Ammonia, NH3, is used as a refrigerant. At its
boiling point of –33 °C, the standard enthalpy of vaporization of
ammonia is 23.3 kJ/mol. What is the change in enthalpy when
53.1 g of ammonia is condensed at –33
°C?
-7.47 kJ | |
7.47 kJ | |
72.7 kJ | |
-72.7 kJ | |
-23.3 kJ |
Ammonia, NH3, is used as a refrigerant. At its boiling point of –33 °C, the standard...
The molar enthalpy of vaporization of NH3 is 23.3 kJ/mol at its normal boiling point of -33.3 °C. How much energy is required to evaporate 2.03 kg of ammonia at -33.3 °C?
Ammonia has a normal boiling point of -33.3 °C. Under a pressure of 2.00 atm, what is ammonia’s boiling point in °C? For ammonia ∆H vaporization = 23.3 kJ/mol.
The normal boiling point of ammonia is -33.3°C, and its enthalpy of vaporization is 23.35 kJ/mol. Calculate the temperature in °C required to double the vapor pressure of ammonia.
For ammonia, ΔHvap = 23.6 kJ/mol at its boiling point, -33 oC. Calculate the values for ΔS, q, w, and ΔE for the vaporization of ammonia at -33 oC and 1 atmosphere pressure.
Liquid ammonia (boiling point = -33.4 degrees Celsius) can be usedas a refrigerant and heat transfer fluid. how much energy is neededto heat 25.0 g of NH3 (liquid) from -65.0 degreesCelsius to -12.0 degrees Celsius ? specific heat capacity, NH3 (liquid) 4.7 J/ (g x k) specific heat capacity, NH3 (gas) 2.2J/ (g x k) heat ofvaporization 23.5 kJ/mol molarmass, 17.0 g/mol correct answer: 39 kJ please show me step by step how to solve this problem, i'm notgetting the correct answer...
The heat of vaporization of carbon disulfide is 27.4 kJ/mol at its boiling point of 46.3 °C. What is the change in enthalpy when 12.5 g CS2 condenses at 46.3 °C?
2.44 Ammonia gas is condensed at its boiling point at 1.013 25 bar at -33.4°C by the application of a pressure infinitesimally greater than 1 bar. To evaporate ammonia at its boiling point requires the absorption of 23.30 kJ mol-1. Calculate (a) Wrev per mole, (b) per mole, (c) AU, and (d) AH.
11) The enthalpy of vaporization of hydrogen sulfide, H2S, at its boiling point under standard pressure, -60.4°C, is 18.67 kJ/mol. What is the molar entropy of vaporization of H2S at that temperature (J/K mol)? (A) 0.088 (B) 87.7 (C) 269 (D) -87.7 (E) 18.7
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 normal boiling point of acetone [(CH3)2CO; MW 58.08 g/mol] is 56.1°C, and its molar enthalpy of vaporization is 29.1 kJ/mol. What is the molar entropy of vaporization of 72.3 g of acetone? molar ΔSvap = _____ J/(mol•K) What is the total entropy of vaporization of 72.3g of acetone? total ΔSvap = J/K