a) Show that the molar entropy change, Asm, is given by ASm = Cy,m In +...
Physical Chemistry 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 K1 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 g1. The molar mass of aluminum is...
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...
9. Derive the equation dH = TDS + VdP and show tha ASm = Cp.m In 2 - R In For the change of one mole of an ideal gas from Tu, P, to T2, P, assuming that Cp,m is independent of temperature. (Hint: Start from dU = Tds - pdV and consider what you need to add to both sides to get an expression for dH on the left side).
The standard molar entropy of NH3 is 192.45 J K'mol ' at 298 K, and its heat capacity is given by the equation Cp.m = a + bT + c/T2 with the coefficients given in table below. Calculate the standard molar entropy of NH3 at a) 100 °C. (10 pts) Table 1: Temperature variation of molar heat capacities, C /OK-Imol-1) = a +bT + c/T2 c b/(10-K) I 25.1 /(10% K) -155 NH3 29.75
Calculate the change in entropy ΔS for 5.2 moles of an ideal gas when its thermodynamic state changes from p1 = 1.50 atm and T1 = 400.0 K to p2 = 3.00 atm and T2 = 600.0 K. The molar heat capacity of the gas at constant volume is CV,m = (7/2) R, and is independent of the temperature.
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.
Calculate the entropy change from burning 41.1 g of solid glucose (C6H1206, molar mass 180.2 g/mol) to produce gaseous carbon dioxide and gaseous water, using the values in the table below. S0/JK mor Substance Glucose(s) O2(g) CO2(g) H2O(g) 209.2 205.15 213.79 188.84 Select one: a. 4.01e4 J/K b. 223 J/K C. -2.67 J/K d. None of the other options e. -482 J/K
Calculate the entropy change from burning 41.1 g of solid glucose (C6H1206, molar mass 180.2 g/mol) to produce gaseous carbon dioxide and gaseous water, using the values in the table below. Substance º/JK' mort Glucose(s) 209.2 02(9) 205.15 CO2(g) 213.79 H2009) 188.84 Select one: a. 4.01e4 J/K o b. 223 JIK O C.-2.67 J/K d. None of the other options. e-482 J/K
Question 17 Incorrect Mark 0.00 out of 1.00 Flag question Calculate the increase of entropy (in J/K) when 76 g of ice melts at 0 °C and 1 atm. (The heat of fusion for ice is 6,000 J/mol.) Answer: 208.4 Question 18 Incorrect Mark 0.00 out of 1.00 Calculate the change in entropy (in J/K) when 29.1 g of water is heated from 27.1 °C to 76.5 °C at 1 atm. (The specific heat is 4.184 J/(g-K).) Flag question Notice...
any help thank you Chapter 12 Ideal Gas Mixtures and Psychrometric Applications Converting Between Mass Fraction and Mole Fraction Mass Fraction Mole Fraction m/M y, M M mf M cy, MM m/M Example 1: Determine the mf CO2 0.04 MW mix mixture molecular weight mf_N2 0.7 m mix (kg) (kg/kmol), specific volume mf_02 0.2 0.06 (m®/kg), and mole fraction for mf_H20 T(C) 40 a gas mixture given the mass P (bar) 1 fraction, temperature, pressure and volume. V(m3) Example 2:...