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- 1 at 1.00 atm and 154 °C, its melting temperature. The molar volume of the liquid at this e. (h) A certain solid occupies a container with volume 0.142 dm mol temperature and pressure is 0.1526 dm mol1 At 11.84 atm the melting temperature changes to 156° C. Calculate the enthalpy and entropy of fusion of the solid using the equation below (submit via link) dP AfusS dT AfusVWhen a metal is heated its density decreases. There are two sources that give rise tothis diminishment of : (1) the thermal expansion of the solid, and (2) the formation of vacancies. Consider a specimen of gold at room temperature that has a density of 19.320 g/cm3.(a) Determine its density upon heating to (800°C) when only thermal expansion is considered.(b) Repeat the calculation when the introduction of vacancies is taken into account. Assume that the energy of vacancy formation is 0.98 eV/atom, and that the volumecoefficient of thermal expansion, is equal to 3 αl3. One mole of liquid water at 100 °C is heated until the liquid is converted entirely to vapor at 100 °C and 1 atm pressure. Calculate q, w, AE and AH for each of the following. (a) The vaporization is carried out in a cylinder where the external pressure on the piston is maintained at 1 atm throughout. (b) The cylinder is first expanded against vacuum (Pext = 0) to the same volume as in part (a), and then sufficient heat is added to vaporize the liquid completely to 1 atm pressure.
- Limestone (CaCO₃) is the second most abundant mineral onEarth after SiO2. For many uses, it is first decomposed thermallyto quicklime (CaO). MgO is prepared similarly from MgCO₃.(a) At what Tis each decomposition spontaneous? (b) Quicklime reacts with SiO2to form a slag (CaSiO₃), a byproduct of steel-making. In 2003, the total steelmaking capacity of the U.S. steelindustry was 2,370,000 tons per week, but only 84% of this ca-pacity was utilized. If 50. kg of slag is produced per ton of steel,what mass (in kg) of limestone was used to make slag in 2003?(a) From the phase diagram for carbon dioxide, determine the state of co2 at 20 atm and 273 K. (b) Explain why co2 can undergo sublimation under normal condition.A recently developed variation of the Mond process carries out the first stepat higher pressures and at a temperature of 150°C. Estimate the maximumpressure of Ni(CO)4(g) that can be attained before the gas will liquefy atthis temperature (that is, calculate the vapor pressure of Ni(CO)4(e) at150°C).
- The normal boiling point of liquid benzene is 80.20 °C and its vapor pressure is 0.10 bar at 20.00°C. Calculate: (a) The value of AH vap m (b) The value of AS at the normal boiling point vap mIndicate whether each statement is true or false. (a) Thethird law of thermodynamics says that the entropy of aperfect, pure crystal at absolute zero increases with themass of the crystal. (b) “Translational motion” of moleculesrefers to their change in spatial location as a functionof time. (c) “Rotational” and “vibrational” motionscontribute to the entropy in atomic gases like He and Xe.(d) The larger the number of atoms in a molecule, themore degrees of freedom of rotational and vibrationalmotion it likely has.The molar enthalpy of fusion of solid magnesium is 8.95 kJ mol-1, and the molar entropy of fusion is 10.0 J K-1 mol-1. (a) Calculate the Gibbs free energy change for the melting of 1.00 mol of magnesium at 955 K. (b) Calculate the Gibbs free energy change for the conversion of 2.20 mol of solid magnesium to liquid magnesium at 955 K. (c) Will magnesium melt spontaneously at 955 K? (d) At what temperature are solid and liquid magnesium in equilibrium at a pressure of 1 atm?
- Calculate the vapor pressure of ethnaol at 25 Celsius. Assume the thermodynamic values are independent of temperatureThe normal boiling point of hexane is 69°C. Estimate 1. its enthalpy of vaporization and 2. its vapor pressure at 25°CFrom the following data determined at 298 K, determine (a) A, H and A₁U for reaction (4) at 298 K; (b) AfH for HI(g) and H₂O(g) at 298 K. Assume ideal gas behavior when necessary. (1) H₂(g) + I2(g) → 2 HI(g) (2) 2H₂(g) + O₂(g) → 2H₂O (g) (3) 1₂ (s)→ I2(g) (4) 4HI(g) + O₂(g) → 21₂(g) + 2H₂O(g) ΔΗΘ = +52.96 kJ mol-¹ A₂H = -483.64 kJ mol-1 A₂H = +62.44 kJ mol-¹