Final Review 8 Solutions System That Consists of Sugar Crystals

FINAL REVIEW #8 - Solutions As the temperature of a liquid increases, its vapor pressure (1) decreases (2) increases (3) remains the same Hexane (C₆H₁₄) and water do not form a solution. Which statement explains this phenomenon? (1) Hexane is polar and water is nonpolar. (2) Hexane is ionic and water is polar. (3) Hexane is nonpolar and water is polar. (4) Hexane is nonpolar and water is ionic. A mixture of crystals of salt and sugar is added to water and stirred until all solids have dissolved. Which statement best describes the resulting mixture? (1) The mixture is homogeneous and can be separated by filtration. (2) The mixture is homogeneous and cannot be separated by filtration. (3) The mixture is heterogeneous and can be separated by filtration. (4) The mixture is heterogeneous and cannot be separated by filtration. The solubility of KClO₃(s) in water (1) increases as the temperature of the solution increases (2) temperature of the solution decreases (3) pressure on the solution increases (4) pressure on the solution decreases A sample is prepared by completely dissolving 10.0 grams of NaCl in 1.0 liter of H₂O. Which classification best describes this sample? (1) homogeneous compound (2) homogeneous mixture (3) heterogeneous compound (4) heterogeneous mixture An unsaturated aqueous solution of NH₃ is at 90°C in 100 grams of water. According to the reference table, how many grams of NH₃ could this unsaturated solution contain? (1) 5 g (2) 10 g (3) 15 g (4) 20 g An unsaturated solution is formed when 80.0 grams of a salt is dissolved in 100 grams of water at 40°C. This salt could be (1) KCl 34 g (2) KNO₃ 63 g (3) NaCl 37 g (4) NaNO₃ 105 g A solution contains 35 grams of KNO₃ dissolved in 100 grams of water at 40°C. How much more KNO₃ would have to be added to make it a saturated solution? (1) 29 g (2) 24 g (3) 12 g (4) 4 g One hundred grams of water is saturated with NH₄Cl at 50°C. According to Table G, if the temperature is lowered to 10°C, what is the total amount of NH₄Cl that will precipitate? (1) 5 g (2) 17 g (3) 30 g (4) 50 g Which of the following could be a supersaturated solution at 40°C? (1) 50 g of KNO₃ (2) 38 g of NaCl (3) 30 g of KClO₃ (4) 110 g of NaNO₃ How many moles of solute are contained in 200 milliliters of a 1M solution? (1) 1 (2) 0.2 (3) 0.8 (4) 200 What is the total number of grams of NaI(s) needed to make 1.0 liter of a 0.010 M solution? (1) 0.015 (2) 0.15 (3) 1.5 (4) 15 13. If 0.025 grams of Pb(NO₃)₂ is dissolved in 100. grams of H₂O, what is the concentration of the resulting solution, in parts per million? * (1) 2.5 x 10⁻⁴ ppm * (2) 2.5 ppm * (3) 250 ppm * (4) 4.0 x 10³ ppm 14. How many moles of KNO₃ must be dissolved in water to make 1.5 liters of a 2.0 M solution? * (1) 0.5 mol * (2) 2.0 mol * (3) 3.0 mol * (4) 1.3 mol 15. What is the molarity of a solution of NaOH if 2 liters of the solution contains 4 moles of NaOH? * (1) 0.5 M * (2) 2.0 M * (3) 8 M * (4) 80 M 16. A student wants to prepare a 1.0 liter solution of a specific molarity. The student determines that the mass of the solute needs to be 30. grams. What is the proper procedure to follow? * (1) Add 30. grams of solute to 1.0 L of solvent. * (2) Add 30. grams of solute to 970 mL of solvent to make 1.0 L of solution. * (3) Add 1000. g of solvent to 30. g of solute. * (4) Add enough solvent to 30. g of solute to make 1.0 L of solution.   17. The freezing point depression of water depends on * (1) the number of solute particles * (2) the molecular mass of the solute particles * (3) the size of the solute particles * (4) the phase of the solute before addition to the water   18. Which of the following would have the greatest effect on the freezing point depression of 1 liter of water? * (1) 1 mole of NaCl * (2) 1 mole of CaCl₂ * (3) 1 mole of C₆H₁₂O₆ * (4) 1 mole of CH₃OH   19. At standard pressure, when NaCl is added to water, the solution will have a * (1) higher freezing point and a lower boiling point * (2) higher freezing point and a higher boiling point * (3) lower freezing point and a lower boiling point * (4) lower freezing point and a higher boiling point   20. What occurs when NaCl(s) is added to water? * (1) The boiling point increases and the freezing point increases. * (2) The boiling point increases and the freezing point decreases. * (3) The boiling point decreases and the freezing point increases. * (4) The boiling point decreases and the freezing point decreases. 21. Which solution has the lowest freezing point? * (1) 10. g of KI dissolved in 100. g of water * (2) 20. g of KI dissolved in 200. g of water * (3) 30. g of KI dissolved in 100. g of water * (4) 40. g of KI dissolved in 200. g of water   22. The vapor pressure of a liquid is 0.92 atm at 60°C. The normal boiling point of the liquid could be * (1) 35°C * (2) 45°C * (3) 55°C * (4) 65°C 23. The boiling point of a liquid is the temperature at which the vapor pressure of the liquid is equal to the pressure on the surface of the liquid. What is the boiling point of propanone if the pressure on its surface is 48 kPa?   Table H (A table showing vapor pressure of propanone at different temperatures is likely present in the image) 24. Which substance has the lowest vapor pressure at 75°C? * (1) water * (2) ethanoic acid * (3) propanone * (4) ethanol FINAL REVIEW #9 - KINETICS & EQUILIBRIUM Name: KEY The kinetic molecular theory assumes that the particles of an ideal gas are in random, constant straight-line motion. Which expression represents the ΔH for a chemical reaction in terms of the potential energy, PE, of its products and reactants? (1) PE of products + PE of reactants   (2) PE of products - PE of reactants (3) PE of products X PE of reactants   (4) PE of products / PE of reactants Increasing the temperature increases the rate of a reaction by increasing the frequency of effective collisions between reacting particles.   A real gas molecule behaves more like an ideal gas when the gas molecules are far apart and have weak attractive forces between them.   In a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is defined as the heat of reaction (ΔH).   Use the following potential energy diagram for questions 6 and 7 potential energy diagram with reactants, products, and an activation energy barrier Which interval on this diagram represents the difference between the potential energy of the products and the potential energy of the reactants? ΔH   (1) 1 (2) 2 (3) 3 (4) 4 Which arrow represents the activation energy of the forward reaction? (1) 1 (2) 2 (3) 3 (4) 4 (from reactants to top of bump) How is a chemical reaction affected by the addition of a catalyst? (1) The activation energy decreases. (2) The heat of reaction increases. (3) The number of collisions between particles decreases. (4) The potential energy of the reactants increases.   Which statement must be true for any chemical reaction at equilibrium? (1) The concentration of the products is greater than the concentration of the reactants.   (2) The concentration of the products is less than the concentration of the reactants. (3) The concentration of the products and the concentration of the reactants are equal. (4) The concentration of the products and the concentration of the reactants are constant.