Starting with the standard free energies of formation from the following table, calculate the values of ΔG° and E°cell of the following reactions.   Substance ΔΔG°f (kJ/mol) FeO(s) -255.2 H2(g) 0 Fe(s) 0 H2O(l) -237.2 Pb(s) 0 O2(g) 0 H2SO4(aq) -744.5 PbSO4(s) -813.0 (b) 2Pb (s) + O2 (g) + 2H2SO4 (aq) ------> 2PbSO4 (s) + 2H2O (l)

Is the following reaction spontaneous as written? Explain. Do whatever calculation is needed to answer the question. CH4(g)+N2(g)HCN(g)+NH3(g)

Elemental boron, in the form of thin fibers, can be made by reducing a boron halide with H2. BCl3(g) + 32 H2(g) B(s) + 3 HCl(g) Calculate rH, rS, and rG at 25 C for this reaction. Is the reaction predicted to be product-favored at equilibrium at 25 C? If so, is it enthalpy- or entropy-driven? [S for B(s) is 5.86 J/K mol.]

Use S values to calculate the standard entropy change, rS0, for each of the following processes and comment on the sign of the change. (a) KOH(s) KOH(aq) (b) Na(g) Na(s) (c) Br2() Br2(g) (d) HCl(g) HCl(aq)

Silver carbonate, Ag2CO3, is a light yellow compound that decomposes when heated to give silver oxide and carbon dioxide: Ag2CO3(s)Ag2O(s)+CO2(g) A researcher measured the partial pressure of carbon dioxide over a sample of silver carbonate at 220C and found that it was 1.37 atm. Calculate the partial pressure of carbon dioxide at 25C. The standard enthalpies of formation of silver carbonate and silver oxide at 25C are 505.9 kJ/mol and 31.05 kJ/mol, respectively. Make any reasonable assumptions in your calculations. State the assumptions that you make, and note why you think they are reasonable.

At 298 K, G = 70.52 kJ for the reaction 2NO(g) + O2(g) 2NO2(g) (a) Calculate _G at the same temperature when PNO = 1.0 104 atm, PO2=2.0103 atm, and PNO2=0.30 atm. (b) Under the conditions in part a, in which direction is the reaction spontaneous?

On the basis of your experience, predict which reactions are spontaneous: (a) PbO2(s)Pb(s)+O2(g)(b) N2(l)N2(g) at 25C (c) C6H12O6(s)C6H12O6(l) at 25C (d) Ca2+(aq)+CO32(aq)CaCO3(s)

The molecular scale pictures below show snapshots of a strong acid at three different instants after it is added to water. Place the three pictures in the correct order so that they show the progress of the spontaneous process that takes place as the acid dissolves in the water. Explain your answer in terms of entropy

According to a source, lithium peroxide (Li2O2) decomposes to lithium oxide (Li2O) and oxygen gas at about 195C. If the standard enthalpy change for this decomposition is 33.9 kJ/mol, what would you give as an estimate for the standard entropy change for this reaction? Explain.

Which contains greater entropy, a quantity of frozen benzene or the same quantity of liquid benzene at the same temperature? Explain in terms of the dispersal of energy in the substance.