Chemistry 111 Homework #11 Due: November 30, 2005 (Wednesday) 1. Calculate the numerical value for the equilibrium constant for the following reaction at 298 K: (ΔG°ffor NOCl = + 66.70 kJ/mol). The one for NO is + 86.69 kJ/mol. 2 NO (g) + Cl2 (g)∏2 NOCl (g) a) 1.02 ×10+7b) 2.03 ×10-12c) 1.02 d) 9.82 ×10-8e) 4.92 ×10+11f) None of these. 2. Calculate the numerical value for the equilibrium constant for the following reaction at 298 K. The ΔG°ffor N2O is + 104.18 kJ/mol. The one for NO can be obtained from a previous question. N2O (g) + 1/2O2 (g) ∏2 NO (g) 3. Calculate the numerical value for the equilibrium constant for the reaction below at 298 K. The ΔG°ffor NH4Cl, NH3, and HCl are – 202.87, - 16.45, and – 95.299 kJ/mol, respectively. NH4Cl (s) ∏NH3 (g) + HCl (g) a) 9.40 ×1015b) 1.82 ×10-22c) 1.07 ×10-16d) 2.25 ×10-14e) 1.00 f) None of these. 4. Determine the equilibrium constant (Kp) for this reaction. 5. Let’s say that we mix initially in a flask at 298 K the gases HA, O2, and A2O6, at partial pressures of 0.555, 1.00, and 0.100 atm, respectively, together with a substantial amount of liquid water. Will the reaction proceed spontaneously toward the formation of A2O6? Type the word yes, no, or cannot tellin Blackboard.
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