For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction   2NO(g)+O2(g)↽−−⇀2NO2(g)   the standard change in Gibbs free energy is Δ?°=−32.8 kJ/mol. What is ΔG for this reaction at 298 K when the partial pressures are ?NO=0.500 atm, ?O2=0.350 atm, and ?NO2=0.800 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 ΔGrxn at 298 K under the conditions shown below for the following reaction. Do not enter units with your answer N2 (g) + 3 H2 (g) → 2 NH3 (g)             ΔG° = -33.3 kJ P(N2) = 1.0 atm, P(H2) = 3.0 atm, P(NH3) = 9.0 atm

Calculate the value of the free energy change, ΔG, for the reaction below at 600.0ºC when the pressures of POCl3 (g) = 20.00 atm, PCl3 (g) = 0.0250 atm, and O2 (g) = 0.0100 atm.2 POCl3 (g) → 2 PCl3 (g) +  O2 (g)