Using data from Appendix C, write the equilibrium-constant expression and calculate the value of the equilibrium constant and the free-energy change for these reactions at 298 K: (a) NaHCO₃(s) ⇌ NaOH(s) + CO₂(g)

Consider the reaction: 2 NO(g) + O₂(g) ⇌ 2 NO₂(g) The following data show the equilibrium constant for this reaction measured at several different temperatures. Use the data to find ΔH°_rxn and ΔS°_rxn for the reaction.

Consider the decomposition of barium carbonate: BaCO₃(s) ⇌ BaO(s) + CO₂(g) Using data from Appendix C, calculate the equilibrium pressure of CO₂ at (b) 1100 K.

Consider the decomposition of barium carbonate: BaCO₃(s) ⇌ BaO(s) + CO₂(g) Using data from Appendix C, calculate the equilibrium pressure of CO₂ at (a) 298 K.

A reaction has an equilibrium constant of 8.5⨉10³ at 298 K. At 755 K, the equilibrium constant is 0.65. Find ΔH°_rxn for the reaction.

The value of K_a for nitrous acid (HNO₂) at 25 °C is given in Appendix D. (c) What is the value of ΔG at equilibrium?

The value of K_a for nitrous acid (HNO₂) at 25 °C is given in Appendix D. (b) By using the value of Ka, calculate ΔG° for the dissociation of nitrous acid in aqueous solution.

The value of K_a for nitrous acid (HNO₂) at 25 °C is given in Appendix D. (d) What is the value of ΔG when [H⁺] = 5.0⨉10^-2 M, [NO₂^-] = 6.0⨉10^-4 M, and [HNO₂] = 0.20 M?