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Study Resources (Chemistry)

11.1   Multiple Choice Questions 1) Which of the following is NOT part of the kinetic molecular theory of gases? A) A gas is composed of very small particles. B) There is very little empty space in a gas. C) Gas particles move rapidly. D) Gas particles do not attract or repel one another. E) Gas particles.
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41) The equilibrium for the solubility of silver sulfate is A) AgSO4 (s) ? Ag+(aq) + 2SO42-(aq) B) Ag2SO4 (s) ? Ag+(aq) + 2SO42-(aq) C) Ag2SO4 (s) ? 2Ag+(aq) + SO42-(aq) D) Ag2SO4 (s) ? 2Ag+(aq) + 2SO42-(aq) E) Ag2SO4 (s) ? Ag2+(aq) + SO42-(aq) 42) The solubility product constant is most useful when examining the.
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11) Carbon tetrachloride, CCl4, is soluble in water. 12) Glucose is a nonelectrolyte. 13) For most solids, solubility decreases as the temperature of the solution increases. 14) The solubility of a gas in water decreases as the temperature increases. 15) The higher the pressure of a gas above a liquid in a closed container,.
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10.5   Short Answer Questions Identify each of the following molecules as polar or nonpolar. 1) carbon tetrachloride 2) water 3) carbon dioxide 4) hydrogen sulfide 5) hydrogen fluoride 6) A bond in which the electrons are shared between atoms is a ________ bond. 7) A molecule in which there are only two atoms held together by covalent bonds.
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13.1   Multiple Choice Questions 1) A catalyst is A) a reactant in a chemical reaction. B) a product in a chemical reaction. C) a substance that speeds up a reaction without being consumed in the reaction. D) a substance that increases the energy of the products. E) a substance that decreases the energy of the products. 2).
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31) The value of the equilibrium constant for the combination of nitrogen and oxygen to make NO is 2 ? 10-9.  What does this tell you about the concentrations of materials in the equilibrium mixture? A) The concentration of products exceeds the concentration of reactants. B) The concentrations of reactants and products.
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13.2   Bimodal Questions 1) What is the value of the equilibrium constant Kc if the concentration of NO and NOBr are   and the concentration of Br2 is 3.0 M? 2NOBr(g) ? 2NO(g) + Br2(g) A) 0.33 B) 9.0 C) 0.010 D) 3.0 E) 2.0 2) For the following reaction, the equilibrium constant Kc is 2.0 at.
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Identify the following solutions as acid, base, or neutral. A) base B) neutral C) acid 16) has a sour taste 17) has a pH = 4.5 18) turns blue litmus red 19) contains more hydronium ions than hydroxide ions 20) H2O 21) [H3O+] = 3.4 × 10-5 M 22) [OH-]= 2.8 x 10-2 M 23) Ca(OH)2 24) pH = 9.0 25) [H3O+] =.
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12.2   Bimodal Questions 1) Acetic acid can be classified as a(n) ________. A) gas B) solid C) weak electrolyte D) strong electrolyte E) ionic compound 2) The molarity of a solution of 5.00 g of KCl in 150. mL of solution is ________. A) 0.0382 M B) 0.0667 M C) 0.447 M D) 0.132 M E) 33.3 M 3) How many grams of.
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14.3   Matching Questions Identify each of the following compounds as an acid, a base, or neither. A) neither B) base C) acid 1) HCl 2) NaOH 3) NH3 4) H2SO4 5) CO32- 6) NaCl 7) CN- 8) H2CO3 In the following solutions, is the [OH-] greater than, less than, or equal to the [H3O+]? A) less than B) greater than C) equal to 9) acid 10) base 11) [H3O+].
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13.3   True/False Questions 1) An equilibrium constant greater than 1 for a reaction indicates that the reaction favors formation of the products. 2) An equilibrium constant Kc = 1 × 107 for a reaction indicates that the reaction favors product formation. 3) If the equilibrium constant for a reaction is 1 × 10-5,.
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31) When sucrose, C12H22O11, is dissolved in water, the sucrose is classified as the ________. A) solute B) solvent C) solution D) electrolyte E) ion 32) Vinegar is a solution of acetic acid (melting point 16.5 °C) in water. At room temperature (25 °C), vinegar is an example of a ________ solution. A) liquid-liquid B) gas-liquid C) solid-liquid D) solid-solid E).
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12.1   Multiple Choice Questions 1) The O-H bond in water is polar because A) it is an ionic bond. B) oxygen is much more electronegative than hydrogen. C) oxygen occupies more space than hydrogen. D) hydrogen is much more electronegative than oxygen. E) it is a hydrogen bond. 2) A hydrogen bond is A) an attraction between a.
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10.3   Matching Questions Indicate the type of bonding you would expect between the following elements. A) polar covalent B) ionic C) none D) nonpolar covalent 1) Na and F 2) N and F 3) F and F 4) He and F 5) H and F Match the molecule to its shape. A) trigonal pyramidal B) tetrahedral C) trigonal planar D) linear E) sulfur oxide F) bent 6) H2S.
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41) The conjugate base of H2S is ________. A) OH- B) H2O C) HOS D) HS- E) HS2 42) Bicarbonate ion, HCO3-, is an example of a(n) ________ substance. A) neutral B) amphoteric C) strongly acidic D) strongly basic E) gaseous 43) Bicarbonate ion, HCO3-, is an example of a(n) ________. A) weak base B) strong acid C) gas D) Arrhenius acid E) Arrhenius base 44) When.
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36) In the kinetic molecular theory of gas behavior, the assumption is made that gas molecules A) move rapidly in random directions. B) are attracted to each other by strong forces. C) are close together in their container. D) move with a kinetic energy equal to their centigrade temperature. E) occasionally come to rest. 37) The.
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A balloon is filled with helium gas. For the following questions, select the letter of the balloon diagram that corresponds to the given change in conditions. 16) The balloon is put into a chamber whose pressure is less than the atmospheric pressure and at atmospheric temperature. A) Balloon A B) Balloon B C) Balloon.
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31) In the following list, which is the polar compound? A) H2O B) CCl4 C) CO2 D) BF3 E) N2 32) The HF molecule can be classified as ________. A) polar covalent B) nonpolar C) ionic D) bent E) planar 33) Which is the most polar bond in the following list? A) O-H B) S-O C) C-S D) I-I E) P-H 34) A molecule has a central atom.
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41) In the reaction of silver nitrate and sodium chloride to produce solid silver chloride, sodium ions and nitrate ions are ________. A) spectator ions B) solvents C) molecules D) gases E) liquids 42) Calcium chloride reacts with sodium hydroxide to form solid calcium hydroxide, Ca(OH)2. The balanced net ionic equation is A) Ca+2(aq) + 2OH-(aq) +.
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10.2   Bimodal Questions 1) The diatomic molecule N2 is held together by a ________ covalent bond. A) double B) single C) ionized D) triple E) polar 2) The diatomic molecule Cl2 is held together by a ________ covalent bond. A) single B) double C) ionized D) polar E) triple 3) The main interactions between molecules of methane, CH4, are ________. A) ionic bonds B) dispersion.
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14.4   True/False Questions 1) A buffer is a solution that tends to maintain a neutral pH. 2) A solution of NaOH will turn phenolphthalein pink. 3) A solution of NaOH will feel slippery. 4) A solution of HCl will taste bitter. 5) In any water solution, [H3O+] [OH-] = 1 × 10-7. 6) An ammonium chloride.
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10.4   True/False Questions 1) Ammonia is a nonpolar molecule. 2) The carbon-chlorine covalent bond is polar. 3) The ammonia molecule has a lone pair of electrons located on the nitrogen atom. 4) N2 is held together by a multiple covalent bond. 5) The total number of valence electrons in the fluorine molecule, F2, is.
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12.3   Matching Questions Identify the term defined in each description. A) weak electrolyte B) strong electrolyte C) hydrogen bonding D) net ionic equation E) solvent F) dissociation G) solute H) unsaturated I) ionic equation J) nonelectrolyte K) solution L) saturated 1) a solution that contains the highest amount of solute that dissolves at a given temperature 2) the major attraction between water molecules 3) a solution.
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11.5   Short Answer Questions 1) The use of high-pressure chambers to control disease processes is known as ________ medicine. 2) Nitrogen makes up about ________ percent of the atmosphere. 3) A barometer is usually filled with ________. 4) One atmosphere is the same as ________ mmHg. 5) The pressure unit 1 mmHg is the same.
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13.4   Short Answer Questions 1) The rule or principle that describes the effect of changing reaction conditions on an equilibrium is known as ________ principle. 2) The minimum energy needed to convert reactants to products is the ________. 3) A substance that increases the rate of a reaction by lowering the activation reaction.
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11.3   Matching Questions Indicate the effect of each change upon the pressure of a gas. A) no change B) decreases C) increases 1) decrease in volume (n, T constant) 2) The temperature is doubled. 3) The volume and the Kelvin temperature are reduced by one-half. 4) A leak occurs and gas escapes. 5) increase in volume, increase in temperature 6).
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12.5   Short Answer Questions 1) In the following equation, ________ will precipitate from solution. BaCl2 + H2SO4 → BaSO4 + 2HCl 2) The number of moles of a compound dissolved in one liter of a solution is called the ________. 3) A substance that carries an electric current when dissolved in water is called.
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21) Refrigerating perishable foods affects biochemical reactions by A) increasing concentrations of antioxidants. B) removing bacteria. C) decreasing the rate of reactions affecting spoilage. D) catalyzing the removal of harmful chemicals from the foods. E) improving the appearance of the foods. 22) In a catalytic converter in an automobile, the reaction of carbon monoxide with.
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10.1   Multiple Choice Questions 1) Double and triple bonds form because A) the atoms involved have high electronegativities. B) single covalent bonds do not give all of the atoms in the molecule eight valence electrons. C) one of the atoms in the molecule has more than 8 valence electrons. D) the ions involved have charges.
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14.1   Multiple Choice Questions 1) According to the Arrhenius concept, if HNO3 were dissolved in water, it would act as ________. A) a base B) an acid C) a source of hydroxide ions D) a source of H- ions E) a proton acceptor 2) The name given to an aqueous solution of HBr is ________. A) hydrogen bromide B).
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12.4   True/False Questions 1) Lithium chloride is soluble in water. 2) The molarity of a solution is the mass of solute divided by the solution volume. 3) The m/m % concentration of a solution is the mass of the solution divided by its volume multiplied by 100. 4) The m/m % concentration of a.
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14.2   Bimodal Questions 1) The correct formula for sulfuric acid is ________. A) H2SO4 B) H2SO3 C) H2SO4- D) H2SO3- E) SO42- 2) What is the pH of a solution with [H3O+] = 1.0 × 10-9 M? A) 1.0 × 10-5 B) -9.0 C) 5.0 D) -5.0 E) 9.0 3) What is the pH of a solution with [OH-] = 1.0 ×.
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11.2   Bimodal Questions 1) The pressure exerted by the particles of vapor above a liquid is called the ________ pressure. A) vapor B) barometric C) standard D) molar E) atmospheric 2) A barometer is a device for measuring ________. A) atmospheric pressure B) blood pressure C) gas pressure in a container D) gas pressure in the.
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