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Exam-2-E

# Exam-2-E - Fall 2010 CHEMISTRY 104 Section 001 Exam 2 Name...

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Fall 2010 CHEMISTRY 104 Section 001 Exam 2 Name: ______________________ ID: XXX-XX-_ ______ Seat #: ___ 1. At 500.0 K, one mole of gaseous ONCl is placed in a one-liter container. At equilibrium it is 5.1 % dissociated according to the equation shown here: 2ONCl 2NO + Cl 2 . Determine the equilibrium constant. A) 7.4 × 10 -5 B) 1.4 × 10 -3 C) 5.4 × 10 -2 D) 9.5 × 10 -1 E) 1.4 × 10 4 2. Given the equation The equilibrium constant is about 0.0215 at 115°C. Calculate K p . 3. At -80°C, K for the reaction is 4.66 10 -8 . We introduce 0.042 mole of N 2 O 4 into a 1.0-L vessel at -80°C and let equilibrium be established. The total pressure in the system at equilibrium will be: Page 1

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4. The reaction has K p = 45.9 at 763 K. A particular equilibrium mixture at that temperature contains gaseous HI at a partial pressure of 4.00 atm and hydrogen gas at a partial pressure of 0.273 atm. What is the partial pressure of I 2 ? 5. Consider the reaction: CaCl 2 (s) + 2H 2 O(g) CaCl 2 ·2H 2 O(s) The equilibrium constant for the reaction as written is A) K = B) C) D) K = [H 2 O] 2 E) K = 6. For the reaction given below, 2.00 moles of A and 3.00 moles of B are placed in a 6.00-L container. At equilibrium, the concentration of A is 0.219 mol/L. What is the value of K ? Page 2

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Exam-2-E - Fall 2010 CHEMISTRY 104 Section 001 Exam 2 Name...

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