For substance A, the entropy of the solid at 98.36 K is 7.36 Cal/molK, at this temperature it takes place the transition from one solid form to another, the transition heat is 284.3 cal/mol. The increase in entropy of the second solid modification is 98.36 K to 158.91 K and is 5.05 Cal/molK; The temperature of 158.91 K is the melting temperature of the solid. The melting heat of the solid is 476 cal/mol. From the melting point to the boiling point, 188.07 K, the increase of entropy is 2.36 Cal/molK and the heat of vaporization is 3860 cal/mol. A heat capacity from the boiling point to 298 K is 6.98 Cal/molK to an atmosphere of pressure. To calculate the absolute entropy of a considering as ideal gas an atmosphere and 298 K.
For substance A, the entropy of the solid at 98.36 K is 7.36 Cal/molK, at this temperature it takes place the transition...
For substance A, the entropy of the solid at 98.36 K is 7.36 Cal/molK, at this temperature it takes place the transition from one solid form to another, the transition heat is 284.3 cal/mol. The increase in entropy of the second solid modification is 98.36 K to 158.91 K and is 5.05 Cal/molK; The temperature of 158.91 K is the melting temperature of the solid. The melting heat of the solid is 476 cal/mol. From the melting point to the...
For substance A, the entropy of the solid at 98.36 K is 7.36 Cal/molK, at this temperature it takes place the transition from one solid form to another, the transition heat is 284.3 cal/mol. The increase in entropy of the second solid modification is 98.36 K to 158.91 K and is 5.05 Cal/molK; The temperature of 158.91 K is the melting temperature of the solid. The melting heat of the solid is 476 cal/mol. From the melting point to the...
Entropy of naphthalene: Consider naphthalene C10H8 at atmospheric pressure. It is a solid with a melting point at 80.1 degrees Celsius and a boiling point at 218 degrees Celsius. The latent heat of fusion is 19,123 kJ / mol. The molar heat at constant pressure of solid naphthalene has a functional temperature dependence (in K) which is linear. Its value is 0 at T = 0 K and 188.41 J / mol-K at T = 317.15 K. The molar heat...
6. Sketch a properly-labeled plot of isobaric molar entropy vs. temperature for a typical pure substance X that exists as solid B below 100. K, solid a above 100. K, and has a melting point of 300. K and a boiling point of 400. K. Assume substance X has no residual entropy. 7. Calculate the standard molar entropy of fusion of substance X in the previous question if the standard enthalpies of formation of solid and liquid X are 147...
4. The standard enthalpy of fusion of mercury is 560 cal/mol at a temperature of 234.1 K Assuming that the densities of solid and liquid mercury at the melting point are 14.19 and 13.69 g/cm, calculate: (report your answers in SI units for parts A and B) A. The standard entropy of fusion B. AU C. The melting point in °C) at 20 torr and 10 atm
32. At what temperature (in kelvin units) is the entropy of a pure crystal 0.0 J/K. 33. Use the standard entropies for liquid water and steam to estimate the enthalpy of vaporization of water at its normal boiling point. AS [H2O(l)] = 69.9 J/K mol and AS [H2O(g)] = 188.8 J/K mol.
The temperature of hte triple point: 195.41 K Consider the phase diagram of NH3. Triple point: 195.410 K and 0.06921 atm Normal boiling point: -33.342 oC Normal freezing point: -77.728 oC Density of liquid: 0.618g/mL Density of solid: 0.817 g/mL (a) Determine the heat of fusion, the heat of vaporization the heat of sublimation at near the triple point. (b) Determine the entropy change of fusion, vaporization and sublimation at near the triple point. (c) Plot the phase diagram...
5. Calculate the heat (in kJ) required to transform 70.80 g of bromine from a solid at a temperature of -7.2 °C to a gas at 92 °C. Report your answer to one decimal place. Data: Molar mass of bromine, Br 2 = 159.808 g/mol Melting point = -7.2 °C Boiling point = 59°C. Enthalpy of fus ion = 10.57 kJ/mol Enthalpy of vaporization = 29.96 kJ/mol. Molar heat capacity of the liquid phase = 75.7 J/mol • K Molar...
X is known to exist at 1 atm in the solid, liquid, or vapor phase, depending on the temperature. Additionally, the values of these other properties of Substance X have been determined: boiling point 35. melting point enthalpy of fusion6.00 kJ/mol enthalpy of vaporization 34.00 kJ/mol 46. J-K mol (solid) 73. JK mol (vapor 2.80 g/em (solid) 2.40 g/mL (liquid density heat capacity61.JKmol Ciquid) You may also assume X behaves as an ideal gas in the vapor phase. Suppose a...
you decided to investigate how much energy it would take to get solid acetone to gaseous acetone. So assuming you took 125 g of -100 degree Celsius solid acetone and heated it 56 degree Celsius gaseous acetone, how many joules of energy would be required to do this? Acetone has a melting point of -95 degree Celsius and a boiling point of 56 degrees Celsius. The heat of fusion (melting) is 98 j/g and the heat of vaporization is 538.9...