Write the expression for the equilibrium constant Kp for the following reaction. Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH3 )2 as (P NH3)2 . If either the numerator or denominator is 1, please enter 1   2 Cl2O(g) + 3 O2(g)   ↔   4 ClO2(g)         K=

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I only want number 2 answered. The question is based on number one

Consider the reaction: 2H₂O(1)→ 2H₂(g) + O2(g) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 2.26 moles of H₂O(1) react at standard conditions. AS⁰⁰ Substance So system H₂(g) 02 (9) H₂O(1) J K mol 130.7 205.1 69.9 J/K

P.9 Assume that a sealed vessel at constant pressure of 1 bar initially contains 2.00 mol of NO₂(g). The system is allowed to equilibrate with respect to the reaction 2 NO₂(g) N₂O4(g). The number of moles of NO₂(g) and N₂O4(g) at equilibrium is 2.00 - 2 and , respectively, where is the extent of reaction. a. Derive an expression for the entropy of mixing as a func- tion of . b. Graphically determine the value of ₹ for which AS mixing has its maximum value. c. Write an expression for Gpure as a function of §. Use Equation 104 to obtain values of Gm for NO2 and N₂O4. d. Plot Gmixture = Gpure + AGmixing as a function of for ₹ T = 298 K and graphically determine the value of & for which Gmixture has its minimum value. Is this value the same as for part (b)?