ytrios.colenIcan.com/5ar05a7aa8cte/3542523?X-Blackboard-Expiration=16143732000008X-B1 / 1100%Using the Lattice Enthalpy and the Hydration Enthalpy to find the Enthalpy of Solution(AHSOLUTION)Figuring out if an ionic compound is more or less soluble with temperature basedon the sign of its AHSOLUTION(1) NazSO4 (s)->2 Na+ (g) + SO?- (g)AH = AH1 = 1944 kJ/mol(2) 2 Nat (g) + S02 (g)->2 Na+ (aq) + S0,2- (aq) AH= AH2 = -1947 kJ/molWhat is the name given to AH1? (Fill in the blank)(a)(b)TheEnthalpyExplain the sign of AH1.(c)(d)What is the name given to AH2 for this ionic compound? TheEnthalpyExplain the sign of AH2.Use the two chemical equations given here with their corresponding AH's to findAHSOLUTION for NazSO4. Would this compound be soluble in water? How do you know?(e)(29isonicMasterf6f7).(f8f10f12

Enthalpy is the heat content of a system at constant pressure.

1 / 1 100% Using the Lattice Enthalpy and the Hydration Enthalpy to find the Enthalpy of Solution (AHSOLUTION) Figuring out if an ionic compound is more or less soluble with temperature based on the sign of its AHSOLUTION (1) NazSO4 (s) -> 2 Nat (g) + SO2- (g) AH= AH1 = 1944 kJ/mol %3D (2) 2 Na* (g) + SO,2 (g) -> 2 Na+ (aq) + SO, (aq) AH =AH2 = -1947 kJ/mol %3D

1 / 1 100% Using the Lattice Enthalpy and the Hydration Enthalpy to find the Enthalpy of Solution (AHSOLUTION) Figuring out if an ionic compound is more or less soluble with temperature based on the sign of its AHSOLUTION (1) NazSO4 (s) -> 2 Nat (g) + SO2- (g) AH= AH1 = 1944 kJ/mol %3D (2) 2 Na* (g) + SO,2 (g) -> 2 Na+ (aq) + SO, (aq) AH =AH2 = -1947 kJ/mol %3D

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

6. Ethylene glycol [CH₂(OH)CH₂(OH)] is a common automobile antifreeze. It is water soluble and fairly nonvolatile (b.p. 197°C). Calculate (a) the freezing point and (b) the boiling point of a solution containing 268 g of ethylene glycol in 1015 g of water.
You are asked to make a aqueous solution of Calcium Chloride, CaCl2 If you add 1 grams of CaCl2to 250 ml of water at a T = 20 °C with a molecular weight of 111 g/mole and a solubility/saturation concentration of 6.712 moles/liter What is the osmotic pressure of the solution? (give your answer to 5 significant figures in mmHg) Tos mmHg
Complete the freezing point depression table below: Mass / Volume added Added reagent Molecular Weight van't Hoff Factor molality Freezing Point 20.0 g NaCl 25.0 g Li2SO4 10.0 mL 0.150 M ethanol Kf (°C/m) of water: 1.86 Freezing Point of Water, °C: 0.0 SOLVENT: 100 g water
(a) Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide. CaCl₂(s) Cal₂(s) Lattice Energy -2247 kJ/mol -2059 kJ/mol * Explain. ΔΗ soln -46 kJ/mol -104 kJ/mol *Lattice energy is defined as the energy change for the process M*(g) + X¯(g) → MX(s). calcium chloride 2201 calcium iodide 1955 XkJ/mol X kJ/mol (b) Based on your answers to part (a), which ion, CI or I, is more strongly attracted to water? chloride iodide The enthalpy of hydration for CaCl₂ is more exothermic than for Cal2. Any differences must be due to differences in hydrations between CI and I¯.
Given the following mixture of two compounds 45.00 mL of X (MW =80.00 g/mol)(density 0.893 g/mL) and 885.00 mL of Y (55.00 g/mol))(density 1.280 g/mL). The freezing point of pure Y is 54.00 degrees C. The molal freezing constant is 4.757 degrees C/m. What is the freezing point of the solution.
What is the freezing point, in °C, of a solution made with 1.07 mol of CHCl₃ in 530.0 g of CCl₄ (Kf = 29.8 °C/m, normal freezing point, Tf = -22.9 °C)?
1.613 g sample of an unknown nonionizing molecular compound is added to 250.0 g of benzene(C6H6, MW = 78.11 g/mol). The normal freezing point of the solution is 0.17 C lower than the normalfreezing point of pure benzene. Based on this information, find the molecular weight of the unknowncompound. benzene = Kf = 5.12 kg x Degrees C/mol.
Given the following mixture of two compounds 45.00 mL of X (MW =53.00 g/mol)(density 1.186 g/mL) and 830.00 mL of Y (71.00 g/mol)(density 1.041 g/mL). The freezing point of pure Y is 71.00 degrees C. The molal freezing constant is 4.609 degrees C/m. What is the freezing point of the solution.
What is the freezing point, in °C, of a solution made with 1.19 mol of CHCl₃ in 530.0 g of CCl₄ (Kf = 29.8 °C/m, normal freezing point, Tf = -22.9 °C)?
The boiling temperature of a substance increases by 0.63ºC when 565 g of a substance is dissolved in 298K in an organic solvent with a Maʼ 78 density of 0.88 g/cm3, consisting of 5.25 g of C and H. Considering that this solvent is Kf = 5.12 K kg/mol and Kb = 2.53 K kg/mol, and its pure vapor pressure is 103 tor at 298K, find the freezing point drop, vapor pressure and osmotic pressure of the solvent in the solution.
Automotive antifreeze consists of ethylene glycol, C₂H6O2, a non volatile nonelectrolyte. Calculate the boiling point and freezing point of a 25% mass percent solution of ethylene glycol in water. MW of Ethylene Glycol: 62.07 g/mol Kb Water: 0.52 °C/m K Water: 1.86 °C/m. 50. What is the molarity of the solution? Answer: 51. What is the change in freezing point temperature (in °C) of ethylene glycol solution? Answer: 52. What is the change in boiling point temperature (in °C) of ethylene glycol solution? Answer: 53. What is the boiling point temperature of the ethylene glycol solution? Answer: 54. What is the freezing point temperature of the ethylene glycol solution? Answer:
EJ0.939 M What is the vapor pressure of a 45.0 % solution of glucose, CH,,06, at a particular temperature, 12 6' given that the vapor pressure of pure water at that temperature is 486 mm Hg? 186 m m Ha