Physical Chemistry Calculate the change in entropy when one mole of metallic aluminum is heated at...
Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 °C to a final temperature of 750 °C. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol' K and 31.75 J mol' K, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 °C) is 396.57 J g! The molar mass of aluminum is 26.98 g...
Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 ℃ to a final temperature of 750 ℃. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol-1 K-1 and 31.75 J mol-1 K-1, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 ℃) is 396.57 J g-1. The molar mass of aluminum is 26.98 g...
Please do not copy the answer from others! Thank you! Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 °C to a final temperature of 750 °C. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol-1 k-and 31.75 J mol-1 k1, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 °C) is 396.57 Jg7....
1. a) Calculate the change in entropy (AS) when one mole of diamond is heated from a temperature of 0 K to 400 K at a constant pressure of 1 bar. The temperature-dependent heat capacity of diamond is C 2.9x10 T J/(mol K), where T is the absolute temperature in K. b) Given that the entropy of diamond is zero at 0 K, calculate its absolute molar entropy (S) at 400 K from the above result.
a) Show that the molar entropy change, Asm, is given by ASm = Cy,m In + Rin" if one mole of an ideal gas is taken from T,,V, to T2, V, assuming that Cv.m is independent of temperature. b) Calculate the value of the molar entropy change, Asm, if one mole of N2(g) is expanded from 20.0 dm² at 273 K to 300 dm at 400 K. (Cp.m = 29.4 JK-Imol-?)
Please explain as much as possible. Why did you use the equation? Or what conditions did you see from the question? etc. a) Show that the molar entropy change, ASm, is given by ASm Cym In2 Rln if one mole of an ideal gas is taken from T, , V to T2 , V2 assuming that Cy m is independent of temperature. b) Calculate the value of the molar entropy change, AS,m, if one mole of N2(g) is expanded from...
Calculate the entropy change for the following processes: (a) a mole of He (g) undergoes an expansion from V to 2V at 298 K (b) the temperature of one mole of CH4 (g) is increased from 298k to 325k at a constant pressure of 1 bar
Calculate the change in entropy that occurs when 18.02 g of ice at –17.5°C is placed in 90.08 g of water at 100.0°C in a perfectly insulated vessel. Assume that the molar heat capacities for H2O(s) and H2O(l) are 37.5 J K^-1 mol^-1 and 75.3 J K^-1 mol^-1, respectively, and the molar enthalpy of fusion for ice is 6.01 kJ/mol. Change in entropy = ______J/K
Calculate the change in Entropy 3. One mole of CO gas is transformed from an initial state of Ti=320K and Vi=20L to a final state of Tf=650K and Vf=120L. The temperature dependence of Cv,m is given as C = a +bT +cT? +dT”; a=31.08, b=-0.01452K-'; c=3.14x10--K?,b=-1.498x10K-
Calculate the entropy change when 72.00 g of ice, at 273.2 K and 1.000 bar pressure, is melted and then heated to 298.2 K. The enthalpy of fusion of ice is 6.009 kJ/mole and the heat molar heat capacity of water at 1.000 atm is 75.43 J/ K mole Please help! Can't figure this homework problem out.