. Use data from appendix B (attached phhoto) to obtain the equilibrium constant Kp for each reaction at 298.15 K. A. 2 HCl(g) ---> H2 (g) + Cl2 (g) B. N2(g) + O2(g) ---> 2 NO(g)
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24. Use data from appendix B (attached phhoto) to obtain the equilibrium constant Kp for each reaction at 298.15 K.
A. 2 HCl(g) ---> H2 (g) + Cl2 (g)
B. N2(g) + O2(g) ---> 2 NO(g)
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- What does the superscript ° indicate when associated with a thermodynamicquantity, as in ΔH°, ΔS°, or ΔG°?What does the superscript ° indicate when associated with a thermodynamicquantity, as in ∆H °, ∆S°, or ∆G°?Consider the following reaction: H2(g) + ½ O2 (g) ------> H2O (g) The standard enthalpy of formation of gaseous H2O at 298 K is -241.82 kJ mol-1. Calculate the value at 153 0C. Given Cp,m for H2O(g): 33.58 kJ mol-1; H2 (g): 28.84 kJ mol-1; O2 (g): 29.37 kJ mol-1. Assume heat capacities are independent of T. NOTE:answer in kilojoules per mole (kJ/mol)
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- The molar enthalpy of fusion of ice at 273.15 K and one atm is ΔfusHm (H2O)=6.01 kJ mol-1, andthe molar entropy of fusion under the same conditions is ΔfusSm (H2O)=22.0 J K-1 mol-1. Show that(a) ΔfusGm (H2O)=0 at 273.15 K and one atm, (b) ΔfusG,m (H2O) < 0 when the temperature is greaterthan 273.15 K, and (c) ΔfusGm (H2O) > 0 when the temperature is less than 273.15 K.A sample of K(s) of mass 3.226 gg undergoes combustion in a constant volume calorimeter at 298.15 K. The calorimeter constant is 1849 J⋅K−Mol-, and the measured temperature rise in the inner water bath containing 1538 gg of water is 1.776 K. CP,m(H2O,l)=75.3J⋅mol−1⋅K−1CP,m(H2O,l)=75.3J⋅mol−1⋅K−1. 1) Calculate ΔU���f for K2O 2) Calculate ΔH∘f for K2OThermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 10. What is the ∆S⁰ in the combustion of hydrogen in the presence of excess oxygen yields water: 2H2(g) + O2(g) → 2H2O(l) in J/K?