Determine AG° for the reaction 2 NO₂(g) → 2 NO(g) + O₂(g) at 25 °C. Substance NO₂ (g) NO (g) A) -70.6 kJ/mol B) +35.3 kJ/mol C) +70.6 kJ/mol D) -35.3 kJ/mol AG°f (kJ/mol) 51.3 86.6

Ag(+aq) + Cl-(aq) AgCl(s) ∆H = +112 kJIf ions are colorless, and AgCl is whiteWill the reaction appear “colorless” or “white” if:a) Some of the AgCl (s) is removed?b) The pressure is decreased?c) The temperature is raised?

For a particular reaction at 180.9 °C, AG = 527.78 kJ/mol, and AS = 953.96 J/(mol · K). Calculate AG for this reaction at -3.7 °C. AG = kJ/mol

Below what temperature does the following reaction become nonspontaneous?             2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l)            ΔH = +136.5 kJ;    ΔS = +287.5 J/K A) 39.2 K B) 151 K C) 475 K D) 501 K

Carbon monoxide reacts with water according to the following equilibrium reaction: CO (g) H2O (g) CO2 (g) + H2 (g) For this reaction, K = 0.810 at a temperature of 1000.°C. Calculate the value of AG for this reaction at 1000.ºC. %3D

Consider the reaction: PbCl2(s) → Pb2*(aq) + 2 Cl (aq) AH° = 23.30 kJ/mol and AS° = -12.5 J/K-mol a) When solid PbCl2 is dissolved in water at 25°C, what are the concentrations of Pb2* and Cl at equilibrium? (Hint: Do your ICE chart and Law of Mass Action.) Concentration of Pb2+: mol/L and Concentration of Cl = mol/L (Do not use superscripts, subscripts, or carets. Write 1.2 x 10-3 as 1.2x10-3 or 1.2e-3.) b) At 25°C, This reaction is (reactant or product) favored. Justify your answer with the appropriate calculation on the separate sheet of paper. c) The Gibbs free energy at 25°C, when both the concentrations of the lead ion and chloride ion are 1.2 x 10-³M is kJ/mol. Show your calculations on the separate sheet of paper.

17. The thermochemical equation for the reaction of F2 and water is as follows. AH = -270 kJ F2(g) + 2 H2O (liq)=HF (aq) + O2 (g) Given a system that is initially at equilibrium, which of the following actions cause the reaction to proceed to the right? a) adding O2(g) b) decreasing the temperature c) adding a catalyst d) decreasing the volume of the reaction chamber e) none of the above

The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K.CO(g) + Cl2(g) COCl2(g)If ΔH° for this reaction is -108 kJ, what is the value of Kp at 699 K?Kp =

Calculate the temperature at which the reaction below will be at equilibrium, then explain how this temperature can affect the spontaneity, meaning how using higher or lower than this temp can affect the value of delta G.   Given.      Br2(l) → Br2 (g),  ΔH = 31.0 kj/mol ΔS = 92.9 j/mol