Estimate the normal boiling point of PCl3. dH (formation) PCl3(l)= -319.7kJ/mol; S(not delta) of PCl3(l)= 217.1J/mol K
Estimate the normal boiling point of PCl3. dH (formation) PCl3(l)= -319.7kJ/mol; S(not delta) of PCl3(l)= 217.1J/mol...
196 The normal boiling point of Br2(l) is 58.8 ∘C, and its molar enthalpy of vaporization is ΔHvap = 29.6 kJ/mol. a) When Br2(l) boils at its normal boiling point, does its entropy increase or decrease? b) Calculate the value of ΔS when 1.50 mol of Br2(l) is vaporized at 58.8 ∘C. ΔS= (answer in J/K)
The normal boiling point of Br2(l) is 58.8 ?C, and its molar enthalpy of vaporization is ?Hvap = 29.6kJ/mol. Part A When Br2(l) boils at its normal boiling point, does its entropy increase or decrease? When boils at its normal boiling point, does its entropy increase or decrease? increase decrease SubmitMy AnswersGive Up Part B Calculate the value of ?S when 2.00mol of Br2(l) is vaporized at 58.8 ?C.
Consider the following data for compound A: (delta)Hf(kj/mol) S(J/K*mol) A(s) -224.57 32.36 A(l) -172.45 109.55 Use these data to determine the normal freezing point of compound A. Report your answer to 3 significant figures and degrees Celsius) Freezing point =
The normal boiling point of CS2(l) is 319k. It's triple point is at (T,p) = ( 161K, 3.2pa). Estimate the enthalpy of vaporization of CS2.
The normal boiling point of Br2(l) is 58.8 ∘C, and its molar enthalpy of vaporization is ΔHvap = 29.6 kJ/mol. Calculate the value of ΔS when 4.00 mol of Br2(l) is vaporized at 58.8 ∘C.
The normal boiling point of methanol is and the molar enthalpy of vaporization if 71.8 kJ/mol. The value of S when 1.75 mol of vaporizes at 64.7 °C is 0.372 4.24 × 107 372 1.94 × 103 1.
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.
Use the thermodynamic data provided below to estimate the boiling point (in K) of V. Report your answer to zero decimal places in standard notation (i.e. 123. kJ *For numbers ending in zero, be sure to include the decimal!*). Substance ΔH°f (kJ/mol) S° (J mol-1K-1) V (l) 17.3 36.1 V (g) 515.5 182.3
Use the thermodynamic data provided below to estimate the boiling point (in K) of CCl4. Report your answer to zero decimal places in standard notation (i.e. 123. kJ *For numbers ending in zero, be sure to include the decimal!*). Substance ΔH°f (kJ/mol) S° (J mol-1K-1) CCl4 (l) -128.4 214.4 CCl4 (g) -96 309.6
Estimate the boiling point elevation of 0.39 m NaCl(aq), assuming it undergoes complete dissociation. The boiling point constant of water is 0.51 K · kg/mol. Answer in units of ◦C.