Homework Help is Here – Start Your Trial Now!
Science
Chemistry
a. Eutexia b. The Phase Rule c. Polymorphism d. Degrees of Freedom Useful device for relating the effect of the least number of independent variables upon the various phases that can exist in equilibrium system containing a given number of components Type of solution has a solute concentration equivalent to its limit of solubility a. Saturated solution b. Unsaturated solution c. Supersaturated solution d. Unknown solution a. Dipole-dipole forces b. Dipole-induced dipole forces c. lon-dipole interaction d. lon-induced dipole interaction Same solute is added to this solution, even in minute amounts, will lead to crystallization, precipitation, or insolubility of that solute Intermolecular bond that is involved in the attraction of electrons of nonpolar molecules resulting to transient polarity

a. Eutexia b. The Phase Rule c. Polymorphism d. Degrees of Freedom Useful device for relating the effect of the least number of independent variables upon the various phases that can exist in equilibrium system containing a given number of components Type of solution has a solute concentration equivalent to its limit of solubility a. Saturated solution b. Unsaturated solution c. Supersaturated solution d. Unknown solution a. Dipole-dipole forces b. Dipole-induced dipole forces c. lon-dipole interaction d. lon-induced dipole interaction Same solute is added to this solution, even in minute amounts, will lead to crystallization, precipitation, or insolubility of that solute Intermolecular bond that is involved in the attraction of electrons of nonpolar molecules resulting to transient polarity

Principles of Instrumental Analysis
Principles of Instrumental Analysis
7th Edition
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Chapter29: Supercritical Fluid Chromatography And Extraction
Section: Chapter Questions
Problem 29.11QAP
See similar textbooks
icon
Related questions
icon
Concept explainers
Question

Encircle the answers here

a. Eutexia b. The Phase Rule c. Polymorphism d. Degrees of Freedom Useful device for relating the effect of the least number of independent variables upon the various phases that can exist in equilibrium system containing a given number of components a. Tetragonal b. Cubic с. Нехаgonal d. Monoclinic Crystalline form of Nacl a. Monoclinic b. Нехagonal c. Rhombic d. Triclinic a. Monoclinic b. Triclinic c. Tetragonal d. Rhombic a. Electrolytes Crystalline form of iodine a. Saturated solution Type of solution has a solute concentration equivalent to its limit of solubility Same solute is added to this solution, even in minute amounts, will lead to crystallization, precipitation, or insolubility of that solute Intermolecular bond that is involved in the attraction b. Unsaturated solution c. Supersaturated solution d. Unknown solution Crystalline form of sucrose a. Dipole-dipole forces b. Dipole-induced dipole forces c. lon-dipole interaction d. lon-induced dipole interaction Electrovalent b. lonic c. Dipole-dipole d. covalent a. Electrostatic force of electrons of nonpolar molecules resulting to transient polarity Substance that does not yield ions when dissolved in water and not conduct electric current through the b. Solutes Non electrolytes d. Solvents с. solutions a. Type of chemical bond where atoms share electrons Type of intermolecular force that is the result of temporary uneven distribution of electrons around molecules that result in momentary dipoles Dipole-dipole b. Molecule-ion Hydrogen bond d. London dispersion forces Gay-Lussac's Law b. Charles' law c. Dalton's law d. Boyle's Law a. Gram atom b. Mole cc. Mass number d. Molecule а. Force of attraction between molecules of different b. Adhesive force phases Law that gives the relation of volume and temperature at constant pressure а. C. Cohesive force d. None of the above a. Normality b. Molarity c. Molality d. osmolarity Electrostatic force Number of gram equivalents of solute per liter of solution Amount of substance whose mass in grams is numerically equal to the molecular weight of the substance a. Force of attraction between molecules of same b. Adhesive force phases a. Soluble liquids b. Immiscible liquids c. Partially miscible liquids d. Volatile liquids Cohesive force Two liquids which are completely insoluble with each С. d. None the above other lonic Dipole-dipole interaction a. Covalent c. Keesom forces d. Debye forces a. Cubic b. Нехagonal c. Triclinic d. Monoclinic b. a. Size of the particles in solution b. pH of the solution c. type of particle in solution d. number of particles in solution Colligative properties depend upon the Crystalline form of boric acid a. Triclinic Crystalline form of urea a. Urea b. lodoform b. Monoclinic Example of tetragonal crystal c. Tetragonal d. hexagonal lodine d. Sodium chloride a. Vapor pressure b. Boiling point c. Freezing point c. a. Rhombic Crystalline form of iodoform b. Cubic Raoult's law is encountered in the determination of c. Tetragonal d. hexagonal
Transcribed Image Text:a. Eutexia b. The Phase Rule c. Polymorphism d. Degrees of Freedom Useful device for relating the effect of the least number of independent variables upon the various phases that can exist in equilibrium system containing a given number of components a. Tetragonal b. Cubic с. Нехаgonal d. Monoclinic Crystalline form of Nacl a. Monoclinic b. Нехagonal c. Rhombic d. Triclinic a. Monoclinic b. Triclinic c. Tetragonal d. Rhombic a. Electrolytes Crystalline form of iodine a. Saturated solution Type of solution has a solute concentration equivalent to its limit of solubility Same solute is added to this solution, even in minute amounts, will lead to crystallization, precipitation, or insolubility of that solute Intermolecular bond that is involved in the attraction b. Unsaturated solution c. Supersaturated solution d. Unknown solution Crystalline form of sucrose a. Dipole-dipole forces b. Dipole-induced dipole forces c. lon-dipole interaction d. lon-induced dipole interaction Electrovalent b. lonic c. Dipole-dipole d. covalent a. Electrostatic force of electrons of nonpolar molecules resulting to transient polarity Substance that does not yield ions when dissolved in water and not conduct electric current through the b. Solutes Non electrolytes d. Solvents с. solutions a. Type of chemical bond where atoms share electrons Type of intermolecular force that is the result of temporary uneven distribution of electrons around molecules that result in momentary dipoles Dipole-dipole b. Molecule-ion Hydrogen bond d. London dispersion forces Gay-Lussac's Law b. Charles' law c. Dalton's law d. Boyle's Law a. Gram atom b. Mole cc. Mass number d. Molecule а. Force of attraction between molecules of different b. Adhesive force phases Law that gives the relation of volume and temperature at constant pressure а. C. Cohesive force d. None of the above a. Normality b. Molarity c. Molality d. osmolarity Electrostatic force Number of gram equivalents of solute per liter of solution Amount of substance whose mass in grams is numerically equal to the molecular weight of the substance a. Force of attraction between molecules of same b. Adhesive force phases a. Soluble liquids b. Immiscible liquids c. Partially miscible liquids d. Volatile liquids Cohesive force Two liquids which are completely insoluble with each С. d. None the above other lonic Dipole-dipole interaction a. Covalent c. Keesom forces d. Debye forces a. Cubic b. Нехagonal c. Triclinic d. Monoclinic b. a. Size of the particles in solution b. pH of the solution c. type of particle in solution d. number of particles in solution Colligative properties depend upon the Crystalline form of boric acid a. Triclinic Crystalline form of urea a. Urea b. lodoform b. Monoclinic Example of tetragonal crystal c. Tetragonal d. hexagonal lodine d. Sodium chloride a. Vapor pressure b. Boiling point c. Freezing point c. a. Rhombic Crystalline form of iodoform b. Cubic Raoult's law is encountered in the determination of c. Tetragonal d. hexagonal
d. Melting point a. Freezing point b. Melting point c. Osmotic pressure d. Boiling point a. London dispersion forces b. Dipole-dipole forces c. lon-dipole forces d. Hydrogen bonds a. Vapor pressure b. Osmotic pressure Critical pressure d. Critical temperature c. Heat potential d. Convertibility Temperature at which the vapor pressure is equal to atmospheric pressure Increases when a solute is The vapor pressure of a liquid a. added to the liquid Is independent of temperature c. Equals atmospheric b. Most important intermolecular forces found between water molecules pressure at liquid's boiling point d. Decreases with an increase The pressure required to liquefy a gas at its critical temperature in temperature a. Melting point b. Boiling point c. Freezing point d. Eutectic point a. Constitutive b. Additive property of solution c. Accumulative d. Colligative a. Raoult's law b. Clausius 'Clapeyron Equation c. Van Slyke equation d. Van't hoff's equation lon-induced dipole A point at which the liquid and solid phase have the same composition C. Solutions of lower osmotic pressure than that of the а. Нурertonic b. Нурotonic c. Isotonic d. None of the above a. London dispersion forces b. lon-dipole forces c. Dipole-dipole forces d. Hydrogen bonding body fluid Osmotic pressure is Type of intermolecular force is present in all substances, regardless of polarity Equation that gives the relationship between the vapor pressure and the absolute temperature of a liquid a. Polymerism b. Isomerism Existence of elemental substances such as carbon and sulfur, in more than one crystalline form c. Polymorphism d. Solvates Attractive interaction between a polar molecule and the induces dipole a. interaction a. Dipole-dipole forces between water molecules b. London dispersion forces between water molecules c. Hydrogen bonds between water molecules d. Molecule-ion attraction Explains the very high melting and boiling point of b. Dipole-induced dipole water interaction c. Induced dipole d. lon-Dipole Forces a. Percent by weight b. Molarity c. Molality d. Gram weight a. Covalent b. Electrovalent c. Dipole d. lonic Number of grams of solute in 100 gram of solution between water molecules a. Boyle's law b. Ideal gas law c. Charles' law d. Gay-Lussac's law a. Hydrogen bond b. London dispersion forces c. Dipole-dipole forces d. Molecule-ion attractions Law that governs the relationship between pressure, volume and temperature of gases which is expressed in the following questions, PV=nRT A polar molecule, one region of which is positive and the other negative Strongest intermolecular forces Solution in which the solute is in equilibrium with the solid phase а. Unsaturated b. Subsaturated c. Supersaturated d. Saturated It is the pressure that must be applied to the solution to prevent the flow of pure solvent into the a. Critical pressure b. Vapor pressure c. Atmospheric pressure d. Osmotic pressure a. Normality b. Molarity Molality d. Equivalent weight The number of moles of solute per 1000g of solvent concentrated solution C. a. Enthalpy b. Entropy That portion of energy of a system which cannot be converted to work
Transcribed Image Text:d. Melting point a. Freezing point b. Melting point c. Osmotic pressure d. Boiling point a. London dispersion forces b. Dipole-dipole forces c. lon-dipole forces d. Hydrogen bonds a. Vapor pressure b. Osmotic pressure Critical pressure d. Critical temperature c. Heat potential d. Convertibility Temperature at which the vapor pressure is equal to atmospheric pressure Increases when a solute is The vapor pressure of a liquid a. added to the liquid Is independent of temperature c. Equals atmospheric b. Most important intermolecular forces found between water molecules pressure at liquid's boiling point d. Decreases with an increase The pressure required to liquefy a gas at its critical temperature in temperature a. Melting point b. Boiling point c. Freezing point d. Eutectic point a. Constitutive b. Additive property of solution c. Accumulative d. Colligative a. Raoult's law b. Clausius 'Clapeyron Equation c. Van Slyke equation d. Van't hoff's equation lon-induced dipole A point at which the liquid and solid phase have the same composition C. Solutions of lower osmotic pressure than that of the а. Нурertonic b. Нурotonic c. Isotonic d. None of the above a. London dispersion forces b. lon-dipole forces c. Dipole-dipole forces d. Hydrogen bonding body fluid Osmotic pressure is Type of intermolecular force is present in all substances, regardless of polarity Equation that gives the relationship between the vapor pressure and the absolute temperature of a liquid a. Polymerism b. Isomerism Existence of elemental substances such as carbon and sulfur, in more than one crystalline form c. Polymorphism d. Solvates Attractive interaction between a polar molecule and the induces dipole a. interaction a. Dipole-dipole forces between water molecules b. London dispersion forces between water molecules c. Hydrogen bonds between water molecules d. Molecule-ion attraction Explains the very high melting and boiling point of b. Dipole-induced dipole water interaction c. Induced dipole d. lon-Dipole Forces a. Percent by weight b. Molarity c. Molality d. Gram weight a. Covalent b. Electrovalent c. Dipole d. lonic Number of grams of solute in 100 gram of solution between water molecules a. Boyle's law b. Ideal gas law c. Charles' law d. Gay-Lussac's law a. Hydrogen bond b. London dispersion forces c. Dipole-dipole forces d. Molecule-ion attractions Law that governs the relationship between pressure, volume and temperature of gases which is expressed in the following questions, PV=nRT A polar molecule, one region of which is positive and the other negative Strongest intermolecular forces Solution in which the solute is in equilibrium with the solid phase а. Unsaturated b. Subsaturated c. Supersaturated d. Saturated It is the pressure that must be applied to the solution to prevent the flow of pure solvent into the a. Critical pressure b. Vapor pressure c. Atmospheric pressure d. Osmotic pressure a. Normality b. Molarity Molality d. Equivalent weight The number of moles of solute per 1000g of solvent concentrated solution C. a. Enthalpy b. Entropy That portion of energy of a system which cannot be converted to work
Expert Solution
steps

Step by step

Solved in 2 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Electronic Effects
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Principles of Modern Chemistry
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Physical Chemistry
Physical Chemistry
Chemistry
ISBN:
9781133958437
Author:
Ball, David W. (david Warren), BAER, Tomas
Publisher:
Wadsworth Cengage Learning,
SEE MORE TEXTBOOKS