1) Form the following data for CH3CI T(°C) y (dynes/cm) pL (g/cc) pv (g/cc) 10 20 19.5 17.8 16.2 0.955 0.937 0.918 0.00599 0.00820 0.0110 b) Determine the constant k' in the Katayama equation and the critical temperature of the liquid using the data for temperatures 10 °C and 20 °C.
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- if ethanol has a vapor pressure of 0.08 bar and a molecular weight of 46 g/mol and water has a vapor pressure of 0.03 bar and a molecular weight of 18 g/mol. c) if the total pressure measured at these conditions is 0.02 bar, what can we conclude from the interaction between ethanol-water, respect to ethanol-ethanol and water-water? Justify your answer briefly.Steam pressures for pure CCl4 and SiCl4 are given as 0.4226 bar and 0.7999 bar respectively, while the temperature is 50°C. For a mixture prepared with these two liquids and boiling at 50°C under a pressure of 0.5333 bar, find the composition of the phases as a mole fraction and a mass fraction. [M(CCl4):153,82 g/mol, M(SiCl4):169,9 g/mol]Imagine that we have a closed system containing pure isobutane that is in a state of vapor-liquid equilibrium at known P sat < Pc. What can we say about mean translational kinetic energy of the molecules in the liquid (KL) and vapor (KV ) phases? a) KV − KL > 0 b) KV − KL < 0 c) KV − KL = 0 d) We need more information.
- Name two characteristic physical properties that distinguish condensed from gas phases, and one which distinguishes solid from liquid phases. Discuss the differences for each property. Name one colligative property and by an equation (label all variables) and 1-2 sentences the physical meaning. Consider a balloon. What thermodynamic system does it represent? How does this system interact with the environment? Calculate the heat capacity at constant pressure of methane for all its contribution and the total value according to the equipartition theorem. What is a more realistic value at room temperature? Why?Calculate the freezing point of water at 95 bar and 450 bar since the melting point of ice is 0⁰C and the melting enthalpy is 6.010 kJ/mol. (Accept that the densities of water in liquid and solid state are 0.997 G/ and 0.917 g/cm3 and remain constant.)What is w when 1.83 kg of H20(1), initially at 25.0 °C, is converted into water vapour at 185 °C against a constant external pressure of 1.00 atm? Assume that the vapour behaves ideally and that the density of liquid water is 1.00 g/ml (Remember to include a+or-sign as appropriate.) Enter your answer in acceptable SI units, accurate to 3. significant figures. Use an acceptable Sl symbol for units.
- A polynomial fit to measurements of the total volume of a binary mixture of A and B isv = 778.55 − 22.5749x + 0.568 92x2 + 0.010 23x3 + 0.002 34x4where v = V/cm3, x = nB/mol, and nB is the amount of B present. Derive an expression for the partial molar volume of B.Melting enthalpy of ice at 1 bar 9.134 kJ /mol; At 0 ° C, the density of water is 999.9 kgm-3, and the density of ice is 812.0 kg m-3. Assuming that the molar volume and enthalpy change in fusion are constant, find the freezing point of water at 85 bar using the informationgiven?The Prandtl number of common gases at 1 atm is about 1 for a very wide range of temperatures. Why is that so? Please explain.
- The vapour pressure of pyridine is 50.0 kPa at 365.7 Kand the normal boi ling point is 388.4 K. W hat is the enthalpyof vaporization of pyridine?The pressure of the saturated vapor of benzene (vapor in equilibrium with liquid) is 101.32 kPa at 80°C and 4.81 kPa at 5.5°C, respectively. The latter pressure and temperature correspond to the triple point of benzene. Calculate the approximate molar heat of vaporization ∆Hmv of benzene (Clausius - Clapeyron equation).Assume that at 298 K, 2.5 µmol (µ =micro) Ar(g) occupies 72 dm3 and grows to 100 dm3. Calculate the process's ΔG