The vapor pressure of a pure substance is measured at a variety of temperatures.
ID: 981218 • Letter: T
Question
The vapor pressure of a pure substance is measured at a variety of temperatures. Based upon the experimental data below, calculate the heat of vaporization for this substance.
P in mm Hg 3800 7600 15200
T in °C 113.0 144.5 181.0
2. What is the atomic weight of an element that crystallizes in a body-centered cubic unit cell? It has an atomic radius of 2.65 Å and a density of 1.93 g/cm3.
3. The solubility limit of ammonium acetate, NH4C2H3O2 is 143 g/100g H2O at 20°C. Explain fully what you would observe as you add 230.0 g of NH4C2H3O2 to 150. grams of water at 20°C.
4. What is the concentration in mole fraction of solute of a 1.05M aqueous solution of potassium nitrate, KNO3? The density of the solution is 1.06 g/mL.
5. Explain on a molecular basis why a solution made from a solvent and a non-volatile solute would have a lower vapor pressure than the pure solvent. Keyboard Shortcuts
Explanation / Answer
1)
Apply clasisu clapeyron equation
ln(P2/P1) = H/R*(1/T1-1/T2)
solve for H
H = R*(ln(P2/P1))/(1/T1-1/T2)
H = (8.314)(ln(15200/7600)/(1/(144.5+273) - 1/(181+273)) = 29926.4325909 J/mol
H = 29.926 kJ/mol
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