For a hypothetical reaction, A + B- Cata temperature T, the Gibbs free energy at each point during the reaction is plotted (see image below). The slope of the tangent to the curve at point P is 0. What is true regarding this reaction at point P? The temperature and pressure of the reaction system are kept constant. Extent of reaction A. The change in Gibbs free energy of the reaction, 4,G = 0 B. The reaction is at thermodynamic equilibrium O C. Product C is spontaneously produced. D.A,H = TxA,S O E. (A), (B), and (D) are all true Gibbs Free Energy

The change in standard free energy (i.e. ΔG°) for a particular reaction has a value of −43.1 kJ/mol at a temperature of 16.1 ℃. Calculate the equilibrium constant for this reaction. R = 8.314472 J/mol⋅K. Report your answer to THREE significant figures. Enter your answer in the appropriate boxes and remember a number such as 1.23 is 1.23 × 100 in scientific notation. Note: Your answer is assumed to be reduced to the highest power possible.

13. For the reaction, 250, (g) + 02 (g) 2- 250, (g), K. = 9 x 102 at 800 K, and K. = 1 x 10 at 635 K. Which of the following is wrong about this reaction? A) It is an exothermic reaction. B) At 800 K, SO, molecules are more stable than %3D %3D those at 635 K, C) The heat content of SO, molecules is less than that of SO, molecules. D) K, is smaller than Ke at 800 K. E) The rátio of specific rate constant for forward re- action to that of the reverse reaction at 635 K is 1x10.

A student determines the value of the equilibrium constant to be 2.69×10-10 for the following reaction.Fe2O3(s) + 3H2(g)2Fe(s) + 3H2O(g)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank than zero.Calculate the free energy change for the reaction of 2.05 moles of Fe2O3(s) at standard conditions at 298K.     G°rxn =  ____kJ

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

In which of the following reactions is ASº expected to be negative? O L(s)I(g) O 2NH;(g) → N(g) + 3H3(g) O 2H,0(g) → 2H,(g) + O>(g) O CH;OH(g) → CH;OH(I) O AS° is not expected to be negative for any of these.

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The standard reaction free energy AG° = 29. kJ for this reaction: Fe2O3(g) + 2H2 (g) --> 2 Fe(s) + 3H2O(l) Use this information to complete the table below. Round each of your answers to the nearest kJ.

Gibbs Free E 3

The decomposition of crystalline N2O5N2O5(s)?2NO2(g)+12O(g)is an example of a reaction that is thermodynamically favored even though it absorbs heat. At 25 ?C we have the following values for the standard state enthalpy and free energy changes of the reaction: Delta H = +109.6 kJ/mol Delta Standard Gibbs Free Energy = -30.5 kJ/mol    C) Calculate delta U for this reaction at 25 C.