AG° at 298 K for the reaction below is -642.9 kJ/mol. P2 (g) + 3CI2 (g) - 2PCI3 (g) Calculate the value of AG at 298 K in kJ/mol for a reaction mixture with the following partial pressures: Pp2 = 1.250 atm, PCI2 = 1.000 atm, and PpC13 = 1.500 atm.

Calculate the equilibrium constant for the following reaction at 60°C using the data at 298°K H2O(g) + CH;OH(g) CO2(g) + 3H2(g) H2(g) Ag°r298 (kJ/mol) Ah°t298 (kJ/mol) H2O(g) - 228.57 - 241.82 CH;OH(g) - 161.96 - 200.66 CO2(g) - 394.36 - 393.51 Kp(0) = 4.69 Kp(333) = 37.44.

The equilibrium constant for the reaction 2NO(g) + O2(g) ⇄ 2NO2(g) was measured at two temperatures: 500 K (Kp = 1.875x104) and 600 K (Kp = 1.933x102). What is ΔH* for the reaction The expected answer is -114.1 kJ, please be precise in explaining the steps to work out this problem

Consider the reaction at 500 °C. N2(g) + 3H2(g)2NH3(g) Kc = 0.061 If analysis shows that the composition of the reaction mixture at 500 °C is 1.14 mol L-¹ N2, 5.52 mol L-¹ H₂, and 3.42 mol L¹NH3, what is the value of the reaction quotient Q? Q = In which direction does the reaction tend to proceed to reach equilibrium? forms more reactants already at equilibrium forms more products