Cr (Na Cr (Na)( cr cr (Na Na Cr(Na)(cr . The process of dissolution of NaCI(s) in H,O() is represented in the diagram above. Which of the following summarizes the signs of AH® and AS for each part of the dissolution process? Breaking solvent-solvent Breaking solute-solute Forming solute-solvent interactions interactions interactions ΔΗ AS AS ΔΗ AS (A) (B) (C) (D)

Cr (Na Cr (Na)( cr cr (Na Na Cr(Na)(cr . The process of dissolution of NaCI(s) in H,O() is represented in the diagram above. Which of the following summarizes the signs of AH® and AS for each part of the dissolution process? Breaking solvent-solvent Breaking solute-solute Forming solute-solvent interactions interactions interactions ΔΗ AS AS ΔΗ AS (A) (B) (C) (D)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter11: Properties Of Solutions

Section: Chapter Questions

Problem 70E: The vapor pressures of several solutions of water-propanol (CH3CH2CH2OH) were determined at various...

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Using KF as an example, write equations that refer to Hsoln and Hhyd Lattice energy was defined in Chapter 3 as H for the reaction K+(g) + F (g) KF(s). Show how you would utilize Hesss law to calculate Hso1n from Hhyd and HLE for KF, where HLE = lattice energy. Hsoln for KF, as for other soluble ionic compounds, is a relatively small number. How can this be since Hhyd and HLE are relatively large negative numbers?
The vapor pressures of several solutions of water-propanol (CH3CH2CH2OH) were determined at various compositions, with the following data collected at 45C: H2O Vapor pressure(torr) 0 74.0 0.15 77.3 0.37 80.2 0.54 81.6 0.69 80.6 0.83 78.2 1.00 71.9 a. Are solutions of water and propanol ideal? Explain. b. Predict the sign of Hsoln for water-propanol solutions. c. Are the interactive forces between propanol and water molecules weaker than, stronger than, or equal to the interactive forces between the pure substances? Explain. d. Which of the solutions in the data would have the lowest normal boiling point?
Which solute has the greatest effect on the boiling pointof 1.00 kg of water: 50.0 g of strontium chloride (SrCl2) or 150.0 g of carbon tetrachloride (CCl4) ? Justify youranswer.
The dissolution of NH4 ClO4(s) in water is endothermic with Delta H solution =33.5 kf/mol. if you prepare a 1.00 m solution of NH4ClO4 beginning with water at 25 ° C what is the final temperature of the solution in ° C ? Assume that the specific heats of both pure water and the solution are the same , 4.18J/g.K.
In an coffee cup calorimeter experiment, sodium hydroxide (7.17 g) was dissolved in water (86.6 g). The initial temperature of both were 11.5 oC. When the sodium hydroxide is dissolved, the solution reached a maximum temperature of 34.1 oC. The specific heat of the solution is 3.98 J∙g -1∙ oC -1. Use NaOH as the limiting reactant, calculate the molar enthalpy change of the solvation of NaOH in water (Δ Hrxn), in the unit of kJ/mole
f dissolving 1.5 g of a solute into 100 mL of water caused the temperature of the solution toincrease by 4.7 ⁰C, what would the change of temperature be if 3.0 g of the solute were dissolvedin the same volume of water? Explain.
If 124.4 mL of water is shaken with oxygen gas at 0.81atm, it will dissolve 0.0036 g O2. Estimate the Henry's law constant for the oxygen gas in water in units of g mL ^-1atm^-1.
A student using a calibrated solution calorimeter measured a temperature decrease of 1.10 K when 1.00 g of KNO3 was added to 74.40 g of deionized water in the calorimeter. The specific heat capacity of the solution calorimeter was found to be 4.15 J/gK. Calculate the experimental value of the molar heat of solution of KNO3, ΔH soln. Was the dissolution of this salt exothermic or endothermic?
Which one statement in italics is NOT correct? Other given information is correct. a. The condensation of steam of liquid water is exothermic. b. When 1 mole of NH4NO3 dissolves in water, the temperature of the water decreases. This dissolution process is endothermic. c. The enthalpy change for freezing 1 mol of wter is -6.0 kJ. This process is exothermic. d. 1 mol of Ca + 1 mol Br2 has a higher enthalpy than 1 mole CaBr2. Thus, the combination reaction of calcium with bromine to give calcium bromide is exothermic. e. When sodium bicarbonate decomposes, heat is absorbed from the surroundings. Thus, the decomposition of sodium bicarbonate is exothermic.
Magnesium citrate, Mg3(C6H5O7)2, belongs to a class of laxativescalled hyperosmotics, which cause rapid emptying of the bowel.When a person consumes a concentrated solution of magnesium citrate, it passes through the intestines, drawing water and promotingdiarrhea, usually within 6 hours. Calculate the osmotic pressure ofa magnesium citrate laxative solution containing 28.5 g of magnesium citrate in 235 mL of solution at 37°C (approximate body temperature). Assume complete dissociation of the ionic compound.
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