4. Calculate (a) AG°, and (b) K, for the following equilibrium reaction at 25.0 °C. PCI,(g) = PCl;(g) + Cl,(g) (c) Calculate AG for the reaction if the partial pressures of the initial mixture are PPCIS= 0.0029 atm, PPC= 0.27 atm, and PCh= 0.40 atm. (d) In which direction is the spontaneous reaction?

3. Consider the following reaction: Co(g) + 2H2(g) S CH;OH(g); Kp = 2.26x10ª at 25 °C Calculate AG for the reaction at 25 °C for each of the following conditions: (a) standard conditions (b) at equilibrium (c) P (CH3OH) = 1.0 atm, P (CO) = P (H2) = 0.010 atm

Consider the following reaction, where AG =-625 J at 300 C, 2 XOG) + Oz(g) 2 X02(g) a) Determine K, at 300 °C. b) Calculate AG° at 300 °C when P(XO) = 8.0x10-4 atm, P(O2) = 0.072 atm, and P(XO2) = 9.0 atm. %3D c)Is the reaction spontaneous when carried out under the conditions in (b)? How do you know? (no points for guessing) d) At 0.00 °C, AG" = 17000 J/mol. Calculate AH and AS.

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