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3. The normal boiling point for the chloro-fluoro- hydrocarbon C,C1,F3 is 47.6°C: C C1,F3(1) C_C1zFz (g)...
The fluorocarbon compound C2Cl3F3 has a normal boiling point of 47.6 ∘C. The specific heats of C2Cl3F3(l) and C2Cl3F3(g) are 0.91 J/g⋅K and 0.67 J/g⋅K, respectively. The heat of vaporization for the compound is 27.49 kJ/mol. Calculate the heat required to convert 45.5 g of C2Cl3F3 from a liquid at 14.10 ∘C to a gas at 78.40 ∘C. Express your answer using two significant figures.
Calculate the entropy change (J/K) for the vaporization of 14.4 g of a hydrocarbon (88 g/mole]), at its boiling point of 86.8°C. The enthalpy of vaporization of this hydrocarbon is 25.1 kJ/mol. Enter to 2 decimal places.
The following information is given for ether, C2H30C2H5, at 1 atm: boiling point = 34.6 °C AH ap(34.6 °C) = 26.5 kJ/mol melting point =-116 °C AH fus(-116 °C) = 7.27 kJ/mol specific heat liquid = 2.32 J/gºC At a pressure of 1 atm, kJ of heat are needed to vaporize a 35.6 g sample of liquid ether at its normal boiling point of 34.6 °C.
The flourocarbon compound C2Cl3F3 has a normal boiling point of 47.6oC. The specific heats of C2Cl3F3(l) and C2Cl3F3(g) are 0.91 J/g-K and 0.67 J/g-K, respectively. The heat of vaporization for the compound is 27.49 kJ/mol. Calculate the heat required to convert 50.0 grams of C2Cl3F3 from a liquid at 10 degrees Celcius to a gas at 85 degrees celcius.
The fluorocarbon compound C_2CI_3F_3 has a normal boding point of 47.6 degree C The specific heats of C_2Cl_3F_3(l) and C_2Cl_3F_3(g) are 0 91 J/g middot K and 0.67 J/g middot K, respectively The heat of vaporization for the compound is 27 49 kJ/mol. Calculate the heat required to convert 73.0 g of C_2CI_3F_3 from a liquid at 10.10 degree C to a gas at 81 90 degree C. Express your answer using two significant figures.
ID: 10. Identify the place which has the highest boiling point of water, a Death Valley, 282 feet below sea level b. A pressurized passenger jet, 39,000 feet C. Panama City, Florida, sea level d. Mt. Everest, 29,035 feet c. Denver, Colorado, 5,280 feet d. Minha City, Florcnger jet. c. Der Everest, 29 onda, sea le 39,000 feet 11. The heat of vaporization of water at 100°C is 40.66 kJ/mol Calculate the quantity of heat that is absorbed released when...
What is the entropy change of the system when 17.5 g of liquid benzene (C6H6) evaporates at the normal boiling point? The normal boiling point of benzene is 80.1�C and ?H vap is 30.7 kJ/mol. �19.5 J/K +85.9 J/K 25.2 J/K +19.5 J/K
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
1) When 1336 J1336 J of heat energy is added to 47.6 g47.6 g of hexane, C6H14,C6H14, the temperature increases by 12.4 ∘C.12.4 ∘C. Calculate the molar heat capacity of C6H14. 2) Liquid sodium is being considered as an engine coolant. How many grams of liquid sodium (minimum) are needed to absorb 9.20 MJ9.20 MJ of energy in the form of heat if the temperature of the sodium is not to increase by more than 10.0 °C?10.0 °C? Use CP=30.8...
1a) Consider the following reaction: 3 C(s) + 4 H2(g) → C3H8(g); ΔH° = –104.7 kJ; ΔS° = –287.4 J/K at 298 K What is the equilibrium constant at 298 K for this reaction? Report answer to TWO significant figures. 1b) Τhe enthalpy of vaporization of ammonia is 23.35 kJ/mol at its boiling point (–33 °C). Calculate the value of ΔSsurr when 1.00 mole of ammonia is vaporized at –33 °C and 1.00 atm. Report answer to THREE significant figures.