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chemistry
organic chemistry
Questions and Answers of
Organic Chemistry
Write a balanced equation for each of the following processes: (a) On heating, ammonium nitrate produces nitrous oxide. (b) On heating, potassium nitrate produces potassium nitrite and oxygen
Explain why, under normal conditions, the reaction of zinc with nitric acid does not produce hydrogen.
Potassium nitrite can be produced by heating a mixture of potassium nitrate and carbon. Write a balanced equation for this reaction. Calculate the theoretical yield of KNO2 produced by heating 57.0 g
Predict the geometry of nitrous oxide, N2O, by the VSEPR method and draw resonance structures for the molecule.
Consider the reaction N2(g) + O2(g) ⇌ 2NO(g) Given that the ΔG° for the reaction at 298 K is 173.4 kJ/mol, calculate (a) The standard free energy of formation of NO, (b) KP for the reaction,
From the data in Appendix 3, calculate DH° for the synthesis of NO (which is the first step in the manufacture of nitric acid) at 25°C: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(l)
Explain why two N atoms can form a double bond or a triple bond, whereas two P atoms normally can form only a single bond.
When 1.645 g of white phosphorus are dissolved in 75.5 g of CS2, the solution boils at 46.709°C, whereas pure CS2 boils at 46.300°C. The molal boiling-point elevation constant for CS2 is 2.34°C/m.
Starting with elemental phosphorus, P4, show how you would prepare phosphoric acid.
Dinitrogen pentoxide is a product of the reaction between P4O10 and HNO3. Write a balanced equation for this reaction. Calculate the theoretical yield of N2O5 if 79.4 g of P4O10 are reacted with an
Explain why (a) NH3 is more basic than PH3, (b) NH3 has a higher boiling point than PH3, (c) PCl5 exists but NCl5 does not, (d) N2 is more inert than P4.
Draw molecular orbital energy level diagrams for O2, O2-, and O22-.
One of the steps involved in the depletion of ozone in the stratosphere by nitric oxide may be represented as NO(g) + O3(g) → NO2(g) + O2(g) From the data in Appendix 3 calculate ΔG°, KP, and Kc
Hydrogen peroxide is unstable and decomposes readily: 2H2O2(aq) → 2H2O(l) + O2(g) This reaction is accelerated by light, heat, or a catalyst. (a) Explain why hydrogen peroxide sold in drugstores
What are the oxidation numbers of O and F in HFO?
In 2004, about 48 million tons of sulfuric acid were produced in the United States. Calculate the amount of sulfur (in grams and moles) used to produce that amount of sulfuric acid.
Sulfuric acid is a dehydrating agent. Write balanced equations for the reactions between sulfuric acid and the following substances: (a) HCOOH, (b) H3PO4, (c) HNO3, (d) HClO3.
Calculate the amount of CaCO3 (in grams) that would be required to react with 50.6 g of SO2 emitted by a power plant.
Explain why SCl6, SBr6, and SI6 cannot be prepared.
Compare the physical and chemical properties of H2O and H2S.
The bad smell of water containing hydrogen sulfide can be removed by the action of chlorine. The reaction is H2S(aq) + Cl2(aq) → 2HCl(aq) + S(s) If the hydrogen sulfide content of contaminated
Describe two reactions in which sulfuric acid acts as an oxidizing agent.
Concentrated sulfuric acid reacts with sodium iodide to produce molecular iodine, hydrogen sulfide, and sodium hydrogen sulfate. Write a balanced equation for the reaction.
Metal chlorides can be prepared in a number of ways: (a) Direct combination of metal and molecular chlorine, (b) Reaction between metal and hydrochloric acid, (c) Acid-base neutralization, (d) Metal
Sulfuric acid is a weaker acid than hydrochloric acid. Yet hydrogen chloride is evolved when concentrated sulfuric acid is added to sodium chloride. Explain.
Show that chlorine, bromine, and iodine are very much alike by giving an account of their behavior (a) With hydrogen, (b) In producing silver salts, (c) As oxidizing agents, and (d) With sodium
A 375-gallon tank is filled with water containing 167 g of bromine in the form of Br- ions. How many liters of Cl2 gas at 1.00 atm and 20°C will be required to oxidize all the bromide to molecular
Draw structures for (a) (HF)2 and (b) HF2-
Hydrogen fluoride can be prepared by the action of sulfuric acid on sodium fluoride. Explain why hydrogen bromide cannot be prepared by the action of the same acid on sodium bromide.
Aqueous copper(II) sulfate solution is blue. When aqueous potassium fluoride is added to the CuSO4 solution, a green precipitate is formed. If aqueous potassium chloride is added instead, a
What volume of bromine (Br2) vapor measured at 100°C and 700 mmHg pressure would be obtained if 2.00 L of dry chlorine (Cl2), measured at 15°C and 760 mmHg, were absorbed by a potassium bromide
Use the VSEPR method to predict the geometries of the following species: (a) I3-, (b) SiCl4, (c) PF5, (d) SF4.
Iodine pentoxide, I2O5, is sometimes used to remove carbon monoxide from the air by forming carbon dioxide and iodine. Write a balanced equation for this reaction and identify species that are
Write a balanced equation for each of the following reactions: (a) Heating phosphorous acid yields phosphoric acid and phosphine (PH3). (b) Lithium carbide reacts with hydrochloric acid to give
(a) Which of the following compounds has the greatest ionic character? PCl5, SiCl4, CCl4, BCl3 (b) Which of the following ions has the smallest ionic radius? F-, C4-, N3-, O2- (c) Which of the
Both N2O and O2 support combustion. Suggest one physical and one chemical test to distinguish between the two gases.
Describe the bonding in the C22- ion in terms of the molecular orbital theory.
Starting with deuterium oxide (D2O), describe how you would prepare (a) NaOD, (b) DCl, (c) ND3, (d) C2D2, (e) CD4, (f) D2SO4.
Solid PCl5 exists as [PCl4+][PCl6-]. Draw Lewis structures for these ions. Describe the hybridization state of the P atoms.
Consider the Frasch process. (a) How is it possible to heat water well above 100°C without turning it into steam? (b) Why is water sent down the outermost pipe? (c) Why would excavating a mine and
Complete the following statements for the complex ion [Co(en)2(H2O)CN]2+. (a) En is the abbreviation for _____. (b) The oxidation number of Co is _____. (c) The coordination number of Co is
Complete the following statements for the complex ion [Cr(C2O4)2(H2O)2]-. (a) The oxidation number of Cr is ______. (b) The coordination number of Cr is ______. (c) _____ is a bidentate ligand.
Give the oxidation numbers of the metals in the following species: (a) K3[Fe(CN)6], (b) K3[Cr(C2O4)3], (c) [Ni(CN)4]2-.
Give the oxidation numbers of the metals in the following species: (a) Na2MoO4, (b) MgWO4, (c) Fe(CO)5.
What are the systematic names for the following ions and compounds? (a) [Co(NH3)4Cl2]+ (b) Cr(NH3)3Cl3 (c) [Co(en)2Br2]+ (d) [Co(NH3)6]Cl3
What are the systematic names for the following ion and compounds? (a) [cis-Co(en)2Cl2]+ (b) [Pt(NH3)5Cl]Cl3 (c) [Co(NH3)5Cl]Cl2
Write the formulas for each of the following ions and compounds: (a) Tetrahydroxozincate(II), (b) Pentaaquachlorochromium(III) chloride, (c) tetrabromocuprate( II), (d)
Write the formulas for each of the following ions and compounds: (a) Bis(ethylenediamine)-dichlorochromium(III), (b) Pentacarbonyliron(0), (c) Potassium tetracyanocuprate(II), (d)
The complex ion [Ni(CN)2Br2]2- has a square-planar geometry. Draw the structures of the geometric isomers of this complex.
How many geometric isomers are in the following species? (a) [Co(NH3)2Cl4]-, (b) [Co(NH3)3Cl3]
Draw structures of all the geometric and optical isomers of each of the following cobalt complexes: (a) [Co(NH3)6]3+ (b) [Co(NH3)5Cl]2+ (c) [Co(C2O4)3]3-
Draw structures of all the geometric and optical isomers of each of the following cobalt complexes: (a) [Co(NH3)4Cl2]+, (b) [Co(en)3]3+.
The [Ni(CN)4]2- ion, which has a square-planar geometry, is diamagnetic, whereas the [NiCl4]2- ion, which has a tetrahedral geometry, is paramagnetic. Show the crystal field splitting diagrams for
Transition metal complexes containing CN- ligands are often yellow in color, whereas those containing H2O ligands are often green or blue. Explain.
Predict the number of unpaired electrons in the following complex ions: (a) [Cr(CN)6]4-, (b) [Cr(H2O)6]2+.
The absorption maximum for the complex ion [Co(NH3)6]3+ occurs at 470 nm. (a) Predict the color of the complex and (b) calculate the crystal field splitting in kJ/mol.
From each of the following pairs, choose the complex that absorbs light at a longer wavelength: (a) [Co(NH3)6]2+, [Co(H2O)6]2+; (b) [FeF6]3-,[Fe(CN)6]3-; (c) [Cu(NH3)4]2+, [CuCl4]2-.
A solution made by dissolving 0.875 g of Co(NH3)4Cl3 in 25.0 g of water freezes at 20.56°C. Calculate the number of moles of ions produced when 1 mole of Co(NH3)4Cl3 is dissolved in water and
Oxalic acid, H2C2O4, is sometimes used to clean rust stains from sinks and bathtubs. Explain the chemistry underlying this cleaning action.
The [Fe(CN)6]3- complex is more labile than the [Fe(CN)6]4- complex. Suggest an experiment that would prove that [Fe(CN)6]3- is a labile complex.
Aqueous copper(II) sulfate solution is blue in color. When aqueous potassium fluoride is added, a green precipitate is formed. When aqueous potassium chloride is added instead, a bright-green
When aqueous potassium cyanide is added to a solution of copper(II) sulfate, a white precipitate, soluble in an excess of potassium cyanide, is formed. No precipitate is formed when hydrogen sulfide
A concentrated aqueous copper(II) chloride solution is bright green in color. When diluted with water, the solution becomes light blue. Explain.
In a dilute nitric acid solution, Fe3+ reacts with thiocyanate ion (SCN-) to form a dark-red complex: The equilibrium concentration of [Fe(H2O)5NCS]2+ may be determined by how darkly colored the
Which is a stronger oxidizing agent in aqueous solution, Mn3+ or Cr3+? Explain your choice.
Carbon monoxide binds to Fe in hemoglobin some 200 times more strongly than oxygen. This is the reason why CO is a toxic substance. The metal-to-ligand sigma bond is formed by donating a lone pair
A student has prepared a cobalt complex that has one of the following three structures: [Co(NH3)6]Cl3, [Co(NH3)5Cl]Cl2, or [Co(NH3)4Cl2]Cl. Explain how the student would distinguish between these
Chemical analysis shows that hemoglobin contains 0.34 percent of Fe by mass. What is the minimum possible molar mass of hemoglobin? The actual molar mass of hemoglobin is about 65,000 g. How do you
Explain the following facts: (a) Copper and iron have several oxidation states, whereas zinc has only one. (b) Copper and iron form colored ions, whereas zinc does not.
A student in 1895 prepared three coordination compounds containing chromium, with the following properties:
The formation constant for the reaction Ag+ + 2NH3 [Ag(NH3)2]+ is 1.5 Ã 107 and that for the reaction Ag+ + 2CN- [Ag(CN)2]- is 1.0 Ã 1021 at
From the standard reduction potentials listed in Table 19.1 for Zn/Zn2+ and Cu+/Cu2+, calculate ÎG° and the equilibrium constant for the reaction
Using the standard reduction potentials listed in Table 19.1 and the Handbook of Chemistry and Physics, show that the following reaction is favorable under standard-state conditions:What is the
What are the differences between geometric isomers and optical isomers?
Oxyhemoglobin is bright red, whereas deoxyhemoglobin is purple. Show that the difference in color can be accounted for qualitatively on the basis of high-spin and low-spin complexes.
Hydrated Mn2+ ions are practically colorless even though they possess five 3d electrons. Explain.
Which of the following hydrated cations are colorless: Fe2+(aq), Zn2+(aq), Cu+(aq), Cu2+(aq), V5+(aq), Ca2+(aq), Co2+(aq), Sc3+(aq), Pb2+(aq)? Explain your choice.
Aqueous solutions of CoCl2 are generally either light pink or blue. Low concentrations and low temperatures favor the pink form while high concentrations and high temperatures favor the blue form.
The compound 1,1,1-trifl uoroacetylacetone (tfa) is a bidentate ligand:It forms a tetrahedral complex with Be2+ and a square planar complex with Cu2+. Draw structures of these complex ions and
How many geometric isomers can the following square planar complex have?
[Pt(NH3)2Cl2] is found to exist in two geometric isomers designated I and II, which react with oxalic acid as follows:Comment on the structures of I and II.
The Kf for the complex ion formation between Pb2+ and EDTA4-
Manganese forms three low-spin complex ions with the cyanide ion with the formulas [Mn(CN)6]5-, [Mn(CN)6]4-, and [Mn(CN)6]3-. For each complex ion, determine the oxidation number of Mn and the number
Commercial silver-plating operations frequently use a solution containing the complex Ag(CN)2- ion. Because the formation constant (Kf) is quite large, this procedure ensures that the free Ag+
Draw qualitative diagrams for the crystal-field splitting in (a) A linear complex ion ML2, (b) A trigonalplanar complex ion ML3, and (c) A trigonal-bipyramidal complex ion ML5.
(a) The free Cu(I) ion is unstable in solution and has a tendency to disproportionate: Use the information in Table 19.1 to calculate the equilibrium constant for the reaction. (b) Based on your
Consider the following two ligand exchange reactions:(a) Which of the reactions should have a larger ÎS°? (b) Given that the Co-N bond strength is approximately the same in both
Copper is also known to exist in +3 oxidation state, which is believed to be involved in some biological electron transfer reactions. (a) Would you expect this oxidation state of copper to be stable?
The radius of a uranium-235 nucleus is about 7.0 × 10-3 pm. Calculate the density of the nucleus in g/cm3. (Assume the atomic mass is 235 amu.)
For each pair of isotopes listed, predict which one is less stable:(a)(b) (c)
In each pair of isotopes shown, indicate which one you would expect to be radioactive:(a)(b) (c) (d) (e)
Given that H(g) + H(g) → H2(g) ΔH° = -2436.4 kJ/mol calculate the change in mass (in kg) per mole of H2 formed.
Estimates show that the total energy output of the sun is 5 × 1026 J/s. What is the corresponding mass loss in kg/s of the sun?
Calculate the nuclear binding energy (in J) and the binding energy per nucleon of the following isotopes: (a) 73Li (7.01600 amu) and (b) 3517Cl(34.95952 amu).
Calculate the nuclear binding energy (in J) and the binding energy per nucleon of the following isotopes: (a) 42He (4.0026 amu) and (b) 18474W (183.9510 amu).
Fill in the blanks in the following radioactive decay series:
A radioactive substance undergoes decay as follows: Time (days) Mass (g) 0 ..................... 500 1 ..................... 389 2 ..................... 303 3 ..................... 236 4
The radioactive decay of Tl-206 to Pb-206 has a half-life of 4.20 min. Starting with 5.00 × 1022 atoms of Tl-206, calculate the number of such atoms left after 42.0 min.
A freshly isolated sample of 90Y was found to have an activity of 9.8 × 105 disintegrations per minute at 1:00 p.m. on December 3, 2003. At 2:15 p.m. on December 17, 2003, its activity was
Why do radioactive decay series obey first-order kinetics?
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