QUESTION If the mass of BaCl, 2H2Os sample subject to thermal decomposition was 2.526 g, what is the theoretical yield of BaCl, H2Os) if Reaction 1 occurred. (The molar mass of BaCl, 2H2O(s) is 244.2 g; the molar mass of BaCl;'H2Os) is 226.2 g)
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- 3. Maximum solubility of an ionic compounds in water depend on different sets of conditions. Out of five sets of conditions (given below), which one is the best for getting maximum solubility? A. The magnitude of the lattice energy should be large, and the enthalpy of hydration of the ions should be large. B. The enthalpy of hydration (Delta H) of the cation should be equal to the enthalpy of hydration of the anion, regardless of the magnitude of the lattice energy C. The magnitude of the lattice energy should be small, and the enthalpy of hydration of the ions should be small. D. The magnitude of the lattice energy should be small, and the enthalpy of hydration of the ions should be large. E. The magnitude of the lattice energy should be large, and the enthalpy of hydration of the ions should be small.The volume of the mixture prepared by taking 1.158 moles and 0.842 moles of water and ethanol, respectively, at 25 ° C was measured as 68.16 cm ^ 3. Interpret the result by finding the volume change during the preparation of the mixture since the densities at 25 ° C for pure water and atanol are given as 0.9970 g / cm ^ 3 and 0.7852 g / cm ^ 3, respectively.If one mixes 50 cm3 of EtOH and 50 cm3 of H2O at room temperature; will the total volume of the solution will be 100.0 cm3? Justify your answer with appropriate calculations and explanations.
- The salt cesium sulfate is soluble in water. When 22.7 g of Cs2SO4 is dissolved in 120.00 g of water, the temperature of the solution decreases from 25.00 to 22.96 °C. Based on this observation, calculate the enthalpy of dissolution of Cs2SO4 (in kJ/mol). Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible.Compound XY is an ionic compound that dissociates as it dissolves in water. The lattice energy of XY is -591.7 kJ mol-1.The hydration energy of its ions is -627.8 kJ mol 1. Write the thermochemical equations for the two steps in the formation of a solution of XY in water. Draw an enthalpy diagram for the formation of this solution. What is the net AH for the formation of a solution of XY? i kJ mol 1A bubble of air escaping from a diver's mask rises from a depth of 155 ft to the surface where the pressure is 1.00 atm. Initially, the bubble has a volume of 10.0 mL. Assuming none of the air dissolves in the water, how many times larger is the bubble just as it reaches the surface? Use this data: 1. The density of seawater is approximately 1.025 g mL! 2. The density of mercury is 13.6 g mL 47 times larger Use your answer to explain why scuba divers constantly exhale as they slowly rise from a deep dive. Since the pressure decreases by a factor of approximately factor of approximately 47 the volume must Increase : by a Divers exhale to decreases the amount of gas in their lungs, so it does not expand : to a volume larger than the diver's lungs.
- 14. Consider two ionic solids, both composed of singly-charged ions, that have different lattice energies. Which solid will be more soluble in water, the one with the larger lattice energy or the one with the smaller lattice energy? Assume that solute- solvent interactions are the same for both solids. (A) The solid with the larger lattice energy, if entropy increases as a result of mixing, and the solid with the smaller lattice energy, if entropy decreases as a result of mixing. (B) The solid with the smaller lattice energy, if entropy increases as a result of mixing, and the solid with the larger lattice energy, if entropy decreases as a result of mixing. (C) The solid with the smaller lattice energy. (D) The solid with the larger lattice energy. (E) They will have the same or very similar solubilities.2 NaCl (I) 2 Na (I) + Cl2 (g) O2 (g). + H2 (g) Explain the reaction and its applications with neat diagram 2 H205. Chemical Xis a solid with white color that forms large crystals. The solubility of chemical X in water at different temperatures is shown below. Solubility of X in H20 124 10- 8- 6- 2- 0+ Ó 10 20 30 40 50 60 70 80 90100 Temperature (°C) Irina wants to dissolve 30 grams of Xin 1 liter of water. She does so by stirring 30 grams of the large crystals into 1 liter of water at 45°C. How could Irina change her method to dissolve all the X faster? Solubility (g/100 g H,O) 4-
- POST-LABORATORY QUESTIONS Due after Laboratory Experiment 1. What is the equation for the dehydration of CuSO4 · 5H20? 2. A student dehydrated a sample of hydrate incompletely. Explain how the incomplete dehydration of the hydrate affects the calculation of the percent of water of hydration. What should the student do? 3. To the cooled anhydrate, CUSO4, of Part I, a student added about 5 mL of distilled water and then stirred the mixture with a stirring rod. When the student carefully touched the outside of the evaporating dish, do you expect the student to feel hot of cold? Is the rehydration an exothermic or endothermic process? 4. A student had a sample of CaCl2 • nH2O. He heated the sample until the mass did not change. From this data, calculate (a). the percentage of CaCl2 in the original sample and (b). the formula of the hydrate NOT ROUND Mass of crucible + cover = 28.39 g T Mass of crucible + cover + sample = 30.41g Mass of crucible + cover + residue = 29.75 5. The chemical…10.0 g ZnCl2 is dissolved in 100.0 g of water at 23.6 °C. The solution reaches a temperature of 36.5 °C. What is the molar heat of dissolution for ZnCl2? Assume the specific heat capacity of the solution is the same as pure water, 4.184 J/g·°C.In an ionic compound, the size of the ions affects the internuclear distance (the distance between the centers of adjacent ions), which affects lattice energy (a measure of the force needed to pull ions apart); the lattice energy, in turn, affects the enthalpy of solution. Based on ion sizes, arrange these compounds by their expected heats of solution. RbCl RbBr Rbl RbF Most exothermic AH soln Most endothermic AH soln Answer Bank