Pa m3 mol K Use van't Hoff's Law (eq. 3.1) to calculate the osmotic pressure (in Pa) of a 0.185 molar solution of non-dissociating molecules at 40°C. Recall that R =8.314

The pressure-volume diagram for a pure substance (M=50 kg/kmol) is shown below. Use the phase diagram shown below to estimate density and molar volume of substance at critical point. P (MPa) 5 4 2 1 2 4 6 0.091 kg/m³, 550 m³/kmol 0.167 kg/m³, 300 m³/kmol 0.250 kg/m³, 200 m³/kmol 0.059 kg/m³, 850 m³/kmol 500 K 405 K 8 10 V (m³/kg) 12 14 620 K 16 18 20

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A high-altitude balloon contains helium, whose molar mass is 4.00 g/mol. At theballoon’s maximum altitude, its volume is 792 m3 and the outside temperatureand pressure are -53.0 °C and 5.00 kPa, respectively. Assume that the helium in theballoon is in equilibrium with the outside air temperature and pressure.(a) Use the ideal gas law to find the amount of helium in the balloon at maximumaltitude.(b) Assuming no loss of helium, what would be the volume of the balloon when itwas launched from the ground, where the air temperature and pressure are 20.0°C and 101 kPa, respectively?(c) If the volume of the balloon when it was launched was 65.0 m3, how many molesof helium were lost during the balloon’s ascent?

Consider the situation where a binary liquid mixture (assume ideal solution) is slowly cooled at constant pressure until it begins to solidify. At the phase equilibrium between the solution and crystal, the chemical potentials of the solvent in each phase must be equal: u** (T,P)= µ"(T,P)+ k;Tlnx ... Equation (1) X, L denotes the crystal and liquid phase, respectively. Since Au = µ*L **: | Aµ = -kgTlnx ... Equation (2) Can you apply Equation (2) at non-phase change temperatures? Why?

Answer only letter a

Question: A volatile molecule (Mw =60 g/mol) is located in a box at 60 °C. It is measured there was a mass loss of 1 g for 200s through a hole in the box. Vapor pressure of the molecule at 60 °C is 50 kPa. Calculate the diameter of the hole.

You have a calorimeter with 100 g of water at 22.6ᵒC and a 50.0 g piece of copper that you have heated to 98.7ᵒC. You place the copper in the water and wait for the temperature of the water to stop rising. What will be the highest temperature of the water? (Specific heats: water = 4.184 J/gᵒC, copper = 0.385 J/gᵒC )

1 mol of water solidifies at 95.0 oC and 1 atm.Calculate the (I) entropy of the sample, (II) entropy of the surroundings, (III) total entropy change for the following processes. Are these processes spontaneous?  Consult the table below.  You will need to use the fact that entropy is a state function to make these calculations.a.1 mol of water solidifies at -5.0 oC and 1atm b. 1 mol of water solidifies at 95.0 oC and 1 atm.