One mole of liquid naphthalene at its freezing point of 80 ˚C is brought into contact with a very large ice-water bath, which remains at 0 ˚C as the naphthalene freezes and cools to 0˚C. The enthalpy of fusion of naphthalene is 19.2 kJ mol-1 and ~ C p for solid naphthalene is 180 J K-1 mol-1. Calculate the decrease in entropy for the naphthalene and the increase in entropy for the overall system (naphthalene + ice-water bath).
One mole of liquid naphthalene at its freezing point of 80 ˚C is brought into contact...
The ΔG for the freezing of H2O(l) at -10 ∘C is-210 J/mol and the heat of fusion of ice at this temperature is 5610 J/mol . Find the entropy change of the universe when 3 mol of water freezes at -10 ∘C.
I would really appreciate your help. God bless you Question 4 The molar enthalpy of fusion of ice at 0 °C and 1 atm pressure is 6024 J mol. The molar heat capacities at constant pressure of ice and water are 37.65 J Kmol and 75.30 J Kmol respectively, and may be taken as constant over the temperature range 0 to -20°C. Consider 2 mole of liquid water supercooled to -20 °C, which is allowed to freeze isothermally from liquid...
The enthalpy of fusion of cadmium at its normal melting point of 321 °C is 6.11 kJ mol? What is the entropy of fusion of cadmium at this temperature? ASfus = J mol-K-1 The molar enthalpy of fusion of solid cadmium is 6.11 kJ mol-1, and the molar entropy of fusion is 10.3 JK+mol-1. (a) Calculate the Gibbs free energy change for the melting of 1.00 mol of cadmium at 622 K. (b) Calculate the Gibbs free energy change for...
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...
You have a block of ice at a temperature of -100°C. This block of ice is made from 180g H2O. The block of ice will be heated continually until it becomes super-heated steam at a temperature of 200°C Cice = 2.03 J/g-K ΔHfus=6.01 kJ/mol Cwater = 4.18 J/g-K Csteam = 1.84 J/g-K ΔHvap=40.67 kJ/mol What is the enthalpy change raising the temperature of 180 g of ice at −100 °C to 0°C? What is the enthalpy change upon melting 180...
The ΔG for the freezing of H2O(l) at -10 ∘C is -210 J/mol and the heat of fusion of ice at this temperature is 5610 J/mol . Find the entropy change of the universe when 2 mol of water freezes at -10 ∘C. (in J/K)
14. For bismuth, Bi, the heat of fusion at its normal melting point of 271 °C is 11.0 kJ/mol. The entropy change when 2.45 moles of solid Bi melts at 271 °C, 1 atm is J/K. For magnesium, Mg, the heat of fusion at its normal melting point of 649 °C is 9.0 kJ/mol. The entropy change when 1.72 moles of liquid Mg freezes at 649 °C, 1 atm is J/K
Exercise 17.102 The ?G for the freezing of H2O(l) at -10 ?C is-210 J/mol and the heat of fusion of ice at this temperature is 5610 J/mol . Part A Find the entropy change of the universe when 2mol of water freezes at -10 ?C. ?Suniv = ? J/K I got -44 but it says I am incorrect. Any help would be greatly appreicated
What is the freezing point of an alcohol in °C to the nearest degree if its heat of fusion(AHlusº) +9.37 kJ/mol and its entropy of fusion ASfusº = 50.6 J/K.mol.
Entropy (S) The second factor involved in determining whether or not a process is spontaneous is the change in randomness or entropy (AS). Entropy is represented by the symbol S. Again, experience can help us understand the relationship between entropy and spontaneous processes. If we look at the two drawings below, we can predict which picture represents the stack of marbles "before" and after they are bumped. We expect the stack of marbles (less random, lower entropy) to be the...