When water is supercooled, it freezes at a temperature below 0.0°C. If 10.9 KJ of heat is released when 2.00 mol of supercooled water at -15.0°C freezes, calculate the molar enthalpy of fusion for ice at 0.0°C and 1 atm. (Assume the molar heat capacities for H2O(s) and H2O(1) to be temperature independent and are 37.5 J/K mol and 75.3 J/K-mol, respectively)

When water is supercooled, it freezes at a temperature below 0.0°C. If 10.9 KJ of heat is released when 2.00 mol of supercooled water at -15.0°C freezes, calculate the molar enthalpy of fusion for ice at 0.0°C and 1 atm. (Assume the molar heat capacities for H2O(s) and H2O(1) to be temperature independent and are 37.5 J/K mol and 75.3 J/K-mol, respectively)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The enthalpy of vaporization of Substance X is 7.00 Round your answer to 2 significant digits. atm П x10 X kJ and its normal boiling point is -125. °C. Calculate the vapor pressure of X at -184. °C. mol
The normal boiling point of liquid acetone is 329 K. Assuming that its molar heat of vaporization is constant at 29.0 kJ/mol, the boiling point of CH3COCH3 when the external pressure is 1.29 atm is | K.
The vapor pressure of water is 41.1 atm at 274.1 K, and the vapor pressure of water is 71.4 atm at 704.3 K. Calculate the enthalpy of vaporization in kJ/mol.
300 °C. Using the following information, determine the vapor pressure of water at H₂0 at T = 179.88 degrees C the vapor pressure is PSAT = 10 bar. The enthalpy of vaporization is 2014.59 kJ/kg W = 0.1944 m³/kg V¹ = 0.001127 m³/kg
Two 20.0 g ice cubes at −16.0 ∘C are placed into 225 g of water at 25.0 ∘C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. heat capacity of H2O (s) 37.7 J/(mol⋅K) heat capacity of H2O (l) 75.3 J/(mol⋅K) enthalpy of fusion of H2O 6.01 kJ/mol Tf= ________∘C
Based on the thermodynamic properties provided for water, determine the amount of energy released for 50.00 g of water to go from 62.0 °C to -17.0 °C. Property Melting point Boiling point 12.3 AHfus Hvap Cp (s) Cp (1) Cp (g) kJ Value 0.0 100.0 6.01 40.67 37.1 75.3 33.6 Units. °C °C kJ/mol kJ/mol J/mol · °C J/mol · °C J/mol °C
kJ The enthalpy of vaporization of Substance X is 5.00 and its normal boiling point is -66. °C. Calculate the vapor mol pressure of X at -87. °C. Round your answer to 2 significant digits. || atm x10
An ice cube with a mass of 45.4 g at 0.0 °C is added to a glass containing 374 g of water at 45.0 °C. Determine the final temperature of the system at equilibrium. The specific heat capacity of water, C, is 4.184 J/g.°C, and the standard enthalpy of fusion, AH; , of water is 6.01 × 10° J/mol. Assume that no energy is transferred to or from the surroundings. fus T = °C TOOLS x10 Question Source: Atkins 7e - Chemical Principles| Publisher: W.H. Fre
The heat of fusion of Hg at its normal melting point of -38.9°C is 2.82 calg^-1. The densities of solid and liquid mercury at 1 atm and at that temperature are 14.193 and 13.690 gcm^-3, respectively. Find its melting point at 200 atm.
Ethanol, with ΔHvap = 40.5 kJ mol-1, has a higher ΔHvap than methanol, which is 35.2 kJ mol-1, due to its larger size and greater intermolecular forces. Because the ΔHvap for ethanol is larger, we would expect that for the two liquids to reach the same vapor pressure, the temperature for ethanol would have to be higher. If the vapor pressure is 0.0992 atm at 27.3 °C, what would the temperature be when the vapor pressure is 4.52 atm?
Please don't provide handwritten solution .....