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19 Nov 2019
Short Answer Questions 1. (10 Points) A 2.00 L flask is filled with 0.159 atm of N2(g) and 0.393 atm of H (g). At equilibrium at 4000c, the flask contains 0.014 atm of NH3 (g), N2 (g) + 3 H2 (g)ê·¼ 2 NH 3 (g), ÎH -92.2 kJ a) Would the amount of NH3 at equilibrium increase or decrease by increasing the pressure of the system? b) Would Kp increase or decrease with inereasing temperature? Answer: a) NH3 b) Kp (6 Points) The reaction A(g) â 3 B (g) + C (g) has Ke equal to 41 298°c. What is Kp at this temperature? 2. .0 at Answer: Kp = 3. (8 Points) Consider the reaction: 2 AB2 (g) A2 (g) 2 B (g) . A 100.0 mL flask is filled with 0.372 mo1 of AB2 and the appearance of A2 is monitored at timed intervals as shown in the table below Assume that temperature and volume are kept constant. Fill in the blanks in the table for the disappearance of AB2 Time (min) Moles of A2 Moles of AB2 10 20 0.0521 0.0813 0.372 (s Points) Given the following reactions and equilibrium constants H2O(g) + CO(g) H2 (g) + CO2 (g) K-1.6 FeO (s) + CO(g) ê·¼ Fe(s) + CO2(g) K = 0.67 calculate K for the reaction Fe(s) + H2O(g) ê·¼ FeO (s) + H2 (g) Answer: K
Short Answer Questions 1. (10 Points) A 2.00 L flask is filled with 0.159 atm of N2(g) and 0.393 atm of H (g). At equilibrium at 4000c, the flask contains 0.014 atm of NH3 (g), N2 (g) + 3 H2 (g)ê·¼ 2 NH 3 (g), ÎH -92.2 kJ a) Would the amount of NH3 at equilibrium increase or decrease by increasing the pressure of the system? b) Would Kp increase or decrease with inereasing temperature? Answer: a) NH3 b) Kp (6 Points) The reaction A(g) â 3 B (g) + C (g) has Ke equal to 41 298°c. What is Kp at this temperature? 2. .0 at Answer: Kp = 3. (8 Points) Consider the reaction: 2 AB2 (g) A2 (g) 2 B (g) . A 100.0 mL flask is filled with 0.372 mo1 of AB2 and the appearance of A2 is monitored at timed intervals as shown in the table below Assume that temperature and volume are kept constant. Fill in the blanks in the table for the disappearance of AB2 Time (min) Moles of A2 Moles of AB2 10 20 0.0521 0.0813 0.372 (s Points) Given the following reactions and equilibrium constants H2O(g) + CO(g) H2 (g) + CO2 (g) K-1.6 FeO (s) + CO(g) ê·¼ Fe(s) + CO2(g) K = 0.67 calculate K for the reaction Fe(s) + H2O(g) ê·¼ FeO (s) + H2 (g) Answer: K
Jean KeelingLv2
14 Oct 2019