Use the standard free energy data in the Standard State Thermodynamic Data table to determine the free energy change for each of the following reactions (in kJ/mol), which are run under standard state conditions and 25°C. Identify each as either spontaneous or nonspontaneous at these conditions.   (a) C(graphite) + O2(g) → CO2(g) ΔG°= ??? kJ/mol --> Do not know how to figure this??? Need answer and explanation. I know this is spontaneous.   (b) N2O(g) + O2(g) → N2O3(g) ΔG°= ??? kJ/mol --> Do not know how to figure this??? Need answer and explanation. I know this is nonspontaneous.   (c) PCl3(l) + Cl2(g) → PCl5(g) ΔG°= ??? kJ/mol --> Do not know how to figure this??? Need answer and explanation. I know this is spontaneous.   (d)Cr2O3(s) + 3 CO(g) → 2 Cr(s) + 3 CO2(g) ΔG°= ??? kJ/mol --> Do not know how to figure this??? Need answer and explanation. I know this is nonspontaneous.   (f) LiI · 2 H2O(s) → LiI(s) + 2 H2O(g) For this part only, use the following data. LiI · 2 H2O(s) = ΔG⁰298 = −780.3 kJ/molLiI(s) = ΔG⁰298 = −270.3 kJ/molH2O(g)= ΔG⁰298 = −228.6 kJ/mol ΔG°= ??? kJ/mol --> Do not know how to figure this??? Need answer and explanation. I know this is nonspontaneous.   PLEASE BE SURE ANSWERS ARE CORRECT!!! THANK YOU!

Is the following reaction spontaneous (a) only at low temperatures; (b) only at high temperatures; (c) at all temperatures? (d) a reaction can also be never spontaneous (Hint: Find formation values for each species in your book and calculate  reaction, you can determine if  is positive or negative by looking at the equation.) 2 NO (g) + O­2 (g) → 2 NO­2 (g)

Use the reaction for the formation of NH3 from its elements N2(g) and H2(g) . This reaction has the following thermodynamic data:  ΔfHo (NH3) = - 45.9 kJ/mol and ΔfSo (NH3) = - 99.1 J/mol*K at 298 K a) Write a balanced equation (whole number ratios) for this process and write out the expression for the reaction quotient Q using partial pressures. b) Without doing any calculations, explain how the progression of the reaction will change (more reactants or more products) with respect to 1) increasing temperature, and 2) increasing pressure. c) Calculate the equilibrium constant K at 298 K d) Assuming that : ΔfHo  is independent of temperature, calculate K at - 78o C

The reaction                         2 NO(g)   ⇆  N2O4(g) occurs at 25oC under standard state conditions with ΔGo = 13.1 kJ/mol. What is the free energy change (in J/mol) when the NO partial pressure is 0.649 Atm and the N2O4 partial pressure is 0.0015 Atm?