When the equation for this reaction is correctly balanced and all coefficients are reduced to their lowest whole-number term, the coefficient for O2 is, 10 HI + 2 KMnO4 + 3 H2SO4 5 I2 + 2 MnSO4 + K2SO4 + 8 H2O. The electron-dot structure (Lewis structure) for which of the following molecules would have two unshared pairs of electrons on the central atom? Represents an atom that has four valence electrons. Which of the following describes the changes in forces of attraction that occur as H2O changes phase from a liquid to a vapor? On the basis of the solubility curves shown above, the greatest percentage of which compound can be recovered by cooling a saturated solution of that compound from 90o to 30o? P5.24) One mole of H2O(l) is supercooled to –2.25ºC at 1 bar pressure. Types of hybridization exhibited by the C atoms in propene, CH3CHCH2, include which of the following? The cooling curve above shows how the temperature of a sample varies with time as the sample goes through phase changes. H3AsO3(aq) + . Liquid naphthalene at 95oC was cooled to 30oC, as represented in the cooling curve above. Explanations for this observation include which of the following? BRILLIANT PUBLIC SCHOOL, SITAMARHI (Affiliated up to +2 level to C.B.S.E., New Delhi) Class-XI IIT-JEE Advanced Chemistry Study Package Session: 2014-15 Office: Rajopatti, Dumra Road, Sitamarhi (Bihar), Pin-843301 Ph.06226-252314 , Mobile:9431636758, 9931610902 Website: www.brilliantpublicschool.com; E-mail: [email protected][email protected] On the basis of strength of intermolecular forces, which of the following elements would be expected to have the highest melting point? The London (dispersion) forces are weakest for which of the following gases under the same conditions of temperature and pressure? The weight of H2SO4 (molecular weight 98.1) in 50.0 milliliters of a 6.00-molar solution is, When a hydrate of Na2CO3 is heated until all the water is removed, it loses 54.3 percent of its mass. Which of the following aqueous solutions has the highest boiling point? Ag(s) + . The pH of a solution prepared by the addition of 10. mL of 0.002 M KOH(aq) to 10. mL of distilled water is closest to. Studyres contains millions of educational documents, questions and answers, notes about the course, tutoring questions, cards and course recommendations that will help you learn and learn. The metal calcium reacts with molecular hydrogen to form a compound. How many mL of 10.0 M HCl are needed to prepare 500. mL of 2.00 M HCl? How many grams of calcium nitrate, Ca(NO3)2, contains 24 grams of oxygen atoms? Which of the following techniques is the most appropriate for the recovery of solid KNO3 from an aqueous solution of KNO3? The mole fraction of CH3OH in this solution is closest to which of the following? A 1.0 L sample of an aqueous solution contains 0.10 mol of NaCl and 0.10 mol of CaCl2. The atom that contains only one electron in the highest occupied energy sublevel. To determine the molar mass of a solid monoprotic acid, a student titrated a weighed sample of the acid with standardized aquesous NaOH. 42.8 grams of KIO3 and add 2.00 kilograms of H2O d. 42.8 grams of KIO3 and add 2.00 liters of H2O b. What is the empirical formula for this compound? H2O and different impurities of a neutral salt consumed 18.9 ml of 0.5 N NaOH solution. An excess of Mg(s) is added to 100. mL of 0.400 M HCl. What is the hybridization of the carbon atom in a molecule of ethyne, represented above? A possible formula for the hydrocarbon is. Which of the following is the most likely explanation for this difference? Predicts that it is impossible to determine simultaneously the exact position and the exact velocity of an electron. What volume of 0.150-molar HCl is required to neutralize 25.0 mililiters of 0.120-molar Ba(OH)2? According to the VSEPR model, the progressive decrease in the bond angles in the series of molecules CH4, NH3, and H2O is best accounted for by the, increasing the number of unshared pairs of electrons, At standard temperature and pressure, a 0.50 mol sample of H2 gas and a separate 1.0 mol sample of O2 gas have the same, ___Li3N (s) + ___H2O (l) ___Li+ (aq) + ___OH- (aq) + ___NH3 (g), The best explanation for the fact that diamond is extremely hard is that diamond crystals, are giant molecules in which each atom forms strong covalent bonds with all of its neighboring atoms. 3 Cu(s) + 8 H+(aq) + 2 NO3-(aq) 3 Cu2+(aq) + 2 NO(g) + 4 H2O(l). What would be the pressure of this sample at 15° C and the same volume? The proper procedure is to weigh out, 42.8 grams of KIO3 and add H2O until the final homogeneous solution has a volume of 2.00 liters, A 2.00-liter sample of nitrogen gas at 27 °C and 600. millimeters of mercury is heated until it occupies a volume of 5.00 liters. Calculate the equilibrium and hydrogen. The volume of hydrogen gas produced at standard temperature and pressure is. At which time does the sample contain the most liquid? isomer - same molecular formula but different chemical structure, The cooling curve for a pure substance as it changes from a liquid to a solid is shown above. Which element exhibits the greatest number of different oxidation states? (R = 0.0821 liter-atm / mole-K), As the temperature is raised from 20 ° C to 40 ° C, the average kinetic energy of neon atoms changes by a factor of, What number of moles of O2 is needed to produce 14.2 grams of P4O10 from P? An oxidation-reduction reaction that is also a synthesis reaction. In which of the following processes are covalent bonds broken? A possible atomic weight of Q is, Is used to explain the fact that the four bonds in methane are equivalent, The simplest formula for an oxide of nitrogen that is 36.8 percent nitrogen by weight is. When a sample of oxygen gas in a closed container of constant volume is heated until its absolute temperature is doubled, which of the following is also doubled? The energy required to convert a ground-state atom in the gas phase to a gaseous positive ion. Which ions must be absent on the basis of each of the following observations of the "unknown"? Propane gas, C3H8, burns in excess oxygen gas. It is suggested that SO2 (molar mass 64 grams), which contributes to acid rain, could be removed from a stream of waste gases by bubbling the gases through 0.25-molar KOH, therby producing K2SO3 . . The solution contains a salt of. Hydrogen gas is collected over water at 24 °C. They have oxides that are acid anhydrides. __ Cr2O72¯ + __ e¯ + __ H+ __ Cr3+ + __ H2O(l) When the equation for the half reaction above is balanced with the lowest whole-number coefficients, the coefficient for H2O is. The partial pressure of O2(g) in the system is, A hydrocarbon gas with an empirical formula CH2 has a density of 1.88 grams per liter at 0 °C and 1.00 atmosphere. Which of the following does NOT behave as an electrolyte when it is dissolved in water? Substances X and Y that were in a solution were separated in the laboratory using the technique of fractional crystalization. just pick the picture that has 2NH3 and 2H2. It depends on the relative molecular masses of X, Y, and Z. In which of the following species does sulfur have the same oxidation number as it does in H2SO4? Equal masses of He and Ne are placed in a sealed container. A mixture of reactants and product at 1400 K contains 0.035 M H2O… .....Mg(s) + .....NO3¯(aq) +.....H+(aq) --->......Mg2+(aq) + ....NH4+(aq) + ....H2O(l), The system shown above is at equilibrium at 28 °C. In a molecule in which the central atom exhibits sp3d2 hybrid orbitals, the electron pairs are directed toward the corners of. A student wishes to prepare 2.00 liters of 0.100-molar KIO3 (molecular weight 214). Which of the following is the best explanation for this observation? What is the molar mass of the gas? the positive charge of an atom is concentrated in a small region. Ag+ + . the molality of the solution remains unchanged. . A sample of 9.00 grams of aluminum metal is added to an excess of hydrochloric acid. concentrations of PCl5, PCl3 and Cl2 if only PCl5 is H2O(g) + CH4(g) CO(g) + 3H2(g) present initially, at a concentration of 0.160 M. Kc = 4.7 at 1400 K Sol. What mass of Au is produced when 0.0500 mol of Au2S3 is reduced completely with excess H2? The following results were obtained. Each sample was then titrated with a sodium hydroxide solution to the appearance of the first permanent faint pink color. Molecules that have planar configurations include which of the following? Closely packed lattice with delocalized electrons throughout, In solid methane, the forces between neighboring CH4 molecules are best characterized as. The sample starts as a gas, and heat is removed at a constant rate. A sample of 3.30 grams of an ideal gas at 150.0 °C and 1.25 atmospheres pressure has a volume of 2.00 liters. W. H. FREEMAN AND COMPANY San Francisco Sponsoring Editor: Peter Renz Project Editor: Nancy Flight Manuscript Editor: Larry McCombs Designer: Marie Carluccio Production Coordinator: William Murdock Illustration … The reason for this precaution is to ensure that, there is a sufficient volume of water to absorb to the heat released. (Assume volumes are additive.). F- has a larger nuclear charge than O2- has. . Of the following electron configurations of neutral atoms, which represents an atom in an excited state? The dehydrated sample absorbed moisture after heating. Is used to explain the fact that the carbon-to-carbon bonds in benzene, C6H6, are identical, The density of an unknown gas is 4.20 grams per liter at 3.00 atmospheres pressure and 127 °C. If 200. mL of 0.60 M MgCl2(aq) is added to 400. mL of distilled water, what is the concentration of Mg2+(aq) in the resulting solution? How many milliliters of 11.6-molar HCl must be diluted to obtain 1.0 L of 3.0-molar HCl? In which of the following groups are the three species isoelectronic; i.e., have the same number of electrons? The Good Egg Presents: The Great Eggscape! The freezing temperature of water at this pressure is 0.00ºC. A measured mass of an unreactive metal was dropped into a small graduated cylinder half filled with water. Which of the following could explain why the student obtained a molar mass that was too LARGE? Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC2H3O2. A 27.0-gram sample of an unknown hydrocarbon was burned in excess oxygen to form 88.0 grams of carbon dioxide and 27.0 grams of water. A rigid metal tank contains oxygen gas. . The concentration of barium ion, Ba2+, in solution after reaction is. What is the molecular weight of this gas? What is the molarity of a solution of phosphoric acid, H3PO4, that contains 24.5 g of phosphoric acid (molar mass 98.0 g) in 100. g of H2O? This difference in boiling points may be attributed to a difference in. The correct value for the percentage of water in the hydrate is 51 percent. The relatively high boiling point of HF can be correctly explained by which of the following? Under which of the following conditions of temperature and pressure would 1.0 mol of the real gas CO2(g) behave most like an ideal gas? Strong single covalent bonds with weak intermolecular forces, When diluting concentrated H2SO4, one should slowly add acid to a beaker of water rather than add water to a beaker of acid. Oh no! A compound contains 30. percent sulfur and 70. percent fluorine by mass. Given that there are only two naturally occurring isotopes of copper, 63Cu and 65Cu, the natural abundance of the 65Cu isotope must be approximately. How to Destroy America in Three Easy Steps, 81% found this document useful (16 votes), 81% found this document useful, Mark this document as useful, 19% found this document not useful, Mark this document as not useful. Which of the following represents acceptable laboratory practice? ...CrO2¯ + ...OH¯ ... CrO42¯ + ... H2O + ... e¯ When the equation for the half-reaction above is balanced, what is the ratio of the coefficients OH¯ / CrO2¯ ? What is the minimum number of moles of AgNO3 that must be added to the solution in order to precipitate all of the Cl- as AgCl (s) ? . Which of the following molecules has an angular (bent) geometry that is commonly represented as a resonance hybrid of two or more electron-dot structures? __ CH3CH2COOH(l) + __ O2(g) __ CO2(g) + __ H2O(l), Forms oxides that are common air pollutants and that yield acidic solution in water. When hafnium metal is heated in an atmosphere of chlorine gas, the product of the reaction is found to contain 62.2 percent Hf by mass and 37.4 percent Cl by mass. When all of the Xe gas reacted, forming a solid compound, the pressure of the unreacted F2 gas was 4.6 atmospheres. 2 H2O(l) + 4 MnO4-(aq) + 3 ClO2-(aq) 4 MnO2(s) + 3 ClO4-(aq) + 4 OH-(aq). (Assume that AgCl is insoluble.). . On titration with KMnO4 solution, 0.4 g of the same substance needed 21.55 ml … At 25°C and 1 atm, is a strong electrolyte in aqueous solution. If 87 g of K2SO4 (molar mass 174 g) is dissolved in enough water to make 250 mL of solution, what are the concentrations of potassium and sulfate ion respectively? A hot-air balloon rises. H2O. If the pressure remains unchanged, the final temperature of the gas is. We must also account for the Na+ and Cl-, so NaCl (aq) seems reasonable. Which of the following acids can be oxidized to form a stronger acid? Therefore, the hybridization of Sb orbitals should be. Is used to explain why iodine molecules are held together in the solid state. Conway Pierce Late of University of California Riverside. Which of the following statements regarding these gas samples is FALSE? One holds 0.50 gram of hydrogen and the other holds 8.0 grams of oxygen. Which of the following is necessary to calculate the molecular weight of the gas, but does NOT need to be measured during the experiment? Get all of Hollywood.com's best Celebrities lists, news, and more. The average speed of the hydrogen molecules is the same as the average speed of the oxygen molecules. The Lewis dot structure of which of the following molecules shows only one unshared pair of valence electron? A 360. mg sample of aspirin, C9H8O4, (molar mass 180. g), is dissolved in enough water to produce 200. mL of solution. Assume that you have an "unknown" consisting of an aqueous solution of a salt that contains one of the ions listed below. . What is the molarity of aspirin in a 50. mL sample of this solution? Which of the following molecules contains only single bonds? CCl4, CO2, PCl3, PCl5, SF6 Which of the following does not describe any of the molecules above? Which of the following does NOT liberate heat when water is added to it? All of the following statements concerning this compound are true EXCEPT: When added to water, it forms an acidic solution. We would like to show you a description here but the site won’t allow us. When the actual gas volume is greater then the volume predicted by the ideal gas law, the explanation lies in the fact that the ideal gas law does NOT include a factor for molecular. A 20.0-milliliter sample of 0.200-molar K2CO3 solution is added to 30.0 milliliters of 0.400-molar Ba(NO3)2 solution. This difference best accounts for which of the following? Which of the following characteristics is common to elemental sulfur, chlorine, nitrogen, and carbon? Of the following pure substances, which has the highest melting point? Of the following molecules, which has the largest dipole moment? The total pressure of the gases in the flask is 800 mm Hg. Two flexible containers for gases are at the same temperature and pressure. Barium carbonate precipitates. Can be used to predict that a gaseous carbon atom in its ground state is paramagnetic, Hund's rule (principle of maximum multiplicity), The ground-state configuration of a negative ion of a halogen, 5 Fe2+ + MnO4¯ + 8 H+ 5 Fe3+ + Mn2+ + 4 H2O, When 70. milliliter of 3.0-molar Na2CO3 is added to 30. milliliters of 1.0-molar NaHCO3 the resulting concentration of Na+ is, The mass of element Q found in 1.00 mole of each of four different compounds is 38.0 grams, 57.0 grams, 76.0 grams, and 114 grams, respectively. How many moles of solid Ba(NO3)2 should be added to 300. milliliters of 0.20-molar Fe(NO3)3 to increase the concentration of the NO3¯ ion to 1.0-molar? In which of the following compounds is the mass ratio of chromium to oxygen closest to 1.62 to 1.00 ? The melting point of MgO is higher than that of NaF. At this temperature, the vapor pressure of water is 28 millimeters of mercury. Which of the following molecules has the shortest bond length? Which of the following represents a pair of isotopes? Which of the following represents the ground state electron configuration for the Mn3+ ion? The boiling points of the elements helium, neon, argon, krypton, and xenon increase in that order. At 25 °C and 1 atm, has molecules with a pyramidal shape. Find the training resources you need for all your activities. To ensure the best experience, please update your browser. What is the partial pressure of the nitrogen? The diagram above represents H2(g) and N2(g) in a closed container. Knowing that an acid and a compound with carbonate form carbon dioxide and water, reasonable products are CO2 and H2O. Which of the elements above has the smallest ionic radius for its most commonly found ion? What is the most electronegative element of the below? At 0oC and 1 atm pressure, what volume of H2 gas can be obtained? Appropriate laboratory procedures include which of the following? Sodium chloride is LEAST soluble in which of the following liquids? (Assume that the volume of the solution remains constant.). From which section of the curve can the melting point of naphthalene be determined? (Assume that the volumes are additive.). Which of the following best helps to account for the fact that the F- ion is smaller than the O2- ion? The formula of the hydrate is, CH4(g) + 2 O2(g) CO2(g) + 2 H2O(l); H = - 889.1 kJ, The net ionic equation for the reaction between silver carbonate and hydrochloric acid is, 2 Ag+ + CO32¯ + 2 H+ + 2 Cl¯ --> 2 AgCl(s) + H2O + CO2(g), The geometry of the SO3 molecule is best described as. This fractional crystalization is possible because substances X and Y have different, The net ionic equation for the reaction that occurs during the titration of nitrous aicd with sodium hydroxide is, A solution is known to contain an inorganic salt of one of the following elements. Secrets of the Millionaire Mind: Mastering the Inner Game of Wealth, Getting Things Done: The Art of Stress-free Productivity, The Subtle Art of Not Giving a F*ck: A Counterintuitive Approach to Living a Good Life, The Extraordinary Life of Sam Hell: A Novel. The oxidation state that is common to aqueous ions of Fe, Mn, and Zn is. What is the formula of the compound? In the periodic table, as the atomic number increases from 11 to 17, what happens to the atomic radius? In a laboratory experiment, H2(g) is collected over water in a gas-collection tube as shown in the diagram above. Which of the following conclusions can be drawn from J. J. Thomson's cathode ray experiments? The elements in which of the following have most nearly the same atomic radius? Which of the following applies to the gas in the tank when additional oxygen is added at constant temperature? The temperature of the water is 21°C and the atmospheric pressure in the laboratory is measured to be 772 torr. . Represents an atom of a transition metal. What is the partial pressure of the SO2(g) in the flask? Based on the information above, what is the standard enthalpy change for the following reaction? The solid and liquid coexist at. The average speed of the gas molecules remains the same. a. (Atomic number Mn = 25). ...Cr2O72-(aq) + ...H2S(g) + ...H+(aq) ...Cr3+(aq) + ...S(s) + ...H2O(l). (Molecular weight P4O10 = 284). Samples of F2 gas and Xe gas are mixed in a container of fixed volume. Is added to silicon to enhance its properties as a semiconductor. ...H+(aq) + ...NO2-(aq) + ... Cr2O72-(aq) ...Cr3+(aq) + ...NO3-(aq) + ...H2O(l). What is the partial pressure of He if the total pressure in the container is 6 atm? Hydrogen bonds between H2O molecules are broken. The gas constant, R, is 0.0821 L atm mol¯1 K¯1). The solution is colorless. Approximately what mass of CuSO4•5H2O (250 g mol-1) is required to prepare 250 mL of 0.10 M copper(II) sulfate solution? For which of the following molecules are resonance structures necessary to describe the bonding satisfactorily? Forms monatomic ions with 2- charge in solutions. Which of the following is probably true for a solid solute with a highly endothermic heat of solution when dissolved in water? Which of the following elements combines with oxygen to form a covalent network solid? What was the concentration of acetic acid in the vinegar if no other acid was present? Which of the following best describes what happens to the substance between t4 and t5? The following measurements were made. A compound is heated to produce a gas whose molecular weight is to be determined. . The initial partial pressure of the F2 gas is 8.0 atmospheres and that of the Xe gas is 1.7 atmospheres. A 40.0 mL sample of 0.25 M KOH is added to 60.0 mL of 0.15 M Ba(OH)2. . What is the simplest formula of this compound? Which of the following ions has the same number of electrons as Br? Which of the following pieces of laboratory glassware should be used to most accurately measure out a 25.00 mL sample of a solution, Are the most difficult to iodize in a given period of the periodic table. Which of the following properties generally decreases across the periodic table from sodium to chlorine? The recorded measurements are shown in the table above. The density of a pure liquid at 25°C was calculated by determining the mass and volume of a sample of the liquid. What is the partial pressure of the hydrogen gas? Strong multiple covalent bonds (including p-bonds) with weak intermolecular forces. By calculating ∆S, ∆Ssurroundings and ∆Stotal , verify that this transformation is spontaneous at –2.25ºC. Studyres contains millions of educational documents, questions and answers, notes about the course, tutoring questions, cards and course recommendations that will help you learn and learn.
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