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![Calculate the average partial molar volume (in cm³/mol) of MgSO4 in the interval [0.1, 0.2] mol of MgSO4 in water
solution.
T, P, n(water) is constant
1002.0
V/cm³ 1001.8.
0
0.2
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- Chloroform (1)/methyl ethyl ketone (2) form a solution in vapor liquid equilibrium at 330 K. The chloroform concentration in the liquid phase is x1 = 0.55. Assuming an ideal gas and an ideal solutionof liquids, what are y1 and P (in kPa), to 3 significant figures?The following evidence was obtained from an experiment to determine the solubility of calcium chloride at room temperature. A sample of saturated calcium chloride solution was evaporated to dryness, and the mass of solid residue was measured.EvidenceVolume of solution (mL) = 15.0Mass of empty beaker (g) = 90.54Mass of beaker and residue (g) = 101.36The solubility of calcium chloride is g/100 mLAn aqueous waste stream that has a maximum concentrationof 0.50 M H₂SO₄ (d=1.030 g/mL at 25C) will be neutralized by controlled addition of 40% caustic soda (NaOH; d=1.430 g/L) before it goes to the process sewer and then to the chemical plant waste treatment facility. However, a safety re-view finds that the waste stream could meet a small stream of animmiscible organic compound, which could form a flammable vapor in air at 40.°C. The maximum temperature of the causticsoda and the waste stream is 31°C. Could the temperature in-crease due to the heat of neutralization cause the vapor to ex-plode? Assume the specific heat capacity of each solution is 4.184 J/gK.
- Consider the following reaction: NH4Cl--->NH3(g)+HCl(g). The vapor pressure after dissasociation of a certain amount of NH4Cl is 608 kPa at 427 Celsius, but rises to 1115 kPa at 459 Celsius. Calclate Keq, deltarGstandard, and deltarHstandard, all at 427 Celsius. Assume that the vapor is an idela gas and that the enthalpy is indepednet of temperature in the range given.The solubility of ZnS(s) in water at a certain temperature is 1.4 × 10–11 mol/L, i.e., x or the [Zn+2]=[S-2]. The value of the Ksp of ZnS isIn an experiment to calculate the solubility product (Ksp) of barium nitrate (Ba(NO3)2), an excess amount of Ba(NO3)2 was added to 2 liters of water at 25oC until the solution is saturated. Because Ba(NO3)2 is only slightly soluble in water, the excess Ba(NO3)2 was filtered out to get a solid-free mixture. The proponents of the experiment thought about using the concept of colligative properties, specifically boiling point elevation, to determine Ksp. It was observed in their experiments that the solution boils at 100.15 K. Barium nitrate dissociates via the process: Ba(NO3)2(s) ⇄ Ba2+(aq) + 2NO?-3(?q) Ksp = [Ba2+][NO3−]2 Calculate the following if Kb,water = 0.51 K-kg/mol: a) Amount of Ba(NO3)2 dissolved in grams. Molar mass of Ba(NO3)2 = 261.3 g/mol b) Solubility product, Ksp c) Vapor pressure of the solution in kPa
- In an experiment to calculate the solubility product (Ksp) of barium nitrate (Ba(NO3)2), an excess amount of Ba(NO3)2 was added to 2 liters of water at 25oC until the solution is saturated. Because Ba(NO3)2 is only slightly soluble in water, the excess Ba(NO3)2 was filtered out to get a solid-free mixture. The proponents of the experiment thought about using the concept of colligative properties, specifically boiling point elevation, to determine Ksp. It was observed in their experiments that the solution boils at 100.15 K. Barium nitrate dissociates via the process: ?a(??3)2(?) ⇄ ??2+(?q) + 2??-3(?q) ??p = [??2+][??3−]2 Calculate the following if Kb,water = 0.51 K-kg/mol: a) Amount of Ba(NO3)2 dissolved in grams. Molar mass of Ba(NO3)2 = 261.3 g/mol b) Solubility product, Ksp c) Vapor pressure of the solution in kPaA 1.00-m solution of acetic acid, CH3COOH, in benzene has a freezing point of 2.96°C. Use the data in the Table to calculate the value of i and suggest an explanation for the unusual result. (Hint: If i is less than 1.0, each formula unit that dissolves yields less than one solute particle, an outcome suggesting aggregation of solute particles.) Answer is: i = 0.50; formation of dimers of composition (CH3COOH)2, need steps shown to understand thoughIdentify the effect of the condition on the indicated parameter. Write increase, decrease, or no effect , and provide an explanation. The test tube used in the determination of the ΔHrxn for nitric acid was still wet with water. [ magnitude of ΔHrxn].
- What is the state of the system that has the following pressures: Pbubble = 80 kPa Psystem = 50 kPa Pdew = 40 kPa i.e. Pbubble > Psystem > PdewIn lecture I mentioned that standard state is usually at 25oC; however, it can be at any specified temperature. In problems 9 and 10 you will calculate ΔGo from Ksp data. The Ksp range over the temperature range in these two problems is consistent with some actual solubility data; however, in order to allow each student to do their own calculation I have made this data for an "unknown" ionic solid. Calculate the value of ΔGo (kJ/mol) at 3.3oC for the dissolution of an ionic solid with a Ksp of 2.5 x 10-11 at 3.3oC. Your answer should have 2 sig figs.Maple water is concentrated using the reverse osmosis process. What pressure (in kPa) must be imposed to obtain maple water with a mass percentage of 21.10%m/m and a density of 1.088 g/mL?The temperature is then 24.35 °C Note: sucrose is not an electrolyte and it is assumed that maple water consists only of sucrose and water. The molar mass of sucrose is 342.30 g/mol. Note: The density of pure water is 1.000 g/mL.R = 8.3145 kPa-L-mol-1-K-10 K = -273.15 °C