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.
Calculation of delta G and delta H for 3 mol water
Calculation of T in K
T (K) = - 10 + 273.15 = 263.15 K
Delta G = 3 mol water x -210 J/mol=-630 J
Delta H = 3 mol waer x 5610 J/mol = 16830 J
Lets find delta S by using following equation.
Delta G = Delta H – Tdelta S
T delta S = Delta H – Delta G
Delta S = [Delta H – Delta G]/T
= {[-630 - ( 16830)] /263.15 }
=-66.35 J /K
Delta S = -66.35 J/K
The ΔG for the freezing of H2O(l) at -10 ∘C is-210 J/mol and the heat of...
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)
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
The constant-pressure molar heat capacity of H2O (s) and H2O (l) is 75.291 J K−1 mol−1 and that of H2O (g) is 33.58 J K−1 mol−1 . Assume that the constant-pressure molar heat capacities are constant over the studied temperature range. Calculate the change in entropy of the system when 15.0 g of ice at −12.0 °C is converted to water vapour at 105.0 °C at a constant pressure of 1 bar!
The change in enthalpy when 1 mol of ice is melted at 273K is 6008 J Heat Capacity of liquid water, Cp_{L} = 75.44 J/mol K Heat Capacity of solid water, Cp_{S} = 38J/mol K Enthalpy chage of melting at 273K, \Delta H_{273}=6008 J Calculate the standard enthalpy of fusion for ice. Calculate the heat released when 100 g of water supercooled at 250K solidify Initial T=25°C=298K Thanks
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).
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
i got this question wrong. the book previously said that the
units of entropy are J/(mol*K). you can get mol with the grams that
they gave, so why not use it?
Example: If, in a reversible process, 6.66 x 10 J of heat is used to change a 200 g block of ice to water at a temperature of 273 K, what is the change in the entropy of the system? (Note: The heat of fusion of ice = 333...
The constants for H2O are shown here: Specific heat of ice: sice=2.09 J/(g⋅∘C) Specific heat of liquid water: swater=4.18 J/(g⋅∘C) Enthalpy of fusion (H2O(s)→H2O(l)): ΔHfus=334 J/g Enthalpy of vaporization (H2O(l)→H2O(g)): ΔHvap=2250 J/g Part A How much heat energy, in kilojoules, is required to convert 73.0 g of ice at −18.0 ∘C to water at 25.0 ∘C ? Express your answer to three significant figures and include the appropriate units. 6.56 kJ is incorrect.
Gaseous H2O is condensed at 100°C and the liquid water is cooled to 0°C followed by freezing to solid water. What is the molar entropy change of the water? Consider the average specific heat of liquid water is 4.2 J/K g. The heat of vaporization at the boiling point and the heat of fusion at the freezing point at 2258.1 and 333.5 J/g, respectively.
13 V.7790 X 10° kg mo, and its vapor pressure is 489 Pa. 4.18 Calculate the molar Gibbs energy G of fusion when su- percooled water at -3 °C freezes at constant T and P. The en- thalpy of fusion of ice is 6000 J mol-1 at 0 °C. The heat capacities of water and ice in the vicinity of the freezing point are 75.3 and 38 JK- mol-, respectively. ion ate