What is the change in entropy of 0.97 mol of liquid water at 0.0 degree C...
An ice tray contains 490 g of liquid water at 0°C. Calculate the change in entropy of the water as it freezes slowly and completely at 0°C. J/K
What is the entropy change of the universe (in J K-1)when 2.00 mol of liquid water at 0 °C freezes in a freezer compartment whose temperature is -15 °C? Assume the freezer is a perfect insulator. (AHfus = 6.01 kJ mol-1 for water) Select one: O a. +90.6 O b. +46.6 C. -2.6 O d. -44.0 o e. +2.6
An ice tray contains 750g of liquid water at 0C. A) Calculate the entropy change of water as it is cooled slowly from 30C to 0C. B) Calculate the change in entropy of the water as it freezes slowly and completely at 0C. The heat of fusion of water is 3.33*10^5 j/kg
Consider converting 1.50 mol of ice at - 25 degree C to liquid water at 55 degree C at 1 atm. What calculation would give the quantity of heat required by this process in J? The molar heat capacity of ice is 37.6 mol^-1 degree C^-1. The molar heat capacity of liquid water is 75.4 J-mol^-1 degree C^-1. The heat of fusion of water is 6.02 kJ mol^-1. (A) q = (1.50 mol) (6.02 kJ/mol) (1000 J/kJ) (B) q =...
What is the entropy change to the surroundings when 1 mol of ice melts in someone's hand if the hand temperature is 32°C? Assume a final temperature for the water of 0°C. The heat of fusion of ice is 6.01 kJ/mol. a. -188 J/K b. -22.0 J/K c. -19.7 J/K d. +19.7 J/K e. +188 J/K
The enthalpy of vaporization of water at 100.0°C is 40.75kJ/mol. What is the entropy change in the surroundings when one mole of water vapor condenses at 100.0°C in a large room maintained at a temperature of 39.00°C? (answer in J/K) Answer: 131 Check
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.
calculate change in entropy and change in enthalpy for freezing 1 mol of water at -10C and 1 atm. Cp,m is 75.3J/kmol for liquid water and 37.7J/Kmol for ice
What is the change in entropy when 0.145 mol of potassium freezes at 61.4°C (ΔHfus = 2.39 kJ/mol)? _______________J/K
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)