The enthalpy of vaporization of water at 100 0°C is 40.43 kJ/mol. What is the entropy...
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
Please answer 12-17 and show work. I’m not sure which equations to use 15. The gas above the liquid in a sealed bottle of soda is primarily carbon dioxide. Carbon dioxide is also dissolved in the soda. When the distribution of carbon dioxide between the gas and liquid is hase , , at equilibrium, molecules ofcarbon dioxide in the gas phase can stilldissolve in the iquid they strike the surface and are captured. Similarly, molecules of carbon dioxide can escape...
Thermodynamics 1) The enthalpy of vaporization of water ∆H = -25 kJ mol-1 at T = 45 °C. When water V = 15 cm3 in an open vessel evaporates at this temperature, calculate the change in entropy of the surroundings. 2) For a given reaction, ∆H = 25 kJ and ∆S = 50 J/K. Above what temperature will this reaction occur spontaneously? 3) At T = 15°C a certain protein denatures reversibly with ∆H = 30 kJ/mol. The system is...
the normal boiling point of ethanol is 78.3 deg C and its molar enthalpy of vaporization is 38.56 Kj/mol. what is the change in entropy in the system in J/k when 97.2 grams of ethanol at 1 atm condenses to a liquid at the normal boiling point?
The enthalpy and entropy of vaporization of ethanol are 38.6 kJ/mol and 109.8 J/mol-K, respectively. What is the vapor pressure of ethanol at 25℃?
What is the entropy change in the surroundings when one mole of ice melts at 0.00'C in a large room maintained at 27.0°C? The heat of fusion of ice is 6.31 kJ/mol (answer in 1/K) Answer: 21.0 Check Finis
The Standard enthalpy of vaporization of water at 100.0 oC is 40.66 KJ*mol-1. The Cp,m values for the liquid and the vapor water are, respectively, 75.3 and 33.58 J*K-1*mol-1. Assume that the heat capacities are independent of temperature, and that the vapor behaves as an ideal gas. a) Calculate sys in taking one mole of liquid water at 25.0 oC and 1.00 atm to gaseous water at 95.0 oC and 0.500 atm. b) Assume that the temperature and pressure of...
Liquid nitrogen has a measured enthalpy of vaporization ( ΔH^o vap) = 2.79 kJ/mol and entropy of vaporization ( Δ S^ovap) = 36.1 J/K mol. Calculate the boiling point of liquid nitrogen, in oC using this information. (Use 273.15 K = 0 oC for the temperature conversion. Report your answer with three significant figures.) Tvap = ????? °C I got 196^oC but it is incorrect.
What is the entropy change in the surroundings when one mole of ice melts at 0.00°C in a large room maintained at 19.0°C7 The heat of fusion of ice is 6.11 kl/mol. (answer in 1/K Answer: 22.4 Check
the heat of vaporization of water at 100*c is 40.66 kj/mol. calculate the quantity of heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100*c