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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.Without carrying out an explicit calculation, explain there lative values of the standard molar entropies (at 298 K) of the following substances: (a) Ne(g) (146 J K-1 mol-1) compared with Xe(g) (170 J K-1 mol-1), (b) H2O(g) (189 J K-1 mol-1) compared with D2O(g) (198 J K-1 mol-1), (c) C(diamond) (2.4 J K-1 mol-1) compared with C(g raphite) (5.7 J K-1 mol-1).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 enthalpy of vaporization (deltaHvap) of water was experimentally determined to be 151.3 kJ for 3.72 mols of water at 100 degrees Celsius? Calculate the molar entropy of vaporaization (deltaSvap,m) of water.Derive a formula for the molar Gibbs free energy change of a closed system at constant temperature if the system obeys the equation of state PV = nRT + nCP where C is a constant.Suppose a certain small bird has a mass of 30 g. What is the minimum mass of glucose that it must consume to fly to a branch 10 m above the ground? The change in Gibbs energy that accompanies the oxidation of 1.0 mol C6H12O6(s) to carbon dioxide and water vapour at 25 °C is -2828 kJ.
- Given a thermodynamic function h=h(s,p) show how to evaluate T, V , U , A or F and GCalculate the molar entropy of an ensemble by S=U/T+klnQ with 1.32 mole of Kr(g) at 47degree and a pressure of 1.7 bar.The change in Gibbs energy that accompanies the combustion of C6H12O6(s) to carbon dioxide and water vapour at 25 °c is -2828 kJ mol-1. The potential energy of an object of mass m at a height h, relative to that at the Earth's surface is given by mgh, where g = 9.81 m s-2 is the acceleration of freefall. How much glucose does a person of mass 65 kg need to consume to climb through 10m?
- a) Find the entropy change associated with melting pure ice at T=273.15K, P=20 bar. b) What is the Gibbs energy of melting pure ice at T=0 C and P=1 bar? c) What is the change in total entropy (system + surroundings) for the melting of pure ice at T=0 C and P=1 bar?The temperature dependence of the heat capacity of non-metallic solids is found to follow the Debye T3 -law at very low temperatures, with Cp,m = aT3. (a) Derive an expression for the change in molar entropy on heating for such a solid. (b) For solid nitrogen, a= 6.15 x 10-3 J K-4 mol-1. What is the molar entropy of solid nitrogen at 5 K?What would the entropy be for a system with 6.05E+1 microstates, in J/mol-K?