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3. The heat of vaporization of a compound is 512 kJ/mol. When 1.28 mol of this...
The heat of vaporization of CH_2CI_2 is 28.0 kJ/mol. Calculate the entropy the entropy change when 42 g of CH_2CI_2 boils at its boiling point of 39.8degreeC. 17 J/K 44J/K 59J/K 350J/K 700J/K
The vaporization of compound A is described by the following chemical equation. A(1) A(8) A rap(72.39 °C) = 38.21 kJ/mol Calculate the entropy of vaporization, Aswap, for A(l) at 25.0 °C given that the boiling point of A is 72.39 °C, and the molar heat capacity of A(l) is 119.09 J/mol K). Assume that the molar heat capacity of A(R) is 56.5% of that of A(1). ASP J. mol-K Calculate the standard enthalpy of vaporization. A Hap, for A(1) at...
Using the density, specific heat, and heat if vaporization of water from Appendix B, calculate the amount of energy required to vaporize 1.00 gal of water beginning with water at 15∘C. Express your answer to two significant figures. Density: 0.99987 g/mL at 0∘C. 1.00000 g/mL at 4∘C. 0.99707 at 25∘C. 0.95838 at 100∘C. Heat (enthalpy) of vaporization: 44.94 kJ/mol at 0∘C. 44.02 kJ/mol at 25∘C. 40.67 kJ/mol at 100∘C. Specific heat: 2.092 J/g-K= 2.092 J/gx∘C for ice at -3∘C. 4.184...
The heat of vaporization of benzene c6h6 , is 30.8 kJ/mol at its boiling point of 80.1 degrees Celsius. How much energy in the form of heat is required to vaporize 128 g benzene at its boiling point?
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.
Benzene has a heat of vaporization of 30.72 kJ/mol and a normal boiling point of 80.1 degrees C. At what temperature does benzene boil when the external pressure is 430 torr ? Express your answer in degrees Celsius using two significant figures.
3. A liquid compound has an enthalpy of vaporization equal to 65.0 kJ and an entropy of equal to 98 J/K at its boiling point. Calculate the boiling point of the compound. AH = 65 kJ AS - 987
The heat of vaporization of benzene, C6H6 is 30.7 kJ/mol at its boiling point of 80.1 C. How much energy in the form of heat is required to vaporize 132 g benzene at its boiling point? a) 0.302 kJ b) 51.9 kJ c) 24.2 kJ d) 40.1 kJ c) 4.05 x 10^3 kJ
OLLILEI UM ALLI LUUIU. Compound Melting point (°C) A Hus (kJ/mol) Boiling point (°C) AHvap (kJ/mol) HF -83.11 4.577 19.54 25.18 HCI -114.3 1.991 -84.9 17.53 HBO -86.96 2.406 -67.0 19.27 HI -50.91 2.871 -35.38 21.16 Using the data in the table, calculate AS tus and ASvap for HCL. Astus = AS = J/(K.mol) ASvap = J/(K.mol) Determine the entropy change when 5.70 mol HCI) melts at atmospheric pressure. AS = | J/K
The heat of vaporization of benzene (C6H6) is 30.77 kJ/mol at it's boiling point (80 C). As a liquid, it has a heat capacity of 134.8 J/mol*K, and as a gas it has a heat capacity of 82.4 J/mol*K. Calculate the enthalpy change of heating 245g of benzene from 50 C to 100 C.