The molar enthalpy of vaporization of ethanol is AvapH = 42.3 kJ/mol at its normal boiling point of 351.5 K. (a) Determine its molar entropy of vaporization at the boiling point, AvapS, in J/K. (b) The values of Cp for liquid and for gaseous ethanol for 300 < T< 400 are 112.4 and 70.85 J/mol-K, respectively. Use this information to estimate AvapH (in kJ/mol) at T = 320 K, assuming that the heat capacities of the liquid and gaseous states are constant over this temperature range. Hint: Construct a multi-step process that includes vaporization at 320 K, but includes a step with vaporization at Tvap. Is this enthalpy of vaporization larger or smaller in magnitude from the standard value?

Do not give handwriting solution. Calculate the entropy change, ΔS, for the following processes. If needed, Cp(O2)= 29.4 J mol-1 K-1 and Cp(CO2) = 37.1 J mol-1 K-1.(a) The pressure of one mole of O2(g) is increased from P to 2P at 298 K.(b) The temperature of one mole of CO2(g) is increased from 298 K to 355 K at aconstant volume of 20.0 L.

When dry ice (solid CO 2) sublimates, its entropy(A) increases(B) decreases(C) does not change(D) could either increase or decrease, depending on other factors

Ice cubes at 0°C are poured into a glass that initially contains 150 g of liquid water at 20°C. The contents of the glass are gently stirred. After a short time, some of the ice melts, and the liquid cools to 0°C. No appreciable heat exchange occurs between matter inside the glass with matter outside the glass during this process. (a) Calculate the entropy change of the universe during the process. Use only the following data: the constant pressure heat capacity of liquid water is approximately 4.18 J/(g K) over the temper- ature range of interest. You may further presume that the density of water is constant over the temperature range. (b) If the same process were performed reversibly, how much useful work would be obtained from it? Any required heat exchange to achieve the same final state reversibly should be with matter outside the glass, which are at 20°C.

A reaction has values ΔS = 60.3 J K-1 mol-1 and ΔH = 49.6 kJ mol-1. At what temperature (in °C) will this reaction become spontaneous?

Consider the reaction 2NaOH(aq) + H2(g)—2Na(s) + 2H2O(l) for which AH° = 368.6 kJ and AS° = 15.30 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.759 moles of NaOH(aq) react under standard conditions at 298.15 K. ASuniverse= J/K (2) Is this reaction reactant or product favored under standard conditions? (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'. Submit Answer

A reaction has values ΔS = 60.3 J K-1 mol-1 and ΔH = 44.7 kJ mol-1. At what temperature (in °C) will this reaction become spontaneous?

"M" represents a metallic element.  "X" represents a nonmetallic element.  Calculate ΔH for the process M3X4(s) ⟶ 3M(s) + 2X2(g) from the following information: M(s) + ½X2(g) ⟶ MX(s)  ΔH°= -286.2 kJ 3MX(s) + ½X2(g) ⟶ M3X4(s)  ΔH°= -84.3 kJ