 7.8 x 10 11 (2) 1.3 x 10 14 (3) 4.7 x 10 9 (4) 2.2 x 10 16 (5) 7.3 x 10 17 3. Consider the equilibrium 2NOBr (g) 2NO (g) + Br 2(g) If NOBr is 34 percent dissociated at 25ºC and the total pressure is 0.25 atm, calculate K c for the reaction at this temperature. (1) 1.8 x 10 –3 (2) 9.3 x 10 –3 (3) 4.5 x 10 –2 (4) 8.5 x 10 –2 (5) 3.8 x 10 –4 4. Consider the following equilibrium in a closed container. C (s) + CO 2(g) 2CO (g) What would happen if the volume of the container was halved? (1) reaction shifts to the right and more CO is produced; K p decreases (2) reaction shifts to the right and more CO is produced; K p increases (3) reaction shifts to the right and more CO is produced; K p does not change (4) reaction shifts to the left and more CO

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Practice Exam 1 - CHM 2046 Gower Sections Exam 1...

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