What is the freezing point of an alcohol in °C to the nearest degree if its...
Ethyl alcohol has a boiling point of 78.0 degree C, a freezing point of -114 degree C, a heat of vaporization of 879 kJ/kg, a heat of fusion of 109 kJ/kg, and a specific heat of 2.43 kJ/kg-K. How much energy must be removed from 0.567 kg of ethyl alcohol that is initially a gas at 78.0 degree C so that it becomes a solid at -114 degree C?
Ethyl alcohol has a boiling point of 78.0 ˚C, a freezing point of -114 ˚C, a heat of vaporization of 879 kJ/kg, a heat of fusion of 109 kJ/kg, and a specific heat of 2.43 kJ/kg·K. How much energy must be removed from 0.689 kg of ethyl alcohol that is initially a gas at 78.0 ˚C so that it becomes a solid at -114 ˚C?
Ethyl alcohol has a boiling point of 78.0 ˚C, a freezing point of -114 ˚C, a heat of vaporization of 879 kJ/kg, a heat of fusion of 109 kJ/kg, and a specific heat of 2.43 kJ/kg·K. How much energy must be removed from 0.683 kg of ethyl alcohol that is initially a gas at 78.0 ˚C so that it becomes a solid at -114 ˚C?
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).
Chapter 18, Problem 039 Ethyl alcohol has a boiling point of 78.0 °C, a freezing point of -114 °C, a heat of vaporization of 879 kJ/kg, a heat of fusion of 109 kJ/kg, and a specific heat of 2.43 kJ/kg K. How much energy must be removed from 0.765 kg of ethyl alcohol that is initially a gas at 78.0 °C so that it becomes a solid at -114 C? Number Units the tolerance is +/-2%
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
Question 5 Ethyl alcohol has a boiling point of 78.0 °C, a freezing point of -114 °c, a heat of vaporization of 879 kJ/kg, a heat of fusion of 109 kJ/kg, and a specific heat of 2.43 kJ/kg-K. How much energy must be removed from 0.539 kg of ethyl alcohol that is initially a gas at 78.0 °C so that it becomes a solid at -114 °C? Number Units the tolerance is +/-2% This answer has no units SAVE FOR...
Ethyl alcohol has a boiling point of 78.0 degrees Celsius, a freezing point of -114 degrees Celsius, a latent heat of vaporization of 879 kJ/K, a latent heat of fusion of 109 kJ/K, and a specific heat of 2.43 kJ/kg.K. How much energy must be removed from 0.510 kg of ethyl alcohol that is initially a gas at 78.0 degrees Celsius so that it becomes a solid at -114 degrees Celsius?
Calculate the change in entropy that occurs in the system when 1.56 mol of isopropyl alcohol (C3H8O) melts at its melting point (-89.5 ∘C). Heat of fusion is 5.37 kJ/mol.
For ethanol, C2H5OH, the heat of fusion at its normal melting point of -115 °C is 5.0 kJ/mol. The entropy change when 1.84 moles of solid C2H5OH melts at -115 °C, 1 atm is J/K.