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At the triple point of a substance, the vapor pressures of the solid and the liquid phase are the same. Using the Clausius-Clapeyron equation for each combination of phases, one can show that the temperature of the triple point,
where the data points (
(a) Given these data, calculate
(b) Calculate the vapor pressure of
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Chapter 6 Solutions
Physical Chemistry
- What is the enthalpy change when a 1.00-kg block of dry ice, CO2(s), sublimes at 78 C? The enthalpy of sublimation of CO2(s) is 26.9 kJ/mol. Is this process exothermic or endothermic?arrow_forwardPredict which liquid—glycerol, HOCH2CH(OH)CH2OH, or hexane, C6H14—has the greater surface tension. Explain your prediction.arrow_forwardWhat mass (g) of ethanol, CH3CH2OH(), can be vaporized at its boiling point of 78.4 C by transfer of 500. kJ to the liquid? The vapH of ethanol is 38.6 kJ/mol at this temperature.arrow_forward
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- Estimating Temperature (or Vapor Pressure) For benzene (C6H6), the normal boiling point is 80.1 °C and the enthalpy of vaporization is 30.8 kJ/mol. What is the boiling point of benzene in Denver, where atmospheric pressure = 83.4 kPa? 101.325 kPa In P₁ P2 AHvap 1 R T₂ T₁ P₁ = 1.00 atm x 101.325 kPa/atm T₁ = 80.1 °C + 273.15 = 353.25 K 1 In 101.325 83.4 P₂ = 83.4 kPa P2 AHvap = 3.08 x 104 J/mol = 3.08 x 104 8.314 1 T2 R = 8.314 J/mol K 1 353.25 - => 0.19468 = 3.7046 x 103 (1/T2 - 2.831 x 10-3) 5.2551 x 10-5 = 1/T₂ - 2.831 x 10-³ 2.8836 x 10-3 = 1/T₂ T₂ = 346.8 K = 73.6 °C T2arrow_forwardThe temperature dependence of the vapor pressure of solid sulfur dioxide can be approximated by log(p) = 10.5916 – 1871.2/T, with p in Torr and T in K. The temperature dependence of the vapor pressure for liquid sulfur dioxide is given by log(p) = 8.3186 – 1425.7/T. Determine the temperature and pressure at the triple point.arrow_forwardFind the enthalpy of vaporization, ΔHvap.arrow_forward
- The triple point for water is T=273.16 K, P=611 Pa. At this temperature, the heat of vaporization is ∆(g,l)H = 45.05 kJ/mol and heat of fusion is ∆(l,s) H =6.01 kJ/mol. In a cold and dry morning the winter (T=268.15 K, vapor pressure of water is 266.6 Pa), will you see some frost?arrow_forwardHow long would it take to convert 100.0 grams of solid sodium at 20.0°C to sodium vapor at 1000.0°C if the heating rate at a pressure of one atm is 8.0 kJ?min–1? The melting point of sodium is 97.8°C; its boiling point is 883°C; its molar enthalpy of fusion is2.60 kJ?mol–1; its molar enthalpy of vaporization is 97.4 kJ?mol–1; and the heat capacities of solid, liquid, and gaseous sodium are 28.2 J?mol–1?K–1, 30.8 J?mol–1?K–1, and 20.8 J?mol–1?K–1, respectively. Answer: 70 mins, but i need the steps.arrow_forward
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