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The molar solubility of lead(II) iodide, PbI2(s), is 1.45 x 10-3 M at 20 oC and 6.85 x 10-3 M at 80 oC. A. (2 pts.) What is the Ksp of PbI2(s) at 20 oC? B. (2 pts.) Determine the Ksp at 80 oC. C. (3 pts.) Use the information from parts A and B to determine the ?Ho. D. (3 pts.) What is ?So for this reaction at 20 oC? E. (2 pts.) Calculate the value of ?Go from your obtained enthalpy and entropy values at 20 oC. F. (2 pts.) At what temperature range is this dissociation spontaneous? Problem #1 continued on next page... G. (3 pts.) Determine the value of Gibbs Free Energy at 20 oC when [Pb+2] = 4.1 x 104 M and [I-] = 5.2 x 103 M. Do these conditions make this reaction more or less spontaneous at this temperature? Briefly explain. H. (2 pts.) In what ways does the Debye-Hückel limiting law provide a more accurate determination of the solubility product constant for PbI2(s)? Briefly explain. I. (3 pts.) A separate experiment is conducted in which 4.82 x 10-5 M CaI2(aq) is added to a solid solution of PbI2 at 20 oC. Qualify how the molar solubility changes. Does this addition favor the dissociation of the solid? Briefly explain. J. (4 pts.) Finally, in another experiment, a student mixes 40.0 mL of 3.00 M Pb(NO3)2(aq) with 20.0 mL of 2.00 x 10-3 M NaI(aq) at 20 oC. Does PbI2(s) precipitate from the solution? Briefly explain why or why not.
Calculate the final temperature when a 29.0 gram sample of ice at 0oC is placed into a styrofoam cup containing 115 grams of water at 75.7 oC. Assume that there is no loss or gain of heat from the surroundings.
how much current is produced by the dissolution of .525 g of chromium per hour to produce chromium (III)?
a 45-g piece of ice at 0 degrees C is added to a sample of water at 9 degrees C. All of the ice melts and the temperature of the water decreases to 0 degrees C. How many gram sof water were in the sample?
A sample of neon has a volume of 470 mL when it is at a pressure of 685 mmHg. What will be the volume when the pressure is increased to 1212 mmHg?
A mixture was prepared with the following initial concentrations: [CO] =0.20M, [H2O] = 0.30 M. No formic acid, HCHO2, was initially present. What was the equilibrium concentration of HCHO2?
The molar mass of the compound is 303.8 g/mol and the molar masses of C, O, and Ag are 12.-1 g/mol, 16.00 g/mol, and 107.9 g/mol, respectively. Determine the empirical and molecular formula of the compound.
Suppose the energy level of an electron with quantum number n was proportional to n instead of 1/n^2, E= -2.18 x 10^-19 J
A solution that has a K+ concentration of 5.00ppm is to be prepared from solid KCl. Assuming a solution density of1.000g/mL how many miligrams of KCl must be added to make 1.00L solution?
what is the volume of 45.6g of silver if the density of silver is 10.5g/ml?
Metallic magnesium can be made by the electrolysis of molten MgCl2. What mass of Mg is formed by passing a current of 6.40 A through molten MgCl2 for 4.90 days?
Which of the following has only a single peak in the proton NMR spectrum
If 2.00 g of Mg reacts completely with 50.0 mL of HCI solution, what is the molarity of the HCI solution?
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