E. Calculating thermodynamic quantities (Individual Work) Temperature (°C) Temperature Ksp (K) AG° (kJ mol-1) 95.00 368.115 Ca(OH)2 Solution 9.1883x10 4.2646x10" 20.90 294.05 1.3371x106 3.30650 AH° (kJ mol-¹) AS (J mol¹ K-1)
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- The enthalpy of vaporization of liquid diethyl ether, (C2H5)2O, is 26.0 kJ/mol at the boiling point of 35.0 °C. Calculate ΔS° for a vapor-to-liquid transformation at 35.0 °C.A 1 mol quantity of hydrogen gas sample was heated at constant pressure from a temperature of 300 K to 500 K. With the entropy transformation process as a function of temperature variation, the heat capacity equation at constant pressure was estimated , Cp = 6.9469 - 0.199 x 10-3 T + 4.808 x 10-7 T2 (J K-1mol-1). Determine the entropy change of the process.Please help answer unanswered parts: Calculations 1 and 2 (at bottom, red boxes) Equation used was as follows: C [crystal graphite] + CO2 [gas ] ⇌ 2CO [gas ] ; Formation of carbon monoxide Equation: C [crystal graphite] + CO2 [gas] + <---> 2CO [gas] + + Standard Enthalpy of Formation and Entropy ∆fHo(T) (KJ/mol) So(T) (J/mol.K) C [crystal graphite] 18.51 30.32 CO2 [gas] -343.41 283.87 CO [gas] -78.69 243.42
- The temperature of the steam coming from the steam boiler to the steam engine cylinder is 120 °C. Steam condensed in a cold reservoir at 40 °C. What is the maximum work. What is done by the engine under ideal conditions with 4.2 kJ of heat absorbed?What is the temperature of the high-temperature reservoir of a process that has an efficiency of 44.0% (0.440) and a low-temperature reservoir at 150°C?The standard Gibbs energy of formation of rhombic sulfur is zero, and that of monoclinic sulfur is +0.33 kJ mol−1 at 25 °C. The standard molar entropy of rhombic sulfur is 31.80 J K−1 mol−1, and that of monoclinic sulfur is 32.6 J K−1 mol−1. At what temperature will the transition occur at 1 bar? _______ K. 3 sig. fig.
- The vaporisation of a certain element at 25.0 oC has the following enthalpy and entropy values: Hvap = 1.00 kJ mol-1 and Svap = 156 J K-1 mol-1. What is the total entropy change (Stot) for the vaporisation of this element, in J K-1mol-1?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)The vaporisation of a certain element at 21 degrees Celsius had the following enthalpy and entropy values: ∆Hvap= 3.40 KJ mol-1 and ∆Svap= 246 J K-1mol-1 What is the total entropy change (∆Stot) for the vaporisation of this element in J K-1 mol-1? With correct significant figures.
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