Kinetics, Thermodynamics and Equilibrium - Revsworld

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5) Changing <strong>Equilibrium</strong> Homework A) For each of the following systems at equilibrium, predict the effect of a given change on the concentration of the specific substances. First, draw an arrow in the direction of the equilibrium shift next to the stated change. Write I if the concentration increases, D if the concentration decreases, <strong>and</strong> R if the concentration remains the same. I) 2 NH 3 (g) + heat N 2 (g) + 3 H 2 (g) 1) Stress: increase in [N 2 ]. Direction of Shift:________________________ What is the resulting effect on the concentration of: a) [NH 3 ]________________________ b) [H 2 ]_________________________ 2) Stress: increase in temperature Direction of Shift:________________________ What is the resulting effect on the concentration of: a) [N 2 ]_________________________ b) [NH 3 ]________________________ 3) Stress: increase in pressure Direction of Shift:________________________ What is the resulting effect on the: a) number of moles of N 2 ______________________ b) number of moles of NH 3 _____________________ II) 2 NO (g) N 2 (g) + O 2 (g) + heat 4) Stress: decrease in [O 2 ] Direction of Shift:________________________ What is the resulting effect on the concentration of: a) [N 2 ]_________________________ b) [NO]_________________________ 5) Stress: decrease in temperature Direction of Shift:________________________ What is the resulting effect on the concentration of: a) [O 2 ]_________________________ b) [NO]_________________________ 6) Stress: increase in pressure Direction of Shift:________________________ What is the resulting effect on the: a) number of moles of O 2 ______________________ b) number of moles of NO______________________ © 2009, Mark Rosengarten AE 32
C) Complete the following questions by CIRCLING THE ANSWER OF YOUR CHOICE: Given the equilibrium N 2 (g) + 3 H 2 (g) 2 NH 3 (g) + heat : a) If N 2 is added to the system at equilibrium, which direction will the equilibrium shift? 1. Forward 2. Reverse b) If H 2 is removed from the system at equilibrium, which direction will the equilibrium shift? 1. Forward 2. Reverse c) If NH 3 is added to the system at equilibrium, which direction will the equilibrium shift? 1. Forward 2. Reverse d) If temperature is decreased to the system at equilibrium, which direction will the equilibrium shift? 1. Forward 2. Reverse e) If pressure is increased to the system at equilibrium, which direction will the equilibrium shift? 1. Forward 2. Reverse f) If H 2 is removed from the system at equilibrium, what will happen to the concentrations of (circle your choice for each) 1. N 2 {increase} {decrease} {remain the same} 2. NH 3 {increase} {decrease} {remain the same} g) If NH 3 is removed from the system at equilibrium, what will happen to the concentrations of (circle your choice for each) 1. N 2 {increase} {decrease} {remain the same} 2. H 2 {increase} {decrease} {remain the same} D) Given the equilibrium system H 2 (g) + I 2 (g) + 53.0 kJ 2 HI (g), list four things that can be done to result in an increase in the concentration of HI (g). 1)____________________________________________ 2)______________________________________ 3)____________________________________________ 4)______________________________________ E) Given the equilibrium system NaOH (s) Na +1 (aq) + OH -1 (aq) + 44.51 kJ, list four things that can be done to result in an increase in the concentration of NaOH (s). 1)____________________________________________ 2)______________________________________ 3)____________________________________________ 4)______________________________________ © 2009, Mark Rosengarten AE 33
Page 1 and 2: Kinetics, Thermodynamics and Equili
Page 3 and 4: FACTORS THAT AFFECT REACTION RATE B
Page 5 and 6: 2) Potential Energy Diagrams (HW: p
Page 7 and 8: Potential Energy Diagrams: graph th
Page 9 and 10: 3) Equilibrium Systems (HW: p. 28,
Page 11 and 12: For the equilibrium 2 SO 2 (g)+ O 2
Page 13 and 14: The more soluble the salt is, the h
Page 15 and 16: 2) ENTROPY - the randomness (disord
Page 17 and 18: The quantity ∆G is Gibbs Free Ene
Page 19 and 20: A/E Reference Table B Energies of F
Page 21 and 22: Catalysts, inhibitors and surface a
Page 23 and 24: Student Name:______________________
Page 25 and 26: D) For the following blank PE Diagr
Page 27 and 28: H) Graph and label a potential ener
Page 29 and 30: 8) Complete the following chart: K
Page 31: D) For the formation of PbO: 1) Usi

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