A student determines the value of the equilibrium constant to be 4.09×10-18 for the following reaction. Fe;O4(s) + 4H2(g)→3FE(s) + 4H,O(g) Based on this value of Kegi AG° for this reaction is expected to be (greater, less) greater than zero. Calculate the free energy change for the reaction of 1.76 moles of Fe;0,(s) at standard conditions at 298K. AG°. rxn = 190.5 kJ

Is the following reaction spontaneous as written? Explain. Do whatever calculation is needed to answer the question. SO2(g)+H2(g)H2S(g)+O2(g)

a Calculate K1, at 25C for sulfurous acid: H2SO3(aq)H+(aq)+HSO3(aq) b Which thermodynamic factor is the most significant in accounting for the fact that sulfurous acid is a weak acid? Why?

Consider the reaction of 1 mol H2(g) at 25C and 1 atm with 1 mol Br2(l) at the same temperature and pressure to produce gaseous HBr at these conditions. If this reaction is run in a controlled way to generate work, what is the maximum useful work that can be obtained? How much entropy is produced in this case?

For the decomposition of formic acid, HCOOH(l)H2O(l)+CO(g) H = +29 kJ/mol at 25C. a Does the tendency of this reaction to proceed to a state of minimum energy favor the formation of water and carbon monoxide or formic acid? Explain. b Does the tendency of this reaction to proceed to a state of maximum entropy favor the formation of products or reactants? Explain

What is meant by the standard free-energy change G for a reaction? What is meant by the standard free energy of formation Gf of a substance?

Is the formation of ozone (O3(g)) from oxygen (O2(g)) spontaneous at room temperature under standard state conditions?

Elemental boron, in the form of thin fibers, can be made by reducing a boron halide with H2. BCl3(g) + 3/2 H2(g) B(s) + 3HCl(g) Calculate H, S, and G at 25 C for this reaction. Is the reaction predicted to be product favored at equilibrium at 25 C? If so, is it enthalpy driven or entropy driven?

Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).

Reword the statement in Question 109 so that it is always true. Criticize this statement: Provided it occurs at an appreciable rate, any chemical reaction for which rG 0 will proceed until all reactants have been converted toproducts.