Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. AG°((kJ/mol) Substance M,0,(s) = 2 M(s) +0,(g) 3 M2O3(s) -9.70 M(s) What is the standard change in Gibbs energy for the reaction, as written, in the O(g) forward direction? AGAN = kJ/mo What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? K = What is the equilibrium pressure of O2(g) over M(s) at 298 K? Poz atm

8. Gaseous nitrosyl bromide, NOBr, is formed by the reaction 2NO(g) + Br,(g) 2 2NOBr(g) At 25°C, the equilibrium constant for this reaction is K, = 116 atm-1. The reaction as written is exothermic, or heat emitting. When the following amounts of the three gases are introduced into a 1-liter flask, is the reaction spontaneous in the forward or reverse direction, or is it at equilibrium? a) 0.045 atm NOBr, 0.01 atm NO, and 0.10 atm Br, at 25°C b) 0.045 atm NOBr, 0.10 atm NO, and 0.01 atm Br, at 25°C c) 0.108 atm NOBr, 0.10 atm NO, and 0.01 atm Br, at 0°C

Calculate the standard free-energy change AG" and the equilibrium constant K, for the following reaction at 25°c. Co(g) + 3H3 (9) → CH, (g) + H20(g) Substance AG (kJ/mol) Co() -137.2 H2 (9) CH, (g) -50.80 H2 O(9) -228.6 AG° kJ K,

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[Review Topics] [References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH=-108 kJ, and K. 77.5, at 600 K. CO(g) + C,(g) COCI,(g) When 0.22 moles of Cl,(g) are added to the equilibrium system at constant temperature: The value of K The value of Qe K. The reaction must O run in the forward direction to restablish cquilibrium. O run in the reverse direction to restablish cquilibrium. O remain the same. It is already at cquilibrium. The concentration of CO will Submit Answer Retry Entire Group 1 more group attempt remaining

8. Consider the following equilibrium: 2Cu(s) + O2(g) = 2CUO(s) Kc = ? How would you calculate Kc using the following coupled reactions? 4Cu(s) + O2(g)= 2Cu2O(s) K1 2CuO(s) = Cu2O(s)+ ½ O2(g) K2 KI x K2 CKI x (K2)2 *(K2)2/K1 X(KI)/K2

38. For this process at 25 °C: H2O(g) H2O (A) AH is negative as energy is released. (B) AH is negative as energy is absorbed. (C) AH is positive as energy is released. (D) AH is positive as energy is absorbed.

Consider the system below at equilibrium at 200°C: 2C12 (g) + 2H20 (g) - 98.6KJ = 4HCI (g) + 02 (g) The change listed below would cause more reactants to form when equilibrium is re- established. Write A if true and B if false (Note: Answer is case sensitive) Decreasing the volume at constant temperature