> 4 NOg g) t 2. The istandaed gibbs yöre enetgy chenge KT/mot Change $2 this čcaction is -29.0 What is the value ck gibis ee ehety 350 K whens %3D 0-602. M, 0.305 M [No, ] = %3D O 021
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![2 N, Og g) -
2.
The istandaed gibbs yece enetgy chenge
KT/mot
Change $2 thins čcaction
is -29.0
what is the value ef gibis eee ehetg
350 K
when
%3D
0-602. M,
[No, ]
%3D
O. 021](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faf736ade-6837-42a5-a5df-ae4bf065fa04%2F5db996fe-01e7-44fe-ba66-0dfa4b0846e0%2F57ki9q9o_processed.jpeg&w=3840&q=75)
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- Calculate the molar concentration of FeSCN2+ in solution #3. The determined molar absorptivity of the solution at 448 nm is 333 L mol-1 cm-1.The mean activity coefficient in an 0.050 molKg-1 LaCl3 (aq) solutions is 0.303 at 25 o C. What is the percentage error in the value predicted by the debye – Huckel limiting law?The reaction A(g) + B(g) ↔ C(g) + D(g) has ΔGrxn° = -28.62 kJ mol-1 and Kp = 0.63 at 980 °C. A rigid cylinder at that temperature contains 1.2 atm of A, 0.20 atm of B, 0.30 atm of C, and 0.27 atm of D. What is the reaction Gibbs energy?
- Q: The concentration of the sulphate ion in a mineral water can be determinedby the turbidity which results from the addition of excess BaCl2, to a quantityof measured sample. A turbidometer used for this analysis has been standardisedwith a series of standard solutions of NaSO4. The following resultswere obtained:Standard solution Conc. (SO4)2− (mg/L) Reading of turbidometerS0 0.00 0.06S1 5.00 1.48S2 10.00 2.28S3 15.00 3.98S4 20.00 4.61i. In supposing that a linear relationship exists between the readings takenfrom the apparatus and the sulphur ion concentration, derive an equationrelating readings of the turbidometer and sulphate concentration(method of least squares).ii. Calculate the concentration of sulphate in a sample of mineral waterfor which the turbidometer gives a reading of 3.67.A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the freezing point of the solution(in C to 2 decimal places)A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the vapor pressure of the solution to 3 decimal places in atm.
- A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the osmotic pressure in atm to three decimal placesA solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the boiling point of the solution(in C to 2 decimal places)A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the following: Boiling point of solution (in °C to two decimal places) Freezing point of solution (in °C to two decimal places) Vapor pressure of the solution (in atm to three decimal places) Osmotic pressure (in atm to three decimal places)
- Sketch a plot of the fraction of species, f, vs pH for Tyr. Show your calculations for several points on the plot. You want to calculate the fraction of the species for more than 3 of the points. pKa’s for Tyr is 2.24, 9.04, and 10.10.Show that the equivalence point N1V1=N2V2 where V1mL of analyte of strength N1 reacts with V2L of o titrant of strength N2?Calculate the masses of (a) Ca(NO3)2 and, separately, (b) NaCI to add to a 0.150 mol kg-1 solution of KNO3(aq) containing 500 g of solvent to raise its ionic strength to 0.250.