Consider the Gibbs energies at 25 ∘C. Substance     Δ?∘f (kJ·mol−1) Ag+(aq)     77.1 Cl−(aq)     −131.2 AgCl(s)     −109.8 Br−(aq)     −

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Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. AG°r(kJ/mol) Substance M2O3(s) -9.70 M,O,(s) = 2 M(s) + M(s) What is the standard change in Gibbs energy for the reaction, as written, in the Oz(g) forward direction? AGAN = 9.70 kJ/mol What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? 0.2305 K = Incorrect What is the equilibrium pressure of O2(g) over M(s) at 298 K? 0.3741 Po, atm Incorrect

Consider the reaction: N₂(g) + 3H2(g) = 2NH3(g) AG°f (NH3) = -15.73kJ/mol Determine the equilibrium constant for this reaction at 298.15K. (Hint: Check the stoichiometry of the reaction when you use the Gibbs energy of formation) Report your answer as a whole number (no places past the decimal point).