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As the number of solute particles in a given volume of solution increase will: freezing point increase, vapor press decrease? or vice versa or boiling point increase, vapor pressure decrease? or vice versa?

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  1. Chemistry

    What Occurs as a salt dissolves in water? the number of ions in the solution increases and the freezing point decrease the number of the ions in the solution increase and the freezing point increase the # of ions in the solution decrease and the freezing
  2. CHM

    As the number of solute particles in a given volume of solution increase will: freezing point increase, vapor press decrease? or vice versa or boiling point increase, vapor pressure decrease? or vice versa?
  3. Chem(again)

    What is the relationship between the amount of solute and the amount of freezing point depression? delta T = kf m where delta T is the difference between the normal freezing point and the f.p. with a solute, kf is the freezing point constant, and m is the
  4. chemistry

    If a solution has a lot of particles, is it going to have a low or high boiling point? For instance, would NaCl have a higher or lower boiling point than C12H22O11, based on the amount of particles it has (NaCl has more than C12H22O11)? Are you thinking of
  5. AP Chem.

    NaCl dissociates completely in water. Therefor the total number of particles in a 1.0 m NaCl solution is no longer 6.02 X 10^23. Since a colligative property is dependent only on the total number of solute particles, what is the freezing point for 1.0 m
  6. CHemistry....Please help

    What mass of ethylene glycol C2H6O2, the main component of antifreeze, must be added to 10.0 L water to produce a solution for use in a car's radiator that freezes at -23C? Assume density for water is exactly 1g/mL. ----------------------------------- This
  7. chemistry(check my answer)

    sorry i forgot add the question The freezing point of a solution is A. lower than the freezing point of the solvent alone because higher temperature is required to accelerate solvent molecular motion enough to overcome obstructon by solute particles.. B.
  8. chemistry(check my work)

    The freezing point of a solution is A. lower than the freezing point of the solvent alone because higher temperature is required to accelerate solvent molecular motion enough to overcome obstructon by solute particles.. B. higher than the freezing point of
  9. chemistry

    The freezing point of a solution is A. higher than the freezing point of the solvent alone because higher temperature is required to accelerate solvent molecular motion enough to overcome obstruction by solute particles. B. lower than the freezing point of
  10. chem(freezing point)

    please help! I am lost! Question: Find the expected freezing point of a water solution that contains 286g of aluminum nitrate (Al(NO3)3) in 8.5 kg of water. answer in celcius Note the correct spelling of Celsius. delta T = i*Kf*m Determine the molality of
  11. Inorganic Chemistry

    Which aqeuous solution has a freezing point closest to that of 0.30M C12H22O11? A) 0.075M AlCl3 B) 0.15M CuCl2 C) 0.30M NaCl D) 0.60M C6H12O6 I know the answer but I don't know the reason or rationale behind it. Please explain. I suggest you review
  12. Chemistry

    The freezing point of a solution is A. lower than the freezing point of the solvent alone because higher temperature is required to accelerate solvent molecular motion enough to overcome obstructon by solute particles.. B. lower than the freezing point of
  13. chemistry

    The freezing point of a solution is A. lower than the freezing point of the solvent alone because higher temperature is required to accelerate solvent molecular motion enough to overcome obstructon by solute particles.. B. lower than the freezing point of
  14. chemistry

    A freezing point depression experiment was conducted using cyclohexane as the solvent. The freezing point of pure cyclohexane is 6.60°C and the freezing point depression constant is 20.00°C/m. The freezing point of a solution containing 0.135 g of an
  15. chemistry

    A compound was found to be composed of the following amounts of elements: 20.00% wt% C, 26.64wt% O, 46.65 wt%N, and 6.71wt%H. A 6.125 grams sample of this compound dissolved in 46.205 grams of water as a solution was found to have a freezing point of
  16. chemistry

    Compute the freezing point of this Solution: 25.5g C7H11NO7S (4-nitro-2-toluenesulfonoic acid dihydrate) in 1.00*10^2g H2O (nonionizing solute) The freezing point of H2O is lowered 1.86 Celsius per mole of solute. The boiling point of H2O is raised 0.512
  17. I am so lost

    The freezing point of pure cyclohexane is 6.60°C and the freezing point depression constant is 20.00°C/m. The freezing point of a solution containing 0.161 g of an unknown nonelectrolyte solute and 5.818 g of cyclohexane was 3.98°C. What is the molar
  18. I am so lost

    The freezing point of pure cyclohexane is 6.60°C and the freezing point depression constant is 20.00°C/m. The freezing point of a solution containing 0.161 g of an unknown nonelectrolyte solute and 5.818 g of cyclohexane was 3.98°C. What is the molar
  19. chemistry

    The freezing point of a 0.010 m aqueous solution of a nonvolatile solute is ?0.072°C. What would you expect the normal boiling point of this same solution to be? have no clue, thanks for the thelp Freezing point depression= N*kf* molality you have
  20. chemistry

    1. Would it be advisable to determine the freezing point of pure p-dichlorobenzene with one thermometer and the freezing point of the solution with a different one? Explain. 2. If 0.150 mole of a nonvolatile non-electrolyte solute is present in 1200g of
  21. Chemistry

    1. Would it be advisable to determine the freezing point of pure p-dichlorobenzene with one thermometer and the freezing point of the solution with a different one? Explain. 2. If 0.150 mole of a nonvolatile non-electrolyte solute is present in 1200g of
  22. Chemistry

    Cyclohexane has a freezing point of 6.6 degree Celsius and a K(f) of 20.0 degree Celsius/m. 1.50g of an unknown solute is dissolved wth 18.0g of cyclohexane. The freezing point of the solution was 1.3 degree Celsius Using this iInformation assuming the
  23. chemistry

    In BHT Freezing Point Depression Lab: The following errors occurred when the above experiment was carried out. How would each affect the calculated molecular mass of the solute (too high, too low, no effect)? Explain your answers. The thermometer used
  24. Physical Chemistry

    When 1.33 g of a nonpolar solute was dissolved in 50.0 g of phenol, the latter's freezing point was lowered by 1.454°C. Calculate the molar mass of the solute. The kf of phenol is 7.27 (K·kg)/mol. What is the normal boiling point of an aqueous solution
  25. chemistry

    which of the following would be expected to have the lowest freezing temperature? a. .1 M Ca(NO3)2 b. .1 M NaC2H3O2 c. .1 M CuSO4 d. .1 M HC2H3O2 e. .1 M C2H5OH Here is what you do Mary. delta T = Kb*i*m Kb is the same for all. m is the same for all. i is
  26. Chemistry II

    An unknown solute (a nonelectrolyte) was obtained and 5.37 g was weighed out. After dissolving the solute in water, the mass of the solution was 26.58 g. From the experimental results, the freezing point depression was found to be 3.6oC. If the freezing
  27. chemistry

    I have the answers, I am just interested in the formulas so that I can solve the problems, thanks! 1. Find the boiling point of a solution composed of 110g of HgCl2 (a non-ionizing solute) in 175g of water. 2. Find the freezing point of a solution composed
  28. Chemistry

    How does dissolving a solute affect the boiling point or freezing point of the solution? What about the solution's vapor pressure? Read about Raoult's Law, freezing point depression and boiling point elevation.
  29. chemistry

    The following errors occurred when the experiment was carried out. How would each affect the calculated molar mass of the solute(too high, too low, no effect)? Explain. a. The thermometer used actually read 1.4 centigrade too high. b. some of the solvent
  30. Chemistry

    The freezing point of a cyclohexane sample is 6.20*C. A soltuion is prepared by dissolving 0.4660g of an unknown solute in 36.0g cyclohexane. The freezing point of the solution if 4.11*C. Calculate the molar mass of the unknown solute. Kf for cyclohexane
  31. chemistry(check my answer)

    A. lower than the freezing point of the solvent alone because higher temperature is required to accelerate solvent molecular motion enough to overcome obstructon by solute particles.. B. higher than the freezing point of the solvent alone because higher
  32. Chemistry - Van't Hoff Factor

    How does the van't hoff factor relate to freezing points? If one van't hoff factor is bigger than another, is its freezing point lower or greater? delta Tf = iKfm. So increasing i will increase delta Tf Van't Hoff factor is the concentration of particles
  33. chemistry

    If the freezing point of the solution had been incorrectly read 0.3degrees C lower than the true freezing point, would the calculated molar mass of the solute be too high or too low? Explain.
  34. Chemistry

    The boiling point of a solution increases directly as a function of the number of moles of solute present in a given mass of solution. This relationship is expressed mathematically by the following equation. ΔTb = Kb·m ΔTb is the boiling-point elevation
  35. Science

    A solution containing 3.22g of solute in 40.0g of 1,4-dichlorobenzene and its freezing point is 49.2 C. Calculate the molar mass of the solute.
  36. Chemistry

    68.0g of solute were dissolved in 393 mL of benzene. The solution froze at -0.50°C. The normal freezing point of benzene is 5.5°C and the molar freezing point constant is 5.12°C kg/mol. The density of benzene is .879 g/mol. Calculate the molar mass of
  37. chemistry

    Data: freezing point of pure cyclohexane: 6.0 degrees celcius Freezing point of unknown soluton: 1.6 degrees celcius weight of cyclohexane: 40.0231g=0.0400231 kg weight of unknown solute: 0.4872 g K_f_ of cyclohexane: -20.00 degrees Celciusx kg/mole
  38. Chemistry

    The solute molecules mixed with the solvent molecules in a solution cause the freezing point of a solution to be ______ than it is for an equal volume of pure _________.
  39. Chemistry

    Can someone check my answer and let me know me if the are right or wrong. 1. What is the maximum amount of KCl that can dissolve in 600 g of water? (The solubility of KCl is 34 g/100 g H₂O at 20°C.) * 34 g 204 g ***** 2040 g 3. (1 point) If the
  40. Chemistry (Regents level)

    1- In the reaction Fe2O3 + 3 CO = 2 Fe + 3 CO2, what is the total number of moles of CO used to produce 112 grams of iron? a) 1.0 b)2.0 c)3.0 d)4.0 2- Given the reaction: 4Al + 3O2 = 2Al2O3 How many moles of Al2O3 will be formed when 27 grams of Al reacts
  41. Chemistry

    3.92g of a nondissociating compound are dissolved in 400.g of liquid benzene. The freezing point of the solution is 5.19 degrees celsius. Calculate the molar mass of the compound. (The freezing point of the pure benzene is 5.50 degrees celsius and its
  42. Physical science

    Which statement correctly describes the relationship between the volume of a gas and its temperature, in Kelvin, assuming pressure is held constant?(1 point) The relationship is inversely proportional; as temperature increases, volume increases in the same
  43. Science

    A stock solution has a concentration of 12.4 M. What volume of stock solution would be needed to make 7.6 L of solution with a concentration of 4.4 M? Which substance is an example of a nonpolar compound? Which statement is the best explanation for the
  44. Chemistry

    A solution contains 15 g non-volatile non-electrolyte solute C6H14O6 dissolved in 500 g of water at 40 c. Calculate (A)Vapor pressure of the solution. (B)Boiling point of the solution. (C)Freezing point of the solution.
  45. Physical Science

    1. boyle's law states that the volume of a gas is inversely proportional to its pressure if the? A) temperature and number of particles are consistent** B) temperature reaches absolute zero C) number of particles are doubled D) temperature and number of
  46. Chemistry

    The vapor pressure of 1 M of KI solution is ________ 1 M of glucose solution. This is because vapor pressure depends only on the _________. Which option correctly completes this statement? the same as; concentration of the solute less than; number of
  47. Chemistry

    Calculate the molecular mass of the nonionic solutes. 8.02 grams of solute in 861 grams of water lower the freezing point to -0.430 celsius. the freezing point of H2O is lowered 1.86 celsius per mole of solute. the boiling point of H2O is raised 0.512
  48. Chemistry II

    If the freezing point depression (DTf) is 5.62 and the freezing point depression constant (Kf) is 3.90, what is the molality of the solution? Assume that the solute is a nonelectrolyte (i = 1).
  49. Chemistry

    Confused on these, please explain or show work for the answer if you can. :) 1. What is the morality of a water solution that freezes at -0.633°C? 2. What is the freezing point of a solution that contains 1.99 g of a molecular solute of molar mass 58.5
  50. Chemistry

    Which contains more solute particles a 0.10 M aqueous solution of methanol (CH3OH) or a 0.10 M aqueous solution of table salt (NaCl)? Are we supposed to go M*L=moles*(6.022*10^23 solute particles)
  51. Chemistry

    1) Benzene freezes at 5.45 degrees celsius. The Kf for benzene is -5.07C/m. What would be the freezing point of a 0.210m solution of octane in benzene? I am not sure how to start this. I know the equation for freezing point is Kfp * m solute.
  52. Chemistry

    Compute the boiling point of this solution: 1.00*10^2g C10H8O6S2 (1,5-naphthalenedisulfonic acid) in 1.00*10^2g H2O (nonionizing solute) The freezing point of H2O is Lowered 1.86 Celsius per mole of solute. The boiling point of H2O is Raised 0.512 Celsius
  53. Chemistry

    Experiment questions: Experiment 1 results mass of beaker:116.944 g mass of dodecanoic:11.629 g hot water: 175 C warm water: 10 C Average Fressing pt of Dodecanoic = 42.7 Experiment 2 results: Unknown C solution mass: 2.091g Hot water: 175C warm water: 10C
  54. Chemistry

    A solution is made by dissolving 0.698 mol of nonelectrolyte solute in 777 g of benzene. Calculate the freezing point and boiling point of the solution
  55. Chem

    A solution is made by dissolving 0.584 mol of nonelectrolyte solute in 883 g of benzene. Calculate the freezing point and boiling point of the solution. Tf=? Tb=? I got Tf as 3.39 degrees Celsius I got Tb as 1.67 degrees Celsius It marked me wrong and said
  56. chemistry

    Compute the boiling point of this Solution: 25.5g C7H11NO7S (4-nitro-2-toluenesulfonoic acid dihydrate) in 1.00*10^2g H2O (nonionizing solute) The freezing point of H2O is lowered 1.86 Celsius per mole of solute. The boiling pint os H2O is raised 0.512
  57. chemistry

    1. Find the molality of the solution prepared by dissolving 0.238g toluene, C7H8, in 15.8g cyclohexane 2. A pure sample of the solvent phenol has a freezing point of 40.85 degrees C. A 0.414 molal solution of isopropyl alcohol was observed to have a
  58. Chemistry

    A solution is made by dissolving 0.526 mol of nonelectrolyte solute in 831 g of benzene. Calculate the freezing point and boiling point of the solution. Constants may be found here.
  59. Chemistry

    Can someone check my answer and let me know me if the are right or wrong. If I wrong can you give me the right answer plz. 1. What is the maximum amount of KCl that can dissolve in 600 g of water? (The solubility of KCl is 34 g/100 g H₂O at 20°C.) * 34
  60. chemistry

    a. Find the amount of solute based on this information Volume = 500 ml Concentration of solution= 15% (w/w) Solute (molar mass) = H2SO4 is 98.0g/mol b. Find the molar mass Amount of solute= 117.0g Volume of solution= 2.00L concentration of a solution= 1.0M
  61. chemistry

    a. Find the amount of solute based on this information Volume = 500 ml Concentration of solution= 15% (w/w) Solute (molar mass) = H2SO4 is 98.0g/mol b. Find the molar mass Amount of solute= 117.0g Volume of solution= 2.00L concentration of a solution= 1.0M
  62. Chemistry

    Two moles of a nonelectrolyte solute are dissolved in 1 kg of an unknown solvent. The solution freezes at 7.8 degrees Celsius below its normal freezing point. What is the molal freezing point constant of the unknown solvent? What is your prediction for the
  63. science

    What is a solvent? a The material that is dissolved b The material that increases the speed of the dissolution c The material that reduces how much can be dissolved d The material that is dissolving another material Question 2 (1 point) Which of the
  64. chemistry

    N2O4(g) + energy ⇄ 2NO2(g) The system is at equilibrium, but then it is subjected to an increase in pressure. Which change will happen? The rate of the reverse reaction will increase, which will increase the number of particles in the system. The rate of
  65. ap chem

    Find the molecular mass of a solute by freezing point depression. Solvent: para-dichlorobenzene Freezing point of pure solvent: 53.02C Mass of unknown substance: 2.04g Freezingpointdepressin constant:7.1c/m Mass of para-dichlo...: 24.80g Freexing point
  66. Chemistry

    Calculate the boiling points of freezing points of the following solutions in water. a) boiling point of a 2.25m solution of propylene glycol (a non-electrolyte) b)freezing point of a 1.0m solution of potassium iodide c)freezing point of a 1.0m solution of
  67. Chemistry

    The normal freeing point of cyclohexane if 6.6 degrees Celsius. A 0.2g sample of an unknown solute is dissolved in 50 ml of cyclohexane (d-0.8g/ml, Kf=20 degreesCelsius/m. If the freezing point of the solution is 3.6 degrees Celsius, what is the molar mass
  68. chemistry

    Which step during the dissolving process releases energy? A. Separating solute particles from one another B. Adding solute into the solvent C. Separating solvent particles from one another D. Mixing the particles of solute with particles of solvent
  69. Physical Science Just One Question PLEASE HELP!

    In an exothermic reaction, the amount of energy required to break the attractions among the solute particles and among the solvent particles is A) greater than the energy released as attractions form between solute and solvent particles. B) less than the
  70. Chemistry

    Derive a formula for the molar mass of the solute in terms of the freezing point depression, deltaT, the freezing-point constant, Kf, and the masses of solvent, msolvent, and solute, msolute, used in an experiment like this one. SHow your work and include
  71. Chemistry

    A solution is made by dissolving 0.624 mol of nonelectrolyte solute in 795 g of benzene. Calculate the freezing point and boiling point of the solution. Tf=_ˆC Tb=_ˆC
  72. Chem

    a solution is prepared by dissolving 0.47 g of a solute in 12.7 g of cyclohexane what is the freezing point change
  73. chemistry

    Which answer choice correctly explains the role of the kinetic theory of matter in the process of solutes being dissolved into solvents? The continuous motion of the particles in the solvent and solute cause them to collide with one another, which results
  74. Chemistry

    What is the freezing point of a solution containing 4.134 grams naphthalene (molar mass = 128.2) dissolved in 30.0 grams paradichlorobenzene? The freezing point of pure paradichlorobenzene is 53.0°C and the freezing point depressing constant Kfp is
  75. Chemistry

    Pure benzene has a normal freezing point of 5.50 degrees Celsius. A solution containing 11.4 grams of a molecular substance dissolved in 150.0 grams of benzene (Kf=5.12C/m) has a freezing point of 1.20 degrees Celsius. What is the molar mass of the solute?
  76. Chem AP

    A 0.505-g sample of a compound is dissolved in enough water to form 100.0 mL of solution. This solution has an osmotic pressure of 2.56 atm at 25°C. If each molecule of the solute dissociates into two particles (in this solvent), what is the molar mass of
  77. Chemistry

    1) The molecular mass of a substance was determined by the freezing point depression technique. The minimum data required for the determination are a. ƒ´Tf and Kf only. b. ƒ´Tf , Kf and mass of solute. c. ƒ´Tf , Kf , mass of solute and mass of
  78. Science

    Please check my answers (at the bottom) with these questions. 1. An apple quickly changes color when exposed to air. This demonstrates a ________. (1 point) physical property chemical property physical change all of the above 2. When a chunk of dry ice is
  79. chemistry

    a solution is prepared by mixing 2.17g of an unknown non-electrolyte with 225.0g of chloroform. The freezing point of the resulting solution is -64.2 C . The freezing point of pure chloroform is -63.5 C and its kf= 4.68C m^-1 . What is the molecular mass
  80. chemistry

    you are conducting a freezing-point determination in the laboratory by using an aqueous solution of KNO3. The observed freezing point of the solution is -1.15 C. Using a pure water sample, you recorded the freezing point of the pure solvent of the same
  81. Chemistry

    What is the molar mass of a molecular solute when 5g of the solute dissolved in 150g of phenol lowers the freezing point 1.5C? do i have to use all three formulas to solve this one?
  82. Chemistry

    The equation for lowering the freezing point of a solvent is given in your manual. Given that the freezing point for the pure solvent is 79.4 °C , the molality is 0.1 m , and the freezing point depression constant is 6.9 °C/m , determine the freezing
  83. Chemistry

    A water solution containing an unknown quantity of an unknown nonelectrolyte solute has a freezing point of -0.21 Celsius. What is the molality of the solution? Kf=-1.86C/m
  84. Chemistry

    WHAT IS THE FREEZING POINT OF THIS SOLUTION? 25.5g C7,H11,N,O7,S(4-nitro-2-toluenesulfonic acid dihydrate) in 1.00x10^2g H2O(nonionizing solute)
  85. Chemistry

    two solutions are prepared using the same solute solution a: 0.27g of the solute disolves in 27.4g of t-butanol solution b: 0.23g of the solute disolves in 24.8g of cyclohexane which solution has the greatest freesing point change? show calculations and
  86. Chemistry

    two solutions are prepared using the same solute solution a: 0.27g of the solute disolves in 27.4g of t-butanol solution b: 0.23g of the solute disolves in 24.8g of cyclohexane which solution has the greatest freesing point change? show calculations and
  87. 5 g vial

    A 5 g igal reguires addinng 8.6 ml diluent to get concentration of 250 mg/ml. The powder volume is __ ml a.9.3 b.10.6 c.11.4 d.12.8 Does the powder form a solution or a colloid? IT makes a big difference. In solutions, the sum of the powder volume and the
  88. chemistry

    if the freezing point of the solution had been incorrectly determined to be lower than the true freezing point, how would that affect the calculated molar mass? Explain. The molecular weight would be higher if the true freezing point is bigger than the
  89. chemistry

    Compute the freezing point of this solution: 25.5 g C7H11NO7S (4-nitro-2-toluenesulfoinoic acid dihydrate) in 100 g H2O. (nonionizing solute)
  90. Chemistry

    An aqueous salt solution is formed by adding 11.67 g sodium sulfate (solute) to water (solvent). What mass (in g) of water is used if the freezing point of the solution is -12.9 Farenheit. Kf H2O = 1.86 Celsius/m
  91. Chemistry

    Given one of the following solution: 50.00mL of 0.10M of K2CrO4 answer the following. 1. How do you prepare the solution? 2. What volume (mL) of your solution contains 5.00X10(-4) moles of the solute? 3. What volume of your solution contains 1.00g of the
  92. chemistry

    Which of the following can be determined if the boiling-point elevation, the mass of solute and the molality of a given solution are known. The identity of the solute The polarity of the solute The size of a molecule of the solute The molecular weight of
  93. chemistry

    Which of the following is NOT true for solutes and solvents? A. At least one solvent must be dissolved in a solute to make a solution. B. Solute concentration can be measured in terms of solute moles / solution volume or solute moles / solvent mass. C. A
  94. Chemestry

    Calculate the freezing point of a solution containing 12.2grams of benzoic acid, C6H5CO2H, dissolved in 250 grams of nitrobenzene, C6H5NO2. The freezing point of nitrobenzene is 7.7 C, and its freezing point depression constant is 7.0 C/m.
  95. Chemistry

    Benzene (C6H6) has a normal freezing point of 5.50oC and a density of 0.88 g/mL. When 1.28 g of naphthalene (C10H8) is dissolved in 125 mL of benzene, the freezing point of the solution is 5.03oC. Determine the molal freezing point constant for this
  96. chemistry

    Calculate the freezing point of 0.15 m calcium chloride aqueous solution. Assume that the molal freezing point depression constant of water is 1.86°C·kg/mol and that the freezing point of water is 0.00°C
  97. chemistry

    Camphor, C16H16O which has a freezing point of 174°C, has a freezing point depression constant of 40.0°C/m. Explain the usefulness and the limitation of camphor as a solvent for determination of molecular weights. For whose kind(s) of solute would
  98. Chemistry - Colligative Properties

    The freezing-point depression for a given aqueous solution is 0.32 K. The freezing-point depression constant for water is 1.86 K/m. Calculate the molality of solutes in the solution. The equation for freezing point depression is ΔTf = Kf · m, where ΔTf
  99. Chemistry

    I am stuck in this problem I need to calculate the molality first so I could find T but I don't know which one is the solvent and which one is the solution the problem is to calculate the freezing point of a solution containing 12.2g of benzoic acid,
  100. Chemistry

    A 1.00% by mass MgSO4(aq) solution has a freezing point of -0.192°C. Water has a kf of 1.86 (K·kg)/mol. (a) Estimate the van't Hoff i factor from the data. (b) Determine the total molality of all solute species. I can probably figure out the second part

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